UI 
 

THE CALORIFIC POWER 
 OF FUELS. 
 
 FOUNDED ON 
 
 SCHEURER-KESTNER'S 
 POUVOIR CALORIFIQUE DES COMBUSTIBLES. 
 
 WITH THE ADDITION OF 
 
 A VERY FULL COLLECTION OF TABLES OF 
 
 HEATS OF COMBUSTION OF FUELS, 
 
 SOLID, LIQUID AND GASEOUS. 
 
 TO WHICH IS ALSO APPENDED 
 
 THE REPORT OF THE COMMITTEE ON BOILER TESTS 
 
 OF THE AMERICAN SOCIETY OF MECHANICAL 
 
 ENGINEERS (DECEMBER, 1897); TABLES 
 
 OF CONSTANTS USED. 
 
 BY 
 
 HERMAN x pOOLE, F.C.S., 
 
 Member of the Society of Chemical Industry ; the American Chemical Society. 
 
 the American Society of Civil Engineers ; the American 
 
 Society of Mechanical Engineers ; etc. 
 
 FIRST EDITION. 
 FIRST THOUSAND. 
 
 NEW YORK: 
 
 JOHN WILEY & SONS. 
 
 LONDON: CHAPMAN & HALL, LIMITED. 
 
 1898. 
 
Copyright, 1898, 
 
 BV 
 
 HERMAN POOLE. 
 
TO MY WIFE 
 
 THIS BOOK IS AFFECTIONATELY 
 DEDICATED. 
 
OF THK 
 
 UNIVERSITY 
 
 PREFACE. 
 
 THE books on fuels hitherto published in English, contain 
 only a few scattered facts regarding their calorific powers, how 
 they are obtained, and the practical use made of them. Quite 
 frequently these books are consulted for these facts, and the 
 information they do contain is utilized to its fullest extent. 
 It was thought that a book especially devoted to this subject 
 containing all the reliable data might be of interest, and in 
 furtherance of that idea this book is published. 
 
 The work commenced as a translation of M. Scheurer-Kest- 
 ner's "Pouvoir Calorifique des Combustibles "/ but changes be- 
 came necessary to adapt it to American methods and data, 
 and it was deemed advisable to simply use the skeleton of the 
 work and fill it in, as considered best. Even this skeleton has 
 hardly been preserved intact, as the arrangement of much of 
 the material has been changed, many portions omitted, many 
 new ones supplied, and in some of the original discussions the 
 argument has been so changed as to point nearly opposite to 
 that advocated by M. Scheurer-Kestner. 
 
 The work embraces only that portion of calorimetric de- 
 terminations having a bearing on fuel values. A concise 
 description is given of the leading calorimeters, those most 
 commonly used being described more fully than the others, and 
 some examples of working and calculations are added. 
 
 Coal being the principal fuel naturally receives more space 
 than any of the others, and most of the examples and calcula- 
 tions are based on results from this fuel. The other fuels are 
 
VI PREFA CE. 
 
 discussed briefly, some space being given to the heats of for- 
 mation of the different kinds of gas, and the advantages gained 
 by their use. A short account of theoretical flame tempera- 
 tures is given, with the methods of calculating and applying 
 the same. 
 
 The Report of the Committee on Boiler Tests, submitted 
 to the American Society of Mechanical Engineers, in Decem- 
 ber, 1897, is published in full, as are also several of the appen- 
 dices to the report. This report revises the old method of 
 1885, and gives the most recent methods of testing boilers 
 and reporting the same. 
 
 A set of tables of constants used in this and allied sub- 
 jects is given, and finally a collection of calorimetric and ana- 
 lytic data on all the kinds of fuel used. It is believed that these 
 tables are fuller and more complete than any previously pub- 
 lished in any language, and in collating them all available books 
 and periodicals have been freely used. In all instances where 
 the author was known, he has been credited with his results. 
 Of course in such a large amount some unreliable data may 
 have crept in, but all possible pains have been taken to exclude 
 any such. The list of periodicals, etc., consulted will be found 
 following the table of contents. 
 
 For help in the work, and especially the tabular matter, the 
 author is under obligations to many. Prominent among them 
 are Profs. R. C. Carpenter, E. E. Slosson, W. O. Atwater, 
 and D. S. Jacobus; and Messrs. William Kent, R. S. Hale, 
 F. L. Slocum, W. B. Day, and C. E. Emery. The Astor 
 Library and the Libraries of the American Society of Civil 
 Engineers and the American Society of Mechanical Engineers 
 were freely used, and much help obtained from the librarians. 
 Most of the cuts are 'from Scheurer-Kestner's book; a few 
 were taken from Lunge and Hurter's Alkali-Maker's Hand- 
 book; some from Groves and Thorpe's work on Fuels; a 
 few from the Reports of the American Society of Mechanical 
 Engineers; two from Dingler's Polytechnic Journal; one 
 
PREFA CE. vii 
 
 from the Scientific American Supplement ; and one from 
 Engineering News. 
 
 The work has been unavoidably delayed waiting for de- 
 sired data, some of which came too late to be used. 
 
 The author knows well that the book is far from perfect 
 or complete, but it is as near so as could be made with the 
 diverse kinds of material obtainable. Some errors, especially 
 in the tables, may be found, which he hopes to correct in the 
 future. 
 
 That it may be found of service and aid to others in their 
 work on fuels is the sincere wish of the author. 
 
 HERMAN POOLE. 
 
 NEW YORK, Jan. i, 1898. 
 
CONTENTS. 
 
 PAGE 
 
 PREFACE v 
 
 CONTENTS ix 
 
 AUTHORITIES xiii 
 
 CHAPTER I. 
 
 FUELS I 
 
 Definitions. Fuels. Calorific Value. Heat of Combustion. 
 Thermometers. Metastatic Thermometers. 
 
 CHAPTER II. 
 
 METHOD OF DETERMINING HEAT OF COMBUSTION 7 
 
 Methods Depending on the Composition. On the Reducing 
 Power. 
 
 CHAPTER III. 
 
 CALORIMETERS 12 
 
 Installation. Evaluation in Water. Correction for Readings. 
 
 CHAPTER IV. 
 
 CALORIMETERS WITH CONSTANT PRESSURE 20 
 
 Calorimeters using Air or Oxygen. Favre and Silbermann's. 
 Alexejew's. Fischer's. Thomsen's. Carpenter's. Schwack- 
 hofer's. W. Thompson's. Barrus's. Hartley and Junker's. 
 
 CHAPTER V. 
 
 CALORIMETERS WITH CONSTANT VOLUME 45 
 
 Relation of Constant Volume and Constant Pressure. An- 
 drews'. Berthelot's. Description. Working. Calculation. 
 
 ix 
 
X CONTENTS. 
 
 CHAPTER VI. 
 
 PAGE 
 
 MAHLER'S BOMB 57 
 
 Description. Working. Calculation. Examples ; Colza Oil, 
 Coal, Gas, Coke. Atwater's. Kroeker's. Walther-Hempel. 
 Witt's. 
 
 CHAPTER VII. 
 
 SOLID FUELS 75 
 
 Coal. Lignite. Peat. Coke. Charcoal. Wood. 
 
 CHAPTER VIII. 
 
 LIQUID FUELS 88 
 
 Shale Oils. Petroleum. 
 
 CHAPTER IX. 
 
 GASEOUS FUELS 92 
 
 Heat of Combustion from Analysis. Coal Gas. Gas of Gaso- 
 genes. Producer or Air Gas. Water and Mixed Gas. Natural 
 Gas. 
 
 CHAPTER X. 
 
 CALORIFIC POWER OF COAL BURNT UNDER A STEAM-BOILER 109 
 
 Distribution of Heat. Weight of Fuel. Sampling the Fuel. 
 Analysis of the Coal. Analysis of the Cinders. Duration of the 
 Test. The Water Evaporated. Temperature of the Steam. 
 Moisture of Steam. Corrections for Quality of Steam. Quality 
 of Superheated Steam. 
 
 CHAPTER XI. 
 
 CALORIFIC POWER OF COAL BURNT UNDER A STEAM-BOILER CON- 
 TINUED. AIR SUPPLIED AND WASTE GASES 125 
 
 Volume of Air Necessary to Combustion. Volume of Waste 
 gases by Analysis. Gas Sampler. Analysis of Gases. Calcula- 
 tion of Volume from Analysis. Calculation of Volume of Air 
 Supplied. Calculation of Weight of Waste Gases from Analysis. 
 Volume of Waste Gases by the Anemometer. Fletcher's Ane- 
 mometer. Segur's Differential Gauge. Hirn's Method. Dasym- 
 eter. Econometer. Gas Composimeter. Temperature of Waste 
 Gases. Pneumatic Pyrometer. Carbon in Smoke. 
 
CONTENTS. XI 
 
 CHAPTER XII. 
 
 PAGE 
 
 CALORIFIC POWER OF COAL BURNT UNDER A STEAM-BOILER CON- 
 TINUED. CALCULATION OF THE HEAT UNITS 159 
 
 Heat of Aqueous Vapor. Heat of Waste Gases. Heat of the 
 Temperature. Heat of the Hygroscopic and Combustion Water. 
 Calories of the Combustible Gases. Calories due to Soot. Dis- 
 tribution of Calories Loss. 
 
 FLAME AND FLAME TEMPERATURES 168 
 
 WEIGHT AND HEAT UNITS OF CARBON VAPOR 173 
 
 EVAPORATIVE POWER OF FUEL 174 
 
 APPENDIX. 
 
 REPORT OF THE COMMITTEE ON THE REVISION OF THE SOCIETY CODE 
 OF 1885, RELATIVE TO A STANDARD METHOD OF CONDUCTING STEAM- 
 BOILER TRIALS 177 
 
 Report of Committee. Rules for Conducting Trial. Form far 
 Report. 
 
 TABLES 198 
 
 FUEL TABLES 209 
 
 INDEX 249 
 
AUTHORITIES CONSULTED. 
 
 The following list contains the names of the different pub- 
 lications consulted to obtain data, especially for the tables. 
 Dates are not usually given, as in many cases the entire file 
 was used since 1868. 
 
 Alkali Reports, England. 
 
 American Engineer. 
 
 American Gas Light Journal. 
 
 American Manufacturer. 
 
 Annalen der Chemie und Physik. 
 
 Annales de Chimie et Physique. 
 
 Annales des Mines. 
 
 Australian Mining Standard. 
 
 Bayerisches Industrie und Gewerbeblatter. 
 
 Bell, Sir I. L., Chemical Phenomena of Iron-smelting. 
 
 Berichte der Deutscher Chemischer Gesellschaft. 
 
 Berthelot, Essai de Mecanique Chimique. 
 
 Berthier, Traite des Essais par la Voie seche. 
 
 Bulletin No. 21, U. S. Dept. Agriculture. 
 
 " University of Wyoming. 
 
 " de la Societe Industrielle de Mulhouse. 
 
 " de la Societe Chimique de Paris. 
 
 " de 1'Association des Proprietaires d'Appareils a Vapeur du 
 
 Nord de la France. 
 Chemical News. 
 Colliery Guardian. 
 
 Comptes Rendus de 1'Academie des Sciences. 
 Crookes and Rohrig, Metallurgy. 
 Dingler's Polytechnisches Journal. 
 Dufrenoy, Traite de Mineralogie. 
 Electrical Engineering. 
 
 xiii 
 
XIV AUTHORITIES CONSUL7*ED. 
 
 Engineer. 
 
 Engineering. 
 
 Engineering and Mining Journal. 
 
 Engineering Mechanics. 
 
 Engineering News. 
 
 Groves and Thorpe, Chemical Technology, Vol. I. 
 
 Gliickauf. 
 
 Ice and Refrigeration. 
 
 Iron Age. 
 
 Isherwood, B. M., Engineering Precedents. 
 
 " Researches in Steam Engineering. 
 Jahrbuch der K. K. Berg-Akademie. 
 
 " fiir Geologic. 
 
 Johnson, W. B., Report to Congress, U. S. A., 1844. 
 Journal American Chemical Society. 
 
 " Canadian Mining Institute. 
 
 " Chemical Society. 
 
 " Franklin Institute. 
 
 " Society of Chemical Industry. 
 
 " Imperial Institute. 
 
 Iron and Steel Institute. 
 
 " de 1'Eclairage au Gaz. 
 
 " des Usines a Gaz. 
 
 " du Gaz et de 1'Electricite. 
 
 " fiir Gasbeleuchtung. 
 
 " fiir Praktische Chemie. 
 
 " fiir Angewandte Chemie. 
 
 of Gas Lighting. 
 Kent, William, Pocket-book. 
 Le Genie Civil. 
 
 Memoires de la Societe des Ingenieurs Civils. 
 Mineral Industry, Vol. I. 
 
 Mineral Resources, U. S. A., various volumes,. 
 Mining Journal. 
 
 Morin and Tresca, Machines a Vapeur. 
 Oesterreichische Zeitschrift fiir Berg- und Hiittenwesen. 
 Peclet, Traite de la Chaleur. 
 Percy's Metallurgy, Fuels. 
 Philosophical Magazine. 
 Poly tech nisches Centralblatt. 
 Progressive Age. 
 
 Proceedings : Alabama Industrial and Scientific Society, 
 " American Gaslight Association. 
 
AUTHORITIES CONSULTED. XV 
 
 Proceedings: American Institute Mining Engineers. 
 " American Society of Civil Engineers. 
 
 " Institute of Mechanical Engineers. 
 
 " Institution of Civil Engineers. 
 
 Reports : British Alkali Commission. 
 
 " British Association of Gas Managers. 
 
 " Bureau of Mines, Canada. 
 
 " Department of Mines, New South Wales. 
 
 " Geological Survey, Ohio. 
 
 " Geological Survey, U. S. 
 
 South Lancashire and Cheshire Coal Association on Boilers 
 
 and Smoke Prevention, 1869. 
 Revista Minera. 
 Revue Scientifique et Industrielle. 
 
 Universelle des Mines. 
 Sanitary Engineer. 
 Scheerer, Lehrbuch der Metallurgie. 
 
 Scheurer-Kestner, Pouvoir Calorifique des Combustibles. 
 Science. 
 
 Ser, Traite de Physique Industrielle. 
 Stahl und Eisen. 
 Stevens Indicator. 
 Thomsen, Thermo-chemie. 
 Transactions Newcastle Chemical Society. 
 Ure's Dictionary. 
 
 United States Census Bulletin, 1890. 
 Williams, C. W. t Fuel, its Character and Economy. 
 Watt's Dictionary of Chemistry. 
 
 Witz, Traite theorique et pratique des moteurs a gaz. 
 Wurtz, Dictionnaire de Chimie. 
 Zeitschrift Physikalische Chemie. 
 
 " des Vereines Deutscher Ingenieure. 
 Zeitung Berg- und Hiittenwesen. 
 
CALORIFIC POWER OF FUELS 
 
 CHAPTER I. 
 INTRODUCTORY. 
 
 FUELS. 
 
 FUELS are those substances containing carbon, or carbon 
 and hydrogen, which are utilized for the heat they produce 
 upon union with oxygen. The products of this union, called 
 combustion, are carbonic acid or carbonic acid and water. 
 Many fuels, such as wood, peat, crude petroleum, etc., exist 
 naturally; others, such as coke, charcoal, coal-gas, etc., are 
 formed artificially. 
 
 The fuel par excellence to-day is coal. Improvements in 
 transportation allow deliveries at points more and more 
 remote from the mines, and the increasing demand, aided by 
 new and improved machinery, tends to lower the cost. New 
 locations are still being discovered, and the old ones are being 
 worked more thoroughly and completely. A large portion of 
 this book will be devoted to coal, other fuels being treated 
 incidentally; and such treatment is fitting, since it is the study 
 of coal to which the energies of physicists and engineers are 
 still principally devoted in their researches on the calorific 
 power of fuel. 
 
 For convenience of discussion the fuels will be divided 
 into three general heads: 
 
 Solid fuels coal, lignite, peat, coke, charcoal, and wood. 
 
2 CALORIFIC POWER OF FUELS. 
 
 Liquid fuels petroleum, shale oils, vegetable and animal 
 oils. 
 
 Gaseous fuels coal gas, producer gas, water gas, mixed 
 gas, natural gas. 
 
 CALORIFIC POWER OR HEAT VALUE. 
 
 The quantity of heat generated by the combustion of 
 a definite quantity of fuel in oxygen is called the calorific 
 power, heat value, or heat of combustion. 
 
 The expression calorific power or heat value has a wider 
 signification than heat of combustion. In the popular sense 
 the former ones apply to the measure of an industrial yield as 
 well as to the heat given off by the fuel during its complete 
 combustion. The expression heat of combustion, more nearly 
 correct from a scientific point of view, is applied, on the con- 
 trary, only to that quantity of heat generated by the substance 
 when completely burnt; that is to say, when the carbon and 
 hydrogen are completely changed to carbonic acid and water. 
 The unit adopted for these quantities of heat is the Calorie 
 and the British Thermal Unit. 
 
 The Calorie is the quantity of heat absorbed by the unit of 
 weight of pure water when its temperature is increased one 
 degree Centigrade. This unit is usually one gram or one 
 kilogram. When it represents the atomic or molecular 
 weight, it is called the atomic or molecular calorie, the gram 
 being taken as the^atomic unity. 
 
 The British Thermal Unit (B. T. U.) is the quantity of 
 heat absorbed by one unit (usually one pound) when its tem- 
 perature is increased one degree Fahrenheit. It is ^ of a 
 calorie. 
 
 A kilogram in burning generates n calories with a kilogram 
 as unit and the Centigrade scale ; a pound generates n calories 
 with a pound as unit and the Centigrade scale (W. Kent's 
 pound-calorie) ; or, whatever the weight taken, there will be 
 generated the same number of calories, using the same unit of 
 
INTROD UCTOR Y. 
 
 weight and the Centigrade scale. Hence to pass from the 
 Centigrade scale to the Fahrenheit scale multiply by the 
 factor 1.8, that being the ratio of the two scales. 
 
 In this work calories referred to the kilogram (kilo- 
 calories) will be used, and the calorie will be the quantity of 
 heat necessary to raise the temperature of that amount of pure 
 water one degree Centigrade. We will omit consideration of 
 the variations in specific heat of water; to consider these it 
 would be necessary to state that the initial temperature was 
 C. But, as remarked by Berthelot, " the calorie varies 
 only to a very slight degree if we take the water at a slightly 
 increased temperature at 15 or 20, for example; so that we 
 are accustomed to regard as constant the specific heat absorbed 
 by the water for each degree comprised in this interval of 
 temperature, thus simplifying the calculations." We may 
 lessen this little -error by referring the calorie to a litre of 
 water instead of a kilogram, that is, by measuring the water 
 instead of weighing it ; the weight of a litre of water diminish- 
 ing from its maximum density at 4 C., while its specific heat 
 gradually increases. The error of calculation is thus made 
 less than the error of experiment. 
 
 HEAT OF COMBUSTION. 
 
 When the fuel contains hydrogen, its heat of combustion 
 may be expressed in two ways. Hydrogen in burning pro- 
 duces water, and this water may be either condensed or in the 
 state of vapor. The same number does not apply to both 
 cases, since the vaporization of the water formed consumes 
 heat, which is not given up to the calorimetric bath. We 
 usually consider the heat of combustion, the result of the 
 experiment made under ordinary conditions, or when the 
 water is in the liquid state; this is the general acceptance of 
 the term heat of combustion. Some authors, however, prefer 
 to consider the water as vapor. 
 
 It is easy, however, to change from one system to the 
 
4 CALORIFIC POWER OF FUELS. 
 
 other. The heat of combustion of one kilogram of hydrogen 
 being 34500 calories,* and the water formed being liquid at 
 O C., a portion of the 34500 calories is used to vaporize the 
 water in the case where it is gaseous or considered as such. 
 
 Experiment has shown that the heat of vaporization of 
 water is expressed by the formula of Regnault, 
 
 606.5 + o- 305*> or 
 1091.7 -f- o.3O5(/ 32) for Fahrenheit degrees, 
 
 in which t represents the temperature of the water in the state 
 of vapor. Now one kilogram of hydrogen produces nine 
 kilograms of water. To keep these nine kilograms of water 
 in vapor, at 100 C. for example, there will be needed, by the 
 above formula, 637 calories per kilogram of water, or nine 
 times as much per kilogram of hydrogen, which is 5733 
 calories. These 5733 calories reduce to 5453 when the water 
 is considered as being at o C. instead of at 100 C. Deduct- 
 ing 5453 calories from 34500 calories representing the heat of 
 combustion of hydrogen, the water formed being condensed, 
 we obtain 29047, which number represents the heat of com- 
 bustion of hydrogen, the water being in the state of vapor 
 at o. We will call it, in round numbers, 29ioof calories, as 
 is done by several writers. 
 
 THERMOMETERS. 
 
 Before taking up the study of calorimeters, we must con- 
 sider the calorimetric thermometer, which is a most important 
 part of the apparatus employed. The reading of the ther- 
 mometer and the corrections are quite delicate and also very 
 important, the calculation of the heat of combustion depend- 
 ing principally on their accuracy. 
 
 In this work calorimetric questions relating to fuel only 
 will be considered; hence a description of ordinary ther- 
 
 * 62100 B. T. U. f 52380 B. T. U. 
 
 x>- 
 
INTRODUCTORY. 5 
 
 mometers and their manufacture will not be needed. They 
 are usually bought all finished, and should be obtained only 
 from reliable dealers. 
 
 Favre and Silbermann employed a thermometer of their 
 own design, divided into ^ degrees and graduated from 32 
 to o C. Each degree occupied about 0.3 inch. By means 
 of a cathetometer they read to pj--^ of a degree. Their calori- 
 metric bath of 2 litres capacity was subjected to at least 8 
 elevation in temperature, and the quantity of substance 
 necessary to use at times exceeded 2 i 2 
 
 grams. To lessen this amount of rise 
 in temperature and also the time of 
 combustion, they used longer thermo- 
 meters, with scales reading to -5-^ or '" 
 even to - Scheurer-Kestner used 
 
 a thermometer divided to -^ with his 
 
 j I I Q 
 
 Favre and Silbermann calorimeter. fl 7 
 
 Since then they have been used gener- 
 ally. Such thermometers are difficult 
 
 s 
 
 to work with, and require care in ma- 
 
 3 
 
 nipulation, and often a series of ther- I Lj 2 
 
 mometers or at least two with scales 
 
 I U o 
 in sequence are employed. If the 
 
 initial temperature of a calorimetric 
 bath is found a little above the highest 
 graduation on the first thermometer, 
 
 and if the rise in temperature of the FIG. I.-METASTATIC 
 
 THERMOMETER. 
 bath amounts to two degrees, we must 
 
 substitute the second one having for its lowest degree the 
 highest of the first. Besides the trouble of substitution, it 
 necessitates a correction for agreement of the degrees common 
 to the two instruments. To obviate this difficulty the 
 " metastatic " thermometer was invented by Walferdin and 
 described in the Comptes Rendus de r Academic des Sciences, 
 1840, p. 292, and 1842, p. 63. 
 
O CALORIFIC POWER OF FUELS. 
 
 The metastatic thermometer is a differential thermometer 
 with a variable scale. At will, a certain quantity of mercury 
 flows into the bulb. By this means we raise or lower the 
 degrees for which it may be used. Suppose an ordinary 
 thermometer graduated from o to 10, and left open at 
 the top at the loth degree. If we wish to use it between 12 
 and 14, heat it to 14, and a portion of mercury correspond- 
 ing to 4 escapes. Now, instead of showing a difference of 10 
 between o and 10, it will show this difference between 4 
 and 8, the original o having descended to 4. It will be 
 similar for temperatures of 10, 20, or 30, as desired. By 
 closing the thermometer at the top instead of leaving it open, 
 and blowing a bulb in the upper portion as overflow, the 
 conditions will remain the same. The thermometer has now 
 become metastatic. These thermometers are made by Baudin 
 of Paris, from whom full directions for use and corrections can 
 be obtained. 
 
 With all thermometers it is essential that the glass of the 
 bulb should be rather thin, or the thermometer will be " too 
 slow." The slightest difference in temperature must be 
 shown immediately by a movement of the mercurial column. 
 To test for sensibility, read the height of the column and then 
 place the hand on the bulb. If sufficiently sensitive the mer- 
 cury will descend quickly from the expansion of the glass and 
 afterwards rise. In thermometers divided to y^ this move- 
 ment should be immediate, and over several hundredths. 
 
 In ordinary calorimetric experiments the correction due to 
 length of the mercury column flowing out of the bulb may 
 be neglected for several reasons; the experiments should be 
 made in a room where the temperature is nearly the same as 
 that of the calorimetric bath, such correction would be of 
 very little consequence for a slight change of temperature, 
 and the experimenter should plunge the thermometer into the 
 bath as deep as is necessary to take the reading at the level 
 of the eye. 
 
CHAPTER II. 
 METHODS OF DETERMINING HEAT OF COMBUSTION. 
 
 THERE are two methods for determining tne heat of com- 
 bustion of substances one by calculation based on the 
 chemical composition, and the other by actual combustion in 
 a calorimeter. The first method may be considered under 
 two heads: that in which the units are calculated directly from 
 the composition, and that in which they are calculated from 
 the quantity of oxygen consumed during combustion in a 
 crucible. 
 
 CALCULATION FROM CHEMICAL COMPOSITION. 
 
 Dulong stated that the heat generated by a fuel during 
 combustion was equal to the sum of the possible heats gener- 
 ated by its component elements, less that portion of the hy- 
 drogen which might form water with the oxygen of the fuel. 
 
 His formula was 
 
 * = 8o8oC + 34500 H - , 
 or expressed in B. T. U.'s, 
 
 x = I4500C + 62 100 (H - -). 
 
 
 in which 
 
 x = the heat of combustion sought ; 
 8080 = the heat of combustion of carbon in calories ; 
 14500= " " " " " " " B. T. U. ; 
 
 34500= " " " " " hydrogen in calories; 
 
 62100 = " "^ " " " " " B. T. U. ; 
 
 7 
 
8 CALORIFIC POWER OF FUELS. 
 
 H = the quantity of hydrogen less that supposed to form 
 water with the oxygen. 
 
 Other authors and experimenters have tried to interpret 
 their results by a general formula with varying success. 
 Many of them by working on a certain number of coals from 
 a certain location work out a formula which applies to that 
 set of coals, but not as well to another set. A few of them 
 will be given. They all resemble Dulong's and are usually 
 only modifications of his original one. 
 
 The Verein Deutscher Ingenieure adopted the following: 
 
 x SiooC + 29000 (H -J + 25008 6oo, 
 
 in which allowance is made for the heat of combustion of 
 sulphur and the heat of the hygroscopic water. All the 
 coefficients are round numbers and that for hydrogen, 29000, 
 is the one in which the water is supposed to be as aqueous 
 vapor, all the water being considered as passing off in that 
 state. None of the other formulae uses this coefficient. 
 It gives rather low results. The question as to the advis- 
 ability of reckoning the heat due to sulphur is a debatable 
 one. In no case does it amount to more than a very small 
 per cent and can have but little effect on the total. 
 Balling gives as* -formula 
 
 x = 8o8oC + 34462 H - _ 6$2(E + 9 H) 
 
 
 
 to represent the actual occurrences in a steam-boiler fire work- 
 ing under a pressure of steam corresponding to 300 F. 
 
 Schwackhoefer made the following modification to allow 
 for the correction due to hygroscopic water: 
 
 x - 8o8oC + 34500 I H g- 1 - 637^. 
 
METHODS OF DETERMINING HEAT OF COMBUSTION. 9 
 
 Mahler formulated one based on the results of calorimetric 
 determination of the heat of combustion of 44 different kinds 
 
 81400 + 345QQH - 3000(0+ N) 
 100 
 
 or simplified, 
 
 x = IH.4C + 375H 3000; 
 or in B. T. U.'s, 
 
 x = 200.50 + 675 H 5400. 
 
 With the coals he examined he found a very close agree- 
 ment between the results calculated by this formula and 
 those observed. A similar but not equally close concordance 
 was found using the Dulong formula. With wood and lig. 
 nites the difference amounted to 2 per cent. His formula 
 applies also to other substances whose constituents are accu- 
 rately known. Cellulose, the heat of combustion of which 
 according to Berthelot is 4200 calories, by Mahler's formula 
 is 4264. 
 
 In summing up he says: '* From a scientific point of 
 view, in the present state of our knowledge on the subject, 
 we cannot give a general formula depending strictly on the 
 chemical composition which will give the calorific power of 
 combustibles, substances so complex and varied." 
 
 Lord and Haas in a paper read before the American Insti- 
 tute of Mining Engineers, Feb. 1897, state that in a series of 
 forty Pennsylvania and Ohio coals they found differences 
 varying from -)- 2.0 to 1.8 per cent between the calculated 
 and the observed results, and an average difference of o. 12 
 per cent. 
 
 In 1896 Bunte published some analyses and calorimetric 
 tests of gas-cokes, showing a difference of from -f- 0.04 to 
 1.2 per cent. 
 
IO CALORIFIC POWER OF FUELS. 
 
 Three elements enter into these cases, the analysis, the 
 calculation, and the combustion; all may be erroneous. As 
 the matter stands now the weight of error seems to be on the 
 side of the analysis, as our methods of analysis, especially in 
 water determinations, are not entirely satisfactory; yet it must 
 be confessed that some of the most recent analyses give a 
 basis trom which very close agreement can be calculated. 
 With such fuels as coke, charcoal, or anthracite, having but 
 little volatile matter, the results agree quite well, but with the 
 bituminous coals, asphalts, mineral oils, etc., which are so 
 very complex, the differences are greater.* In these the 
 actual proximate chemical constitution seems to make a differ- 
 ence. It may be safely stated, however, that for ordinary 
 industrial uses, in absence of the possibility of a calorimetric 
 test, and with coals having under 20 per cent of volatile 
 matter, a fairly accurate approximation may be arrived at by 
 calculation. 
 
 The great inducement that formerly existed in favor of 
 calculated results exists.no longer. I refer to the difficulty 
 of making a calorimetric test. These can be made now by 
 means of the modern apparatus, so simple and almost self- 
 regulating that the time consumed is but a small fraction of 
 that needed for an analysis, and the labor and care, hardly 
 anything in comparison. 
 
 If possible, by ^11 means have a calorimetric test. If not 
 possible, use the best analysis available. 
 
 CALCULATION FROM QUANTITY OF OXYGEN USED. 
 
 This is the litharge reduction test. It depends on 
 Welter's formula, which is based on the hypothesis that the 
 heat of combustion is proportional to the quantity of oxygen 
 consumed : 
 
 N = mP, 
 
 * Mahler's limit for Dulong's formula is O -f N > 15. 
 
METHODS OF DETERMINING HEAT OF COMBUSTION. II 
 
 in which N is the heat of combustion sought, m is the coeffi- 
 cient previously determined, and P is the weight of oxygen 
 necessary for the combustion of one kilogram of the substance. 
 Giving P the value resulting from the use of the equiva- 
 lents 1 6 for oxygen to burn 6 of carbon, and 8 for oxygen 
 to burn I of hydrogen we have 
 
 and the general formula becomes 
 
 N = Sm (- + H) = 26880 (- + H). 
 
 To use this method the combustible is mixed with an 
 excess of litharge and heated in a crucible. The button of 
 lead formed shows the amount of oxygen consumed, and from 
 this is deduced the heat by means of the formula. The heat 
 should be increased very slowly. Mitchell substituted white 
 lead for litharge and claimed to obtain uniform results. 
 
 This formula was recommended by Berthier, and has been 
 used since by a few others. It is faulty, as was shown by 
 some of Berthier's own determinations in which contradictory 
 results were obtained. Dr. Ure showed that no uniform re- 
 sults could be obtained using the same materials. Scheurer- 
 Kestner in 1892 showed that the formula not only gave erro- 
 neous results, but actually reversed the relation of combus- 
 tibles. In one case cited the heats actually obtained by a 
 calorimeter were 8813 and 8750, while by the litharge test 
 they were 7547 and 7977. The results were not only low, 
 but reversed the ratio. 
 
 This method is allowable only in cases where the crudest 
 approximations are desired and where no analyses or calori- 
 metric tests can possibly be made. 
 
CHAPTER III. 
 CALORIMETRY. 
 
 CALORIMETERS for rapid combustion are invariably com- 
 posed of a combustion-chamber and a calorimetric bath, 
 usually a cylinder, surrounding it and containing a known 
 quantity of water, the elevation in temperature of which is 
 measured. The combustion is made in oxygen, pure or 
 diluted. 
 
 Combustion-chambers are either under a constant pressure, 
 as in the calorimeters of Rumford, Favre and Silbermann, 
 etc. ; or with a constant volume, as in the calorimeters of 
 Andrews, Berthelot, etc. With solids the difference of results 
 obtained under constant volume and constant pressure is so 
 small that we shall not consider it. With gases, however, it 
 is different, and we will state under which conditions the 
 results have been obtained. 
 
 The first calorimetric experiments date from Lavoisier and 
 Laplace. In 1814 Count Rumford replaced the ice calorim- 
 eter of Lavoisier by an apparatus in which the heat devel- 
 oped during the combustion was absorbed by water. It was 
 some time after, 1858, that Favre and Silbermann discovered 
 the causes of the great errors of their predecessors, and pub- 
 lished methods for correcting some while avoiding others. 
 We owe to them, above all, the observation that, even when 
 supplied with pure oxygen, combustion may be only partial, 
 on account of the formation of combustible gases. They 
 determined that this occurs generally, and gave a method of 
 estimating the unburnt gases, so as to make allowances in the 
 calculation. 
 
 12 
 
CA L RIME TRY. I 3 
 
 Carbon, which, before their time, had given only 7624 
 calories to Laplace, 7386 to Clement-Desormes, 7915 to Des- 
 pretz, 7295 to Dulong, and 7678 to Andrews, yielded to F. 
 & S. 8081 after correction for carbonic oxide in the waste 
 gases. This number has since been increased to 8140 by the 
 latest determinations of Berthelot. Berthelot and Vielle have 
 shown that by using oxygen under pressure complete com- 
 bustion can be attained. 
 
 INSTALLATION OF APPARATUS. 
 
 The apparatus should be placed in a room free from 
 sudden changes in temperature and consequently protected 
 from direct sunlight. If it is not entirely protected from 
 solar radiation, the apparatus may be set up on the north 
 side and shaded from the direct midday sun by a screen. 
 
 The calorimeter cylinder with its accessories, as well as the 
 distilled water used, should remain in the room long enough 
 to acquire its proper temperature. The cylinder should be 
 protected as much as possible from radiation by envelopes 
 which vary according to circumstances. Favre and Silber- 
 mann used a cylinder with a double wall. The external one 
 was filled with water, and between this one and the cylinder 
 proper swan's down was packed. The upper part of the 
 cylinder also had a layer of thick paper covered with down 
 on the under side. 
 
 Berthelot states that the down is more troublesome than 
 useful, and that it may be omitted with advantage. The space 
 between the cylinder and its envelope forms a layer of air 
 which is an excellent non-conductor. In modern instruments 
 the down is replaced by a thick layer of felt. Berthelot even 
 omits this covering, stating that the great cause of loss of 
 heat was not from radiation, but due to evaporation produced 
 by the agitation of the water in contact with the air. He 
 surrounds his cylinder with a layer of air inside of the 
 envelope of water, and outside of all a layer of felt O.8 inch 
 thick. By this means external influence is much reduced. 
 
14 CALORIFIC POWER OF FUELS. 
 
 EVALUATION OF THE CALORIMETER IN WATER. 
 
 Before using a calorimeter its equivalent in water must be 
 determined; that is, we must calculate to what quantity of 
 water it corresponds in terms of specific heat. This is to 
 be added to the weight of water employed and includes the 
 combustion-chamber, cylinder, and the immersed pieces, 
 thermometer, supports, etc. 
 
 Below is given an example showing the calculation of the 
 value in water of a Favre and Silbermann's calorimeter: 
 
 Copper, 1145.651 grams at 0.09516 specific heat = 109.008 grams. 
 
 Platinum, 22.810 " "0.0324 " " = 0.706 
 
 Value in water of the chamber and accessories = 109.714 " 
 Thermometer, weight of glass immersed, 12 grams at 0.198 = 2.400 " 
 Mercury, 63 " " 0.332 = 2.070 
 
 Total equivalent of water 114.184 " 
 
 which added to the 2 kilograms of water in the bath makes a 
 total of 2114.184 grams of water. 
 
 The calorimetric weight for the Berthelot bomb at the 
 College of France in 1888 was 398.7 grams for bomb and 
 accessories. 
 
 The water value of the calorimeter used by Lord and Haas 
 at the Ohio State University, Columbus, O., was determined 
 as 465 grams. Mahler's apparatus had a water equivalent 
 of 481 grams. Still, it is better to determine this equivalent 
 by actual experiment, as we are not sure of the specific heat 
 of the metal of the bomb, which might, however, be deter- 
 mined by a sample taken from the original block of which it 
 was made. 
 
 Several methods may be employed for this. 
 
 When we use the calorimetric bomb, we burn in the obus, 
 using 2000 grams of water, a known quantity of a substance 
 of fixed composition, and of which the heat of combustion 
 is known, as sugar, or naphthalin. We then use less water 
 and burn a smaller quantity of the substance. If I gram of 
 substance was taken the first time, we may take 0.8 gram with 
 1800 grams of water the second time. We then have two 
 
CALORIMETRY. 
 
 equations, Itom which we eliminate the heat of combustion of 
 the substance and deduce thence the value in water of the 
 cylinder, etc. 
 
 This method, suggested by Berthelot, may be replaced by 
 the following, to which he gives the preference: 
 
 Pour into the calorimeter a certain quantity of warm 
 water, at 60 C. for instance. This water is previously con- 
 tained in a bottle, and the temperature is measured by a 
 thermometer placed inside. As control, operate first without 
 the bomb in the cylinder and afterwards with it in place. 
 
 One test of this kind gave Berthelot a value of 354 calories 
 for the bomb. The value deduced by calculation from specific 
 heat was 355.4. Below is the detailed calculation giving the 
 separate parts of the bomb. 
 
 Names of the Different Parts. 
 
 Soft Steel. 
 
 Platinum. 
 
 Brass. 
 
 Weight 
 m 
 Grams. 
 
 Value in 
 Water. 
 
 Weight 
 in 
 Grams. 
 
 Value in 
 Water. 
 
 Weight 
 in 
 Grams. 
 
 Value in 
 Water. 
 
 
 1709.7 
 221.2 
 II.7 
 
 187.61 
 24.28 
 1.28 
 
 728.8 
 528.8 
 
 23.63 
 17.15 
 
 20.0 
 3.97 
 
 108.9 
 
 1.86 
 0-37 
 
 10.13 
 
 
 
 Cone-screw and socket 
 
 
 
 Movable accessories serv- 
 ing for suspension and 
 
 
 
 33-0 
 
 1.07 
 
 
 802.7 
 
 88.08 
 
 
 
 
 
 
 
 2745-3 
 
 301.24 
 
 I2Q0.6 
 
 41.85 
 
 132.9 
 
 12.36 
 
 
 RECAPITULATION. 
 
 Metals Used. 
 
 Weight in 
 Grams. 
 
 Calculated 
 Value in Water. 
 
 Steel 
 
 27/1 e a 
 
 OOT 2J. 
 
 
 1290.6 
 
 4.1. 85 
 
 Brass (calorimeter and agitator omitted) 
 
 T-22 Q 
 
 12 36 
 
 
 
 
 
 4168 8 
 
 oce je 
 
 
 
 I.C.A 7 
 
 
 
 
16 CALORIFIC POWER OF FUELS, 
 
 CORRECTIONS FOR THE READINGS. 
 
 The corrections to be applied to thermometric readings, 
 besides those due to the thermometer itself, are of various 
 kinds, and naturally vary with the kind of calorimeter used. 
 Some, however, are common to all. 
 
 The correction relative to heating and cooling concerns all 
 calorimeters. Favre and Silbermann made this correction with 
 a coefficient previously determined, once for all, by a series 
 of experiments. For example, the coefficient that they found 
 for their calorimeter ( 0.0020225) represents the influence 
 of the external temperature through the envelopes and pack- 
 ings for one minute and one degree. 
 
 Instead of a coefficient of correction thus determined, 
 use preferably a system of correction devised by Regnault and 
 Pfaundler. This system is superior to the preceding, as it 
 allows consideration of all external conditions at the time of 
 the experiment. It is evident, for example, that the evapora- 
 tion of a liquid may vary in such proportions that a fixed 
 coefficient will not always represent it. 
 
 The system of Regnault and Pfaundler does not need 
 previous experiments nor a determined coefficient. It rests 
 on observation of the thermometer immersed in the bath a 
 few minutes before and after the experiment, or at the times 
 when external influence is at its minimum or maximum. 
 Knowing the value of these two kinds of influence, it is 
 easy to calculate it for the whole duration of the test. 
 
 It is well to continue the observations before combustion 
 for some five minutes. These five minutes should be pre- 
 ceded by at least ten minutes' immersion of the combustion 
 chamber with agitator, so as to establish equilibrium of tem- 
 perature between the cylinder and the water. 
 
 Suppose the initial correction corresponding to the first 
 period to be zero which is rare, it is true, but simplifies the 
 
CA L ORIME TRY. 1 7 
 
 demonstration and that the observations have given the fol- 
 lowing data: 
 
 Initial temperature of bath 18.460 
 
 After i minute 19.700 
 
 " 2 " 20.540 
 
 " 3 " 20.670 
 
 ' " 4 " 20.680 
 
 5 " 20.676 
 
 6 " 20.665 
 
 7 " 20.655 
 
 8 " ..' 20.640 
 
 " 9 ' 20.630 
 
 ' 10 " 20.620 
 
 The combustion once commenced is continued till after 
 the fourth minute and ends between the fourth and fifth 
 minutes, but the equilibrium of temperature between the bath 
 and the combustion-chamber is not established until the 
 eighth minute, the time when the variation due to difference 
 between them has become regular (0.010 per minute). 
 
 A table of corrections is formed as follows: 
 
 18.460 
 
 1st minute 19.700 -_ _. 
 
 Mean 19.080 Difference 0.620 
 2d " .... 20.540 _ 
 
 20.120 1. 660 
 
 3d " 20.670 , 
 
 20.605 2.145 
 
 4th " .... 20.680 
 
 20.675 2.215 
 
 5th " , 20.676 
 
 ' 20.678 2.218 
 
 6th " .... 20.665 
 
 7th t( 20.655 
 
 8th " 20.640 
 
 9th " .... 20.630 
 
 loth " 20.620 
 
1 8 CALORIFIC POWER OF FUELS. 
 
 The total elevation of temperature is 
 
 20.676 18.460 = 2.216, 
 
 and the correction is 
 
 20.676 20.620 = 0.056 for five minutes, 
 or 0.011 for one minute. 
 
 Then 
 
 2.216 : o.on = 0.620 : 0.0031 
 2.216 : o.on = 1. 660 : 0.0083 
 2.216 : o.on = 2.145 : 0.0107 
 2.216 : o.on = 2.215 ' o.ono 
 2.216 : o.on = 2.218 : o.ono 
 
 Total 0.0441 
 
 There is then 0.0441 to be added to the difference, 2.2 16, 
 increasing it to 2.260, which is the corrected difference of the 
 bath temperature, from which the heat of combustion of the 
 substance burnt in the calorimeter is calculated. 
 
 Regnault and Pfaundler's formula is 
 
 Atn = Ato + K(tn to) ; 
 in which 
 
 Atn = ascertained variation of temperature from the heat- 
 ing and cooling of the calorimeter for one 
 minute; 
 
 Ato = variation at the beginning; 
 
 t n t = loss or gain during the total time of the test; 
 n = number of minutes of test. 
 
 Using the above numbers, 
 o.on 
 
CALORIMETRY. 19 
 
 It will suffice, then, to find the total loss or gain to take 
 the sum of all the gains or losses calculated by means of the 
 coefficient K during the whole time of the experiment. 
 
 Thus, 
 
 0.620 X 0.00496 = 0.0031, 
 i. 660 X 0.00496 = 0.0083, 
 and so on. 
 
CHAPTER IV. 
 CALORIMETERS WITH CONSTANT PRESSURE, 
 
 THE first calorimeters were of constant pressure; that is, 
 the combustion was carried on at the atmospheric pressure or 
 very near it, and did not vary from the beginning to the end 
 of the experiment. Hence the modifications in the volume 
 of the gases before and after combustion exercised no influ- 
 ence on the observed results. 
 
 Rumford, in 1814, was the first who tried to correct 
 external influences. He employed a practical method which 
 has often been used since, and consists in giving the calo- 
 rimeter bath a temperature in the beginning of the test less 
 than that of the room, and allowing it at the close to attain 
 a temperature in the same proportion above that of the room. 
 His calorimetric apparatus was composed of a copper boiler 
 of several litres capacity, heated by an interior tube through 
 which passed the gaseous products of the combustion. The 
 combustible was burnt in a little burner placed under the 
 boiler, and the air used circulated around the heater before 
 passing to the burner, thus preventing any loss of caloric by 
 radiation. 
 
 Dulong in 1838 used oxygen, and obtained much superior 
 results. His calorimeter consisted of a rectangular copper 
 box, 25 centimetres (about 10 inches) deep, 7.5 centimetres 
 (2.9 inches) wide, and 10 centimetres (3.9 inches) long. It 
 was closed at the upper part by a cover with a mercury seal. 
 
 20 
 
FAVRE AND SILBERMANN'S CALORIMETER. 21 
 
 The oxygen passed into the calorimeter by a copper tube 
 opening at one of the sides of the box near the bottom. 
 The gases of combustion were drawn into a gas-holder. The 
 apparatus was enclosed in another likewise rectangular, in 
 which was put 1 1 litres (9$ quarts) of water. This was the 
 calorimetric cylinder. The water was kept in motion by an 
 
 agitator. 
 
 The unit chosen by Dulong was one gram of water whose 
 temperature was raised one degree. He corrected the tem- 
 perature observed, same as Rumford, but he also noticed 
 that this correction was correct only when the first period 
 was equal to the second. The results obtained by Dulong in 
 1838 were not published till after his death, in 1843. For 
 hydrogen and carbonic oxide they are but slightly different 
 from the most modern determinations. 
 
 CALORIMETER OF FAVRE AND SILBERMANN. 
 
 In 1852 Favre and Silbermann published their first 
 researches on the quantities of heat generated by chemical 
 action and described their calorimeter. 
 
 All rapid-combustion calorimeters and all with constant 
 pressure intended for solid bodies are copied more or less after 
 that of Favre and Silbermann. The principle and mode of 
 execution in their general lines are the same; the form in some 
 details or the material employed for the combustion-chamber 
 has been modified more or less; but the general apparatus 
 and accessories, as well as the method, have remained as 
 F. & S. left them. We will describe, then, this calorimeter 
 in its details, and outline the modifications made by other 
 experimenters. 
 
 The calorimeter called Favre and Silbermann's is composed 
 of three concentric copper cylinders (Fig. 2, B, C, D). 
 Cylinder B is the calorimeter cylinder; it is silver-plated and 
 polished on the inner surface so as to lessen its emitting 
 power; its capacity is a little over 2 litres (3^ pints), being 20 
 
 OF 
 
 UNIVERSITY 
 
22 
 
 CALORIFIC POWER OF FUELS. 
 
 centimetres (about 8 inches) high and 12 centimetres (4! 
 inches) in diameter. In the middle is placed the combustion- 
 chamber A (Figs. 2 and 3). 
 
 FIG. 2. FIG. 3. 
 
 FAVRE AND SILBERMANN CALORIMETER. 
 
 The combustion-chamber is of burnished gilt copper, and 
 is shown in Fig. 3. It is a slightly conical vessel, the large 
 opening in which receives a stopper from which is suspended 
 the burner made of a material suitable to that of the sub- 
 stance operated on. The stopper itself carries two tubes, m 
 and n, the first being an observation tube for the combustion, 
 and is surmounted by a mirror. M, which allows examination 
 during the burning. The mirror receives light by the tube 
 m, which is closed by an athermanous system of quartz, 
 alum, and glass. The other tube, , carries the jet for the 
 oxygen. Tube b is closed, or removed during the test with 
 coal, as it is of no use then. Tube c serves as the exit for the 
 waste gases of the combustion, which pass through the coil cc 
 (Fig. 2) before reaching the analytical apparatus. This coil 
 
FAVRE AND SILBERMANN'S CALORIMETER 
 
 is sufficient to cool the gas to the temperature of the bath. 
 Experimenters should solder the oxygen-jet to the stopper 
 so as to diminish the number of openings. It is also advan- 
 tageous to solder the coil to the cover. 
 
 Certain fuels with very smoky flames require the addition of 
 oxygen very near their surfaces. Scheurer- 
 Kestner and Meunier-Dollfus employed the 
 following arrangement (Fig. 4), a being the 
 platinum capsule; cc' , the platinum tube, 
 which at the part c fits tight in the mouth 
 of the oxygen-jet; b, b, b, platinum suspen- 
 sion-rods; d, fuel. 
 
 It is impossible to prevent the genera- 
 tion of more or less hydrocarbons and car- 
 bonic oxide. The weight of the hydrogen 
 and carbon is determined by causing the 
 gaseous products of combustion to pass 
 through an organic analysis tube, after re- 
 moving the water and carbonic acid. For 
 this purpose the exit-tube c (Fig. 3) is con- 
 nected by a caoutchouc tube with a Liebig apparatus, fol- 
 lowed by a U-tube of soda-lime. 
 
 The gas-current being rather rapid, an absorption appa- 
 ratus must be used, large and powerful enough to completely 
 free the gas from the carbonic acid and water before it reaches 
 the red-hot copper oxide. This is done by passing the gases 
 through another U-tube smaller than the preceding, and whose 
 weight should vary only a few milligrams. The gases thus 
 freed pass to the tube of hot copper oxide, where the com- 
 bustible gases are burnt to water and carbonic acid, which are 
 collected and weighed as usual. 
 
 Scheurer-Kestner and Meunier-Dollfus employed a plati- 
 num combustion-tube, and prefer soda-lime as absorbent for 
 the water after the conclusive experiments by Mulder.* 
 
 *Zeitschrift fiir analytische Chemie, I. 4. 
 
24 CALORIFIC P*OWER OF FUELS. 
 
 The coal for the experiment must be in pieces; if in 
 powder, the combustion is more difficult, unburnt gases 
 escaping in considerable quantities, so that it is rare to obtain 
 a complete combustion, and the cinders almost invariably 
 contain small quantities of coke. To determine these, the 
 capsule and tube are withdrawn from the combustion-cham- 
 ber, dried, and weighed. The coke and the little soot on the 
 sides of the capsule are burnt off by calcination in the air and 
 a new weighing made, giving the weight of the carbon and 
 cinder elements which must be considered in the corrections. 
 From half a gram to a gram of coal may be used. 
 
 When the combustion-chamber containing the weighed 
 substance is put into the calorimeter all the parts of the 
 apparatus are connected by caoutchouc joints and tested. 
 A slow current of oxygen* from a gas-holder is passed 
 through the apparatus. The combustible is ignited by a few 
 milligrams of burning charcoal, the joint 'in the tube being 
 broken for the moment, and immediately reconnected without 
 stopping the flow of oxygen. The little glass M allows inspec- 
 tion of the combustion, the intensity of which can be regulated 
 by the flow of oxygen from the gas-holder. The temperature 
 shown by the thermometer is recorded each minute to obtain 
 the data necessary for the correction spoken of above (pages 
 1 6 et seq.\ 
 
 To calculate the heat-units developed by the combustion 
 the following elements are needed : 
 
 1. Weight of the combustible used; 
 
 2. Weight of the carbon remaining in the cinders unburnt 
 or as black; 
 
 3. Weight of the cinders; 
 
 4. Weight of hydrogen escaped unburnt; 
 
 * To prepare the oxygen a copper flask of one litre capacity is used, in 
 which is placed some chlorate of potash, which is then heated by a gas 
 flame. The gaseous current is very regular, except towards the end, when 
 it may become tumultuous. The addition of a small percentage of black 
 oxide of manganese promotes the regularity of the gas generation. 
 
FAVRE AND SILBERMANN'S CALORIMETER. 2$ 
 
 5. Weight of carbon escaped unburnt in the gaseous 
 products ; 
 
 6. Elevation of temperature of calorimeter bath; 
 
 7. Correction for heating and cooling caused by external 
 influences on the calorimeter cylinder. 
 
 The combustion of the coal by this means is rarely com- 
 plete; there remain variable quantities of coke mixed with 
 the cinders formed. An uncertainty attends the calorimetric 
 value according as the combustion was slow or rapid, since 
 this small quantity of coke contains more or less hydrocarbons. 
 These differences, however, apply within very close limits, so 
 that no fear need be entertained of large errors therefrom. 
 When a coal, in pieces, has been burnt, there remains in the 
 -capsule only a few milligrams of coke or unburnt carbon. 
 From this we calculate the calorimetric value, using 8080 as 
 coefficient (heat of combustion of charcoal according to Favre 
 and Silbermann); and in using that coefficient the hydrogen 
 which may exist in the coke is naturally neglected, but this 
 cannot be prevented. The carbon and hydrogen of the com- 
 bustible gases which escaped combustion are transformed into 
 water and carbonic acid, and weighed as such. The hydrogen 
 is calculated as in the free state (coefficient 34500) and the 
 carbon as carbonic oxide (coefficient 2435). 
 
 It is evident that these are only approximations, since the 
 hydrogen is not disengaged in a free state, but as a hydro- 
 carbon; and its coefficient (34500) should be diminished by the 
 heat of formation of this compound, or, in other words, by the 
 heat of combustion of hydrogen and carbon. This correction, 
 however, is not possible; for neither the composition nor state 
 of molecular condensation of such hydrocarbon is known. 
 Similarly for the carbon, and its heat of combination in the 
 carbon compound. There are, then, some uncertainties, 
 but not of much importance, in the determination of the heat 
 of combustion of fuels uncertainties which the use of the 
 calorimetric bomb has entirely avoided. 
 
26 CALORIFIC POWER OF FUELS. 
 
 A complete test will now be described, giving all the cor- 
 rections. 
 
 Suppose one gram of dried coal in fragments is used. 
 After combustion in the calorimeter, weigh the capsule con- 
 taining the cinders. 
 
 Cinders after combustion o. 1 10 gram* 
 
 " " calcination in the air o. 100 " 
 
 Unburnt carbon remaining in cinders o.oio " 
 
 Then 
 
 Coal used, dried at 100 C i.ooo gram. 
 
 Cinders. . . o. 100 " 
 
 Pure coal (cinders out).. 0.900 
 
 Carbon not burnt during the experiment., o.oio 
 
 There was collected from the combustion of the hydro- 
 carbons and the carbonic oxide o. 10 gram of carbonic acid, 
 corresponding to 0.006 of carbonic oxide (molecular ratio 
 ii 17); also o.oio gram of water, corresponding to o.oon 
 gram hydrogen (molecular ratio 9 : i). 
 
 Increase of temperature of the bath 3.702 
 
 Correction 0.020 
 
 Total increase". 3. 722 
 
 Calorimeter equiv. in water 2.114 kilos * and 3.722 X 2.114 =7.8683 
 
 Unburnt carbon o.oio X 8.o8ocal. = 0.0808 
 
 Carbonic oxide 0.006 X 2.403 " =0.0144 
 
 Hydrogen o.oon X 34- 500 " = 0.0383 
 
 Total calories from 0.900 gram coal completely burnt = 8.0018 
 
 I gram pure coal = 8.891 calories, 
 I kilogram pure coal = 8891 calories, or 
 i pound " " = 16003.8 B. T. U. 
 
 * 2000 grams of water -}- 114 grams for value in water of calorimeter and 
 accessories. 
 
FAVRE AND SILBERMANN'S CALORIMETER. 2J 
 
 In this example the corrections are not very important, 
 since they do not exceed one-half per cent. These are the 
 ordinary conditions when the coal used is in pieces. With 
 pulverized coal, on the contrary, the quantity of unburnt 
 carbon and of combustible gases increases considerably and 
 renders results less certain. The oppor- 
 tunity we have to weigh the cinders of 
 each test obviates pulverization of the coal 
 to obtain an average sample of the cinders. 
 
 Favre and Silbermann's calorimeter has 
 been modified by Berthelot in several par- 
 ticulars.* He has happily modified the 
 agitator and given it a coiled form, as 
 shown in Fig. 5, a detailed description of 
 which is given in his Essai de Me'canique 
 Chimique, p. 145. 
 
 This agitator has the advantage over 
 the old one of more completely mixing 
 the water, with less force, and without 
 accelerating evaporation. Fig. 5 shows 
 it placed in the middle of the calorimeter. 
 
 FlG * 5 * 
 
 He has also replaced the gold-plated copper combustion- 
 chamber by the glass apparatus which Alexejew used for 
 combustibles. 
 
 *The F. & S. calorimeter with all accessories and an agitator (not me- 
 chanical) costs about 500 francs ($100.00); with mechanical agitator arranged 
 for a laboratory turbine or dynamo the cost is about 600 francs ($120.00). 
 Berthelot's calorimetric bomb of platinum, enamelled inside and not 
 double, costs no more, and is much preferable. A single operator can 
 handle it, while the F. & S. apparatus requires two. 
 
 Nevertheless, the manner of working the F. & S. calorimeter is de- 
 scribed in detail, because its use fs surrounded by conditions easily realized 
 in all countries. The calorimetric bomb requires oxygen compressed to 25 
 atmospheres, which cannot be obtained everywhere. 
 
28 
 
 CALORIFIC POWER OF FUELS. 
 
 ALEXEJEW S CALORIMETER. 
 
 The apparatus used by Alexejew was composed of a glass 
 combustion-chamber A (Fig. 6), in which he burnt the coal 
 
 previously reduced to fragments. 
 These fragments were placed on a 
 platinum grating in the centre of 
 the chamber. The fuel was kindled 
 by means of a platinum sponge 
 placed over it, on which impinged 
 a jet of hydrogen from the gas- 
 holder My opening at c, correction 
 for which is of course made in the 
 calculation. The grating contain- 
 ing the fuel was suspended from 
 the glass rod a. As soon as the 
 combustion was started the current 
 of hydrogen was cut off by the cock 
 /, and the oxygen allowed to flow 
 in through b, the waste gases pass- 
 ing out through the coil. If the 
 combustion was interrupted, it was 
 rekindled by the hydrogen and 
 
 platinum sponge. The hydrogen used was calculated in grams 
 and multiplied by 34500. The number of calories thus ob- 
 tained was deducted from that calculated from the rise in 
 temperature of the bath. According to Alexejew, the im- 
 portance of this correction never exceeded one-half per cent, 
 and he never had to rekindle the fuel. 
 
 Alexejew did not determine the unburnt gases, as experi- 
 ence showed they never exceeded 0.35 per cent. It is im- 
 possible, however, to determine the hydrogen of the hydro- 
 carbons if desired, as these would be mixed with the hydrogen 
 used for kindling-, part of which may escape combustion. 
 The kindling with hydrogen might, however, be replaced by 
 that with carbon, as in the F. & S. apparatus. 
 
 FIG. 6. ALEXEJEW CALORIM- 
 ETER. 
 
FISCHER ' S CA L ORIME TER. 
 
 2 9 
 
 Burning the fuel on a grating renders it impossible to 
 weigh the cinders, and this inconvenience is of more impor- 
 tance as the coal is used in pieces. The use of pastilles is not 
 possible, as they splinter in burning. 
 
 The calorimeter contained 2500 grams (5.511 Ibs.) of 
 water, a quantity somewhat larger than that usually employed, 
 and which is based on the sensibility of the thermometer. 
 To attain the same degree of precision it was necessary to use 
 larger samples of fuel or else have more delicate thermometers. 
 The water was kept in motion by the coil-agitator. 
 
 
 FISCHER S CALORIMETER. 
 
 Fischer made a combustion-chamber of silver 0.940 fine, 
 so that it would be less easily attacked 
 by sulphur, from which the gaseous pro- 
 ducts of coal are rarely free. He drew 
 off the waste gases at the bottom of the 
 apparatus (Fig. 7), thus avoiding the in- 
 convenience of exit-tubes in the cover 
 of the combustion-chamber. The coot- 
 ling coil was replaced by a flattened 
 pipe of a certain size. A represents 
 the combustion-chamber. The oxygen, 
 purified by passing over potash and 
 then dried, arrived by the tube a fast- 
 ened in the tube of the cover by a 
 caoutchouc joint, and passed by means 
 of the platinum tube r into a crucible 
 z of the same metal, containing one 
 gram of the fuel. The crucible was 
 covered by a grating, which became 
 red-hot towards the end of the opera- 
 tion. This was intended to burn the 
 waste gases, and the black deposited at the beginning. The 
 gases flowed out at z, and after having encircled the outside 
 
 FIG. 7. FISCHER'S CAL- 
 ORIMETER. 
 
30 CALORIFIC POWER OF FUELS. 
 
 of the crucible escaped at b. The thermometer / showed 
 whether the temperature of the gases was the same as that 
 of the bath. 
 
 The calorimetric bath contained 1500 grams (3.3 Ibs.) of 
 water, and was protected against external influences by a 
 wood casing, while the space C was filled with glass wool; 
 but this is not necessary, n is a brass cover which may be 
 dispensed with. The thermometer T is the calorimetric 
 thermometer; m is an agitator moved by the string o. The 
 value in water of the one used by Fischer was 113.5 calories. 
 The coal was dried in nitrogen. The carbonic acid and the 
 unburnt carbon were determined. 
 
 THOMSEN'S CALORIMETER. 
 
 This calorimeter was designed especially for tests of gases 
 and vapors. It is not adapted to tests of solid fuels. It 
 
 consisted (Fig. 8) of a calorimetric 
 bath of thin brass, with a capacity 
 of some 3 litres (195 cubic inches), 
 protected from radiation by a cylin- 
 drical ebonite envelope ; and a plati- 
 num balloon of half a litre (32.5 
 cubic inches) capacity, in which the 
 gases were burnt, being delivered 
 through the opening at the bottom. 
 The waste gases passed off 
 through a coil, and a mechanical 
 agitator kept the water in circula- 
 
 ' FIG. 8. THOMSEN CALO- tion. 
 
 RIMETER. The dried gas was delivered 
 
 with perfect regularity from a mercury gas-holder, sufficient 
 air or oxygen being added to render it free-burning, and 
 enough oxygen was supplied to insure perfect combustion. 
 This he attained by always having 40 to 50 per cent in the 
 
CARPENTER'S CALORIMETER. 31 
 
 waste gases. The gases passed off through a carbonic acid 
 absorbing apparatus. 
 
 To reduce to the minimum, or entirely suppress, the cor- 
 rection for temperature he regulated his gas-flow so that the 
 temperature was as much higher than the air at the close of 
 the experiment as it was lower at the beginning. This he 
 easily did by means of his hydrogen supply. If a liquid was 
 tested, it was vaporized and burnt in a specially devised 
 burner which allowed complete combustion of almost all com- 
 pounds not having too high a boiling-point. If too high for 
 heat vaporization, they were carried along by a current of air, 
 oxygen, or hydrogen, as seemed best adapted. 
 
 The water of the calorimeter being weighed, the lower 
 portion was closed with a rubber stopper and by means of an 
 aspirator a pressure of 8 to 12 inches of water was put on the 
 apparatus to test the joints. When ready, the temperature 
 of the bath and the air was noted for some minutes, the gas- 
 holder reading taken, the burner placed in position, and the 
 test commenced. The depression produced by the aspirator 
 was about 0.4 inch during the whole test. The regularity of 
 the working was shown by a gauge registering the pressure. 
 When the temperature had reached the desired point the gas 
 and electric current were shut off, the burner removed, and 
 the opening closed again. The aspirator was used to draw 
 dry air, freed from CO a , through the apparatus to insure 
 removal of all waste gases. The apparatus was then allowed 
 to rest, taking the temperature at short intervals for fifteen 
 minutes. He then had all the data required. 
 
 CARPENTER'S CALORIMETER. 
 
 Prof. R. C. Carpenter devised a calorimeter especially for 
 coal determinations, which is a modification or extension of 
 Thomsen's. He has used it considerably in connection with 
 work he has been engaged on, and the results credited to him 
 in the tables at the end of the book were obtained with it. 
 
32 CALORIFIC POWER OF FUELS. 
 
 Fig. 9 is a sectional view of his apparatus. It consists of 
 a combustion-cylinder, 15, with a removable bottom, 17, 
 
 FIG. 9. CARPENTER CALORIMETER. 
 
 through which passes the tube, 23, to supply oxygen, and also 
 the wires, 26 and 27, to furnish electricity for the igniter. 
 It also supports the asbestos combustion-dishes, 22, used for 
 
CARPENTER'S CALORIMETER. 33 
 
 holding the fuel. At its top is a silver mirror, 38, to deflect 
 the heat. The plug is made of alternate layers of asbestos 
 and vulcanite. The products of combustion pass off through 
 the spiral tube, 28, 29, 30, 31, which is connected with the 
 small chamber, 39, attached to the outer case of the instru- 
 ment. This chamber has a pressure-gauge, 40, and a small 
 pinhole outlet, 41. Outside the chamber is the calorimetric 
 bath, i, which is connected with an open glass gauge, 9, 10. 
 Above the water is a diaphragm, 12, used to adjust the level. 
 
 The calorimeter h'as an outer nickel-plated case, polished 
 on the inside. The bath holds about 5 pounds of water, and 
 uses about 2 grams of coal at a time. It is thus considerably 
 larger than the bomb, and the charge being larger the time 
 consumed by the test is longer, being some ten minutes for 
 each gram burnt. The entire outside dimensions of the case 
 are 9^ inches high and 6 inches diameter. 
 
 In using the apparatus the coal is ground to a powder in a 
 mill or mortar. The asbestos cup is heated to burn off all 
 organic matter and weighed. The sample is then placed in 
 it, and the whole weighed again. This gives the weight of 
 the coal used. Place it in the combustion-chamber, raise the 
 platinum igniting wire above the coal, make the connections 
 with the battery, and as soon as the heat generated causes the 
 water to rise in the glass tube turn on the oxygen, and by 
 pulling down the wires kindle the coal. At this instant the 
 reading on the glass scale must be taken. 
 
 By means of the glasses 33, 34, and 36 watch the 
 progress of the combustion, and as soon as finished take the 
 scale-reading and the time. The difference between this 
 scale-reading and the one previously made is the " actual " 
 scale-reading. 
 
 To correct for radiation, allow the apparatus to stand with 
 the oxygen shut off for a length of time equal to that of the 
 combustion, and take the scale-reading and the time. The 
 
34 CALORIFIC POWER OF FUELS. 
 
 difference between this and the " actual " reading is to be 
 added to the " actual " for the " corrected " reading. 
 
 Now, by inspection of the calibration-curve previously 
 prepared, at the point corresponding to the corrected scale- 
 reading will be found the B. T. U.'s for the quantity burnt. 
 The ash is determined by weighing the asbestos cup after the 
 combustion. 
 
 The following shows all the calculation needed : 
 
 Weight of crucible (asbestos cup) .... 1.269 grams. 
 
 and coal 3.017 " 
 
 " ash.. 1.567 " 
 
 " " combustibles I-45O " 
 
 ' ash 0.297 
 
 " coal 1.747 " 
 
 1.747 grams X 0.002205 = 0.003852 pounds. 
 
 First scale-reading 3.90 inches; time 2 hrs. 55 m. 
 
 Second" " 14.70 " " 3 " 20" 
 
 Third " " 14.30 " ll 3 " 45 " 
 
 "Actual" scale-reading. 14.70 3.90= 10.80 inches. 
 
 Radiation correction 14.70 14.30= .40 " 
 
 Corrected reading 11.20 " 
 
 On the calibration-sheet 11.2 corresponds to 46.25 
 B. T. U.'s, and 46.25 B. T. U. -r- 0.003852 = 12000 B. T. U. 
 per pound. 
 
 All air must be removed from the water in the bath, 
 the apparatus must work at a constant pressure, and the 
 pressure for which it is calibrated. A pressure of 10 inches 
 of water has been found satisfactory. Complete combustion 
 is always attained in the asbestos cups. 
 
 It will be seen that the use of thermometers is obviated, 
 and also all corrections but one. The apparatus is intended 
 
SCHWA CKHOFER 'S CALORIME TER. 
 
 35 
 
 for ordinary every-day work, and will give good comparative 
 results when used according to directions, which must be 
 implicitly followed. The amount of calculation is reduced to 
 a minimum, and there are no delicate parts requiring extra 
 care and adjustment. For the purpose intended, it seems an 
 advance over the others previously used, which could never 
 give more faint approximations to correct results. 
 
 SCHWACKHOFER S CALORIMETER. 
 
 In 1884 Schwackhofer published calorimetric researches 
 on different kinds of coal, using a calorimeter in which he made 
 
 FIG. io. SCHWACKHOFER CALORIMETER. 
 
 several modifications intended to render it specially applicable 
 to such fuel. 
 
 He considered it advisable to use as much as five or six 
 grams of coal, which is six times that generally used. He 
 burnt at the same time and under definite conditions, shown 
 
36 CALORIFIC POWER OF FUELS. 
 
 in the sketch (Fig. 10), a certain quantity of sugar-charcoal, 
 the combustion of which was intended to accelerate and com- 
 plete that of the coal tested. 
 
 In the figure (Fig. i<S)ab represents the combustion-cham- 
 ber, c the calorimetric bath. Minor details of accessories, en- 
 velopes, regulators, etc., are omitted. The burner proper is of 
 platinum and of two pieces, a and b, superimposed, the coal 
 being placed in the lower portion, the sugar-charcoal in the 
 upper one. All pieces of the burner may be removed for the 
 introduction of the coal and for cleaning. The two combus- 
 tibles rest on perforated plates of platinum, in which the per- 
 forations, made by a special machine, are so small that light 
 can hardly pass through, and from which the cinders can be 
 completely removed ; the holes in the upper one are slightly 
 larger than those of the lower. The oxygen enters through 
 three tubes, e, f, g. Tubes g and m pass outside the bath, and 
 carry mirrors to allow inspection during the burning. The 
 waste gases pass off at the bottom through a coil n, and are 
 collected in H. This vessel is simply to detect smoking, he 
 having found that it happened only when the pressure was di- 
 minished at the burner, and that it could be stopped by a rein- 
 statement of the normal pressure. / represents an aspirator, in 
 which are collected the waste gases. Another one, not shown 
 in the sketch, serves to contain the gas analyzed. Both are 
 filled with waters-covered with a film of oil. The oxygen 
 passes through a jar s filled with soda-lime, a bottle o fur- 
 nished with a thermometer, a cock t as regulator of the flow, 
 and one or more wash-bottles q containing sulphuric acid. 
 
 The calorimeter-chamber c contains 5200 cc. (4.6 qts.) of 
 water. 5 or 6 grams (77 to 92. 5 grains) of coal were used, with 
 2 to 4 grams (3 1 to 62 grains) of sugar-carbon of a known 
 calorific value. The temperature of the bath rose about 10 
 C., and the experiment generally lasted an hour. 
 
 The sugar-carbon was first kindled in the upper part of the 
 burner, the under portion burning first. From this sparks 
 
W. THOMPSON'S CALORIMETER. 37 
 
 were thrown to the coal, and it soon kindled. The oxygen 
 flowed in by g and e. When combustion was well under way 
 and had reached the lower portions of the coal, g was shut off 
 and /opened. 
 
 Schwackhofer obtained complete combustion of the sugar- 
 carbon and coal, with no formation of black, and no residue of 
 coke. 
 
 The gaseous product of the combustion was generally of 
 the following composition : 
 
 Carbonic acid 50 to 60 percent; 
 
 Carbonic oxide 1.2 to 0.3 " " 
 
 Oxygen 10 to 15 " " 
 
 Nitrogen 30 to 40 " " 
 
 arising principally from the fact that to keep up the normal 
 pressure the combustion-chamber was in communication with 
 the open air. The cinders were weighed after each test. 
 
 This apparatus should give exact results, but its use is 
 complicated. The long duration of the test requires impor- 
 tant corrections for influence of external heat, and it needs 
 several thermometers. 
 
 w. THOMPSON'S CALORIMETER. 
 
 W. Thompson devised a calorimeter in which the com- 
 bustion is started by a jet of oxygen, but the waste gases in- 
 stead of passing through a coil bubble up through the water 
 of the calorimetric bath. In this apparatus the uncombined 
 gases are naturally neglected. (See Fig. n.) It is an appa- 
 ratus, as the inventor says, not intended for scientific re- 
 searches, but for handy use of mechanics or " for popular use." 
 
 a is a galvanized-iron gas-holder containing oxygen ; b, a 
 stop-cock regulating the flow of water to this holder; d, stop- 
 cock for gas ; ^, rubber tube ; /, level-gauge ; g> pressure- 
 gauge; /z, bell-glass covering the platinum crucible k, in which 
 the coal is burnt ; / is a support of earthenware suspended 
 
35 CALORIFIC POWER OF FUELS. 
 
 from the bell-glass by metal springs, and intended to insulate 
 the crucible and prevent too quick cooling ; m is a glass jar 
 containing 2000 grams (4.4 Ibs.) of water, forming the calori- 
 metric bath. Water cannot enter the bell h while the cocky 
 
 FIG. ii. W. THOMPSON CALORIMETER. 
 
 is closed, and it is opened only when the pressure in the 
 gas-holder is sufficient ; n is a glass jar filled with water and 
 surrounding the calorimetric jar, and/ is the agitator. 
 
 One gram of fuel is put into the crucible, and on this is 
 placed a small cotton wick impregnated with bichromate of 
 potash. This is lighted at the instant of putting into the jar, 
 and its combustion* .aided by the oxygen kindles the fuel. 
 
 This is an imperfect apparatus, and will give in most cases 
 only unsatisfactory results. Still it is in rather common use 
 in the shops of England, where it serves principally as a com- 
 parative measure, the errors being considered constant. 
 
 BARRUS'S CALORIMETER. 
 
 The Barrus calorimeter is a modification of the one just 
 mentioned. While it requires considerable care in using to 
 get correct results, yet it is one of the simplest and most in- 
 expensive. 
 
BARRUS'S CALORIMETER. 
 
 39 
 
 As described by Mr. Barrus, "it consists of a glass beaker 
 (Fig. 12) 5 inches in diameter and n inches high, which 
 can be obtained of most dealers in 
 chemical apparatus. The combus- 
 tion-chamber is of special form, and 
 consists of a glass bell having a 
 notched rib around the lower edge 
 and a head just above the top, with 
 a tube projecting a considerable dis- 
 tance above the upper end. The 
 bell is 2\ inches inside diameter, 5^ 
 inches high, and the tube above is f 
 inch inside diameter and extends 
 beyond the bell a distance of 9 
 inches. The base consists of a cir- 
 cular plate of brass 4 inches in diam- 
 eter, with three clips fastened on 
 the upper side for holding down 
 the combustion-chamber. The base 
 is perforated, and the under side 
 has three pieces of cork attached, 
 which serve as feet. To the centre 
 of the upper side of the plate is attached a cup for holding 
 the platinum crucible in which the coal is burned. To the 
 upper end of the bell, beneath the head, a hood is attached 
 made of wire gauze, which serves to intercept the rising 
 bubbles of gas and retard their escape from the water. The 
 top of the tube is fitted with a cork, and through this is 
 inserted a small glass tube which carries the oxygen to the 
 lower part of the combustion-chamber. This tube is movable 
 up and down, and to some extent sideways, so as to direct 
 the current of oxygen to any part of the crucible and to 
 adjust it to a proper distance from the burning coal." 
 
 The method of working it can be easily seen from the 
 description and cut. In burning very smoky coals he mixes 
 
 FIG. 12. BARRUS CALORIM- 
 ETER. 
 
4O CALORIFIC POWER OF FUELS. 
 
 them with a proportion of non-smoking coal of known calo- 
 rific value, and when anthracite or coke is burnt he mixes it 
 with a small portion of bituminous coal. In Mr. Barrus's 
 hands very satisfactory results have been obtained. 
 
 HARTLEY AND JUNKER'S CALORIMETER. 
 
 Hartley's calorimeter is an apparatus of constant pressure 
 and continued combustion. The gas measured by a meter is 
 burnt in a Bunsen burner surrounded by a cylindrical copper 
 
 /I 
 
 FIG. 13. JUNKER CALORIMETER. 
 
 vessel filled with water, which is constantly renewed. The 
 flow of liquid is such as to avoid much heating and time suf- 
 ficient is used to increase the temperature so as to have a good 
 thermometric observation. The volume or weight of the water 
 is determined at such intervals and the thermometric readings 
 taken often enough to obtain an average. 
 
JUNKER'S CALORIMETER 41 
 
 Hugo Junker's modification of the apparatus rendered it 
 more exact. It has been used for some time in Germany 
 and in the United States. It is composed (Fig. 13) of a 
 gas-meter a, preceded by a very sensitive regulator b. On 
 leaving the meter the gas passes to a Bunsen burner c. The 
 products of combustion give up their heat to a calorimetric 
 tube d, through which regularly flows a stream of water. The 
 temperature of the gases is regulated by means of a thermom- 
 eter e. In order to keep the flow of water as regular as pos- 
 sible, it flows from the supply-tube g into a small reservoir 
 kept at a constant level governed by the tube h. The water 
 passes through i to the calorimeter and escapes at k, run- 
 ning into the glass in which it is measured or weighed. The 
 graduated tube / is to catch the condensed water from the 
 interior of the calorimeter. The thermometer m shows the 
 heat of the escaping water, and n that of the water enter- 
 ing the calorimeter. 
 
 To calculate the calories generated during the combustion 
 proceed as follows: 
 
 Measure the quantity of water which runs through it in 
 one minute, take the temperature of the two thermometers, 
 and note the flow of gas. The heat of combustion per cubic 
 metre of burnt gas is obtained by multiplying the volume of 
 water flowing per minute by the difference of the two temper- 
 atures and dividing the product by the gas volume burnt per 
 minute. 
 
 Thus : 
 
 Volume of water flowing per minute... . 902.3 cc. 
 
 " " gas burnt per minute ...... 2500.0 cc. 
 
 Temperature at inlet ................. I3.IC. 
 
 " outlet ................ 27.5 C. 
 
 Q == 902.3 X (27 5 -.3.1) 
 
42 CALORIFIC POWER OF FUELS. 
 
 The gas tested has a value of 5 196 calories per cubic metre. 
 
 Since the calorie is 3.968 times the B. T. U., and the 
 
 cubic metre is 35.316 times the cubic foot, multiplying 
 
 the calories per cubic metre by = 0.11235 will give 
 
 B. T. U.'s per cubic foot. 
 Multiplying, then, 
 
 5 196 X o. 1 1235 = 583.8 B. T. U.'s per cubic foot. 
 
 The above example considered the volume of the water. 
 It is sometimes advisable to consider the weight instead. The 
 following example illustrates this: 
 
 Weight of water used during the test 2000 grams. 
 
 Volume of gas burnt 7.23 litres. 
 
 Temperature at inlet 14.4 C. 
 
 *' outlet 36.5 C. 
 
 Then 
 
 2000 X (36.5 - 14.4) 
 Q = - = 6102 calories per cubic metre, 
 
 and 
 
 6102 X 0.11235 = 685.6 B. T. U. per cubic foot. 
 
 Two causes of *error may occur. It is not certain that the 
 combustion of the gas in the burner is regular; indications by 
 gas-meters are not always very sure, the start being capricious. 
 But these do not have much weight in its use for industrial 
 purposes, for which it is chiefly designed. The results are 
 very near those obtained by other methods. Stohmann, whose 
 competence in such matters is universally recognized, says 
 they give good results. 
 
 Bueb-Dessau, to prove the calorimeter, burnt hydrogen 
 prepared by electrical decomposition, and obtained after cor- 
 rections for thermometer and barometer 34150 calories per 
 
LEWIS THOMPSON'S CALORIMETER. 
 
 43 
 
 kilogram a difference of 350 calories from the usual number, 
 34500, or only 9 thousandths. 
 
 Prof. Jacobus has determined that there is a constant error 
 due to neglect of latent heat of moisture in products of com- 
 bustion of 2 per cent in the determinations with this appa- 
 ratus ; otherwise it is very satisfactory. 
 
 LEWIS THOMPSON S CALORIMETER. 
 
 Lewis Thompson's calorimeter has been used in England 
 for some time. It gives only approximate results, but as the 
 errors are of the same kind in each case, the results are com- 
 parable, and it has been found serviceable in industrial works 
 where quick and comparative observations are required. 
 
 The apparatus (Fig. 14) is composed of a glass calorimeter- 
 bath H containing water, a copper cylinder E in which the 
 
 FIG. 14. L. THOMPSON CALORIMETER. 
 
 FIG. 15. CALORIMETER 
 IN ACTION. 
 
 mixture of coal and potassa chlorate is placed, and surmounted 
 by the nitrate of lead fuse F. Enclosing this cylinder is a bell 
 D, having a tube C carrying a stop-cock. The cock is closed 
 before putting it in position in the water. K is a cleaner for 
 the tube C, and J is a thermometer. 
 
44 CALORIFIC POWER OF FUELS. 
 
 The fuze is lighted, and the whole quickly put in the jar of 
 water. The mixture of combustible and potassium chlorate 
 soon ignites and burns, all the gases generated being forced 
 out at the bottom of the bell through the perforations, and 
 bubble up through the liquid. After the combustion is finished 
 the temperature is taken and the heat-units calculated. 
 
 From 8 to 10 parts of oxidizing mixture is recommended 
 for one of coal; but if the coal is very rich this must be 
 increased to 1 1 parts, calculated on the crude coal. With 
 pure coal, cinders out, the extreme limits are 1 1 and 14 parts. 
 It would probably increase the accuracy of the method, if 
 the same quantity of oxidizing mixture was employed, what- 
 ever the kind of coal used, and to mix with it inert substances, 
 as silica or ground porcelain, in quantity varying with the 
 richness of the coal. 
 
 Scheurer-Kestner tested this apparatus very carefully, 
 using a great variety of fuels whose heats had been previously 
 ascertained by means of Favre and Silbermann's calorimeter. 
 He found some 15 per cent deficit in the figures, and after 
 correcting by this amount the results varied only a few per 
 cent from those actually obtained. In thirty different kinds 
 of coal tested the average was 1.8 per cent too low. 
 
 The use of this calorimeter requires some skill. Its imper- 
 fect insulation requires prompt reading and rapid combustion. 
 Care must be taken to wojk at temperatures very close to 
 that of the room, as the calorimetric bath is not protected. 
 The proportions of the mixture used vary, not only with each 
 kind of coal, but for each sample, on account of the propor- 
 tions of cinders. Fat coals require more oxidizer than lean 
 coals, as it is evident an increase in quantity of cinders should 
 require a decrease in oxidizer. But in changing the propor- 
 tions of oxidizer a certain difference in elevation of tempera- 
 ture is necessarily produced by the heat of solution of the 
 salts left after the combustion. These various causes render 
 its working rather delicate, and always uncertain. 
 
CHAPTER V. 
 CALORIMETERS WITH CONSTANT VOLUME. 
 
 THE results obtained with a calorimeter of constant volume 
 are not exactly the same as those obtained with one of con- 
 stant pressure ; but for solid or liquid substances the difference 
 is too small to consider, since the volume, as well as that of 
 the water produced, is inconsiderable in relation to the volume 
 of gas employed. As regards the correction for contraction 
 and expansion of the gases, they also are inconsiderable. 
 
 In his Traite de Mdcanique Berthelot has shown that 
 the heat generated by a reaction between gases at constant 
 pressure is equal to the heat of combination at constant 
 volume at any temperature whatever, increased by the pre- 
 ceding product counting from absolute zero; and he gives the 
 following formula for passing from one system to the other: 
 
 QT P = QT V + o.5424(A^- N'} + o.oo2(N N*)t, 
 
 QT P being the heat generated by the reaction at constant 
 pressure, and at the temperature T counting from ordinary 
 zero; QT V , the heat generated by the reaction at same tem- 
 perature and constant volume; N, the number of units of 
 molecular volume occupied by the components, these being 
 taken according to usage equal to 22.32 litres under normal 
 pressure at o ; N' ', the corresponding number of units of 
 molecular volume occupied by the product of the reaction. 
 
 As example, take the combustion of carbonic oxide at 15. 
 Then we have 
 
 CO + O = CO 8 generates at constant volume 68 calories.* 
 
 * These numbers refer to molecular weights. 
 
 45 
 
46 CALORIFIC POWER OF FUELS. 
 
 To pass from this to the heat given off under constant 
 pressure, observe that CO occupies a unit of volume and O a 
 half unit. Then 
 
 N = ii. 
 CO, occupies a unit of volume and 
 
 N' = i. 
 Hence N - N' = J., 
 
 At o there would be, then, for the difference between the 
 heat of combustion at constant pressure and that at constant 
 volume, 
 
 -j- 0.542 X i = + 0.271 calories. 
 
 At + 15 add to this + 0.015, which increases the cor- 
 rection then to 0.286. The heat of combustion of carbonic 
 oxide at constant pressure and 15 is then -|- 68.29 calories. 
 
 With a solid or liquid, this volume in relation to those 
 of the gases formed may be practically neglected, the same 
 as with the water; all reduce then to. the contraction and 
 expansion of the gases. Thus, for naphthalin, this correc- 
 tion does not exceed 8.8 in 9692 calories less than o. I per 
 cent. 
 
 In case of solids or liquids with unknown molecular 
 weight, as with fuels generally, this difference nrtey still be 
 approximately calculated, as it is sufficient to know the volume 
 of oxygen used in the combustion and that of the- gases pro- 
 duced. 
 
 The first calorimeter of constant volume in date is that of 
 Thomas Andrews, who in 1848 published results obtained 
 with a closed calorimeter. The calorimeter was not applicable 
 to solids or liquids ; the combustion of the gases was con- 
 ducted as in a eudiometer, but he did not take all the 
 precautions necessary to be certain of complete combustion. 
 
ANDREWS' CALORIMETER. 47 
 
 Nevertheless, the results obtained for certain gases are 
 remarkable, considering the elementary character of his 
 apparatus and working. The combustion of solids, on the 
 contrary, gave worthless results. 
 
 The calorimetric bomb of Berthelot and Vielle seems able 
 to replace advantageously all the other calorimeters as much 
 by its convenience as by its certainty of results. 
 
 Aime Witz made certain changes in the bomb designed to 
 facilitate its use, and devised his " calorimetric eudiometer," 
 in which only gases can be burnt. The apparatus is more 
 convenient than the bomb, but this convenience has been 
 gained at a sacrifice of precision. It is more an instrument 
 for practical use than a scientific calorimeter, but may be 
 useful within narrow limits. 
 
 ANDREWS' CALORIMETER. 
 
 In 1848 Andrews published his labors on the heat of 
 combustion of bodies, and notably on that disengaged h^ 
 combustion of different gases. He used a cal- 
 orimeter of constant volume, in which the com- 
 bustion-chamber was a copper cylinder (Fig. 
 1 6) weighing 170 grams (6 ounces), of 380 
 cubic centimetres (about 23^- cubic inches) ca- 
 pacity, and capable of resisting the pressure 
 
 exerted by the combustion of the same vol- FIG. 16. 
 
 rir /r* TT \ ^i ANDREWS' CALO- 
 
 ume of olefiant gas (C 2 H 4 ) with oxygen. RIMETER. 
 
 At the upper part, the cylinder had a small conical tube 
 closed by means of a perfect-fitting stopper b. A silver wire 
 a was fixed in this stopper, and to this was soldered a very 
 fine platinum wire for igniting the gases by a galvanic 
 current. The mixture of gases was prepared as for eudio- 
 metric analysis. 
 
 The combustion-chamber was entirely submerged in a 
 glass cylinder filled with water, of which the temperature is 
 
4 CALORIFIC POWER OF FUELS. 
 
 regulated so as to compensate approximately for the probable 
 use, and thus avoid corrections for influence of external air. 
 This cylinder was put into another, also of glass. A rotary 
 motion imparted to the cylinder aided circulation in the 
 liquid during combustion, which usually lasted thirty-five 
 seconds. 
 
 Andrews also applied his calorimeter to combustion of 
 solids, but judging from the low results he did not have per- 
 fect combustion. The results obtained with some of the 
 gases, on the contrary, are quite reliable, notwithstanding the 
 imperfections of the apparatus. 
 
 CALORIMETRIC BOMB OF BERTHELOT AND VIELLE. 
 
 Of all the calorimeters known to-day, the calorimetric 
 bomb of Berthelot is that which offers the most advantages, 
 as much from its ease of operation as from the precision of 
 its results. Only one operator is needed ; the combustion is 
 perfect ; the gaseous products need not be analyzed to deter- 
 mine the combustible substance ; no weight save that of the 
 substance used is needed ; and it is as applicable to solids and 
 liquids as to gases. 
 
 True, its use requires oxygen under high pressure ; but 
 this pressure (25 atmospheres) may be readily obtained with a 
 compression-pumg, which is easily procured; and at the 
 present time oxygen may be bought sufficiently compressed 
 for the purpose. Berthelot states that as much as 5 or even 
 10 per cent of nitrogen is allowable, but that the latter limit 
 must not be exceeded. 
 
 Mahler used compressed oxygen, and obtained good 
 results with that bought in the Paris market. This gas is 
 furnished in steel tubes and under 120 atmospheres pressure. 
 The cylinders contain sufficient gas to make a large number 
 of experiments before the pressure falls too low, i.e., below 
 25 atmospheres. 
 
BERTHELOT'S CALORIMETER. 
 
 Fig. 17 shows the bomb adjusted ready to place in the 
 calorimeter. Full details of the construction 
 will be found in Berthelot and Vielle's treatise, 
 Sur la force des metiers explosives, vol. I, p. 
 245. 
 
 Fig. 21 shows the arrangement adopted 
 by Berthelot to burn solids. The cylinder 
 (Fig. 1 8) is lined with platinum, and con- 
 structed so as to resist a pressure of 200 to 
 300 atmospheres. It is furnished with a 
 tight-fitting head (Fig. 17) fastened ex- 
 teriorly by a piece of steel (Fig. 19), clamped 
 on the external face of the bomb by a screw- 
 clamp (Fig. 20), which does not form a part of the apparatus 
 as immersed. 
 
 The sealing of the bomb results from the adherence of 
 the margin of the head BB (Fig. 21), and the interior of 
 the cylinder, and also between the platinum of the head and 
 the platinum of the cylinder. Berthelot makes the joint 
 
 FIG. 17. 
 
 FIG. 18. 
 
 FIG. 19. 
 
 FIG. 20. 
 
 tight with a smearing of vaseline around the opening, being 
 careful not to have a trace on the inside. If no bubbles 
 escape on putting it into the calorimetric bath, the joints are 
 tight. 
 
 The cover is pierced at the centre with a small hole, in 
 which is fitted a tube formed of a hollow screw acting as a 
 cock, and itself provided at the upper end with a circular 
 head. The electric ignition is produced by a platinum wire 
 
CALORIFIC POWER OF FUELS. 
 
 FIG. 21. 
 
 fitting in an opening of the removable conical cover E. This 
 is prepared (Fig. 21) in advance, and is covered with a layer 
 of gum lac applied in a strong alcoholic solution. When the 
 first coat is dry, a second one is put on and 
 dried in a stove. Berthelot says that the 
 combination of these two coatings, one elas- 
 tic and soft, the other hard and brittle, 
 resists very well the enormous pressure on 
 the cone. This cone, lightly greased, is put 
 into the conical opening in the bomb cover, 
 and screwed up tight by means of a nut. It 
 is well to protect the base of the cone by a 
 film of mica. 
 
 An electric current passed through E 
 (Fig. 21) reddens the spiral of very thin 
 iron wire f placed between the platinum 
 wires and one of the supports SS of the cap- 
 sule cc containing the substance m. This iron wire soon 
 burns and kindles the combustible. 
 
 Fig. 22 gives a general and complete internal view. 
 The iron spiral is formed of an iron wire ^ millimetre 
 (0.004 inch) thick, rolled up on a spindle. The wire may be 
 weighed, or by using the same length of wire always have the 
 same weight. 
 
 The spiral is attached on one side to the cone, and on the 
 other side by means of a platinum wire to the platinum sup- 
 porting the fuel, taking care that the iron has no straight por- 
 tions. The support of the capsule or platinum-foil is then 
 fixed in the cover, by aid of the screw, arranging it so that 
 the spiral is directly over the combustible used. The cover 
 is put on, turning it gently to make the contact more perfect. 
 The nut is tightened and the wire carefully screwed up, 
 always using wooden tongs to prevent injuring the bomb. 
 
 The form of the bomb is such as permits filling the calo- 
 rimeter with the smallest possible quantity of water a neces- 
 
BERTHELOT'S CALORIMETER. 5 1 
 
 sary condition that the temperature, and consequently the 
 precision, attain a high degree. For solids and also for coal 
 Berthelot uses bombs containing 400 to 600 cubic centimetres 
 (24 to 37 cubic inches), placed in a calorimeter of 2000 grams 
 (4.4 Ibs.) of water. 
 
 To determine the heat of combustion of coal, for instance, 
 
 FIG. 22. BERTHELOT BOMB. 
 
 it must be previously reduced to powder in order to have a 
 sample whose cinder is known. As all kinds of coal do not 
 burn completely in this state, they are formed into pastilles,* 
 which are weighed and burnt. They are put on a platinum 
 grating or foil, placed on the support 55 (Fig. 21), over 
 
 * We obtain very resisting pastilles or briquettes from fat coals by 
 simple compression in a pastille or suppository mould such as used by 
 druggists. With lean coals, or anthracite, the pastilles are too friable and 
 burn incompletely. This is easily remedied by mixing with a small 
 quantity of silicate of soda solution. Several of them should be made at 
 a time, the cinders of some being determined to obtain a mean and the 
 others burnt in the bomb. They may contain about I gram of pure coal. 
 
52 CALORIFIC POWER OF FUELS. 
 
 which and in contact with it is the iron spiral. At the 
 instant of lighting a slight noise is made, and soon the ther- 
 mometer begins to rise, showing that the combustion is pro- 
 ceeding. 
 
 Compressed oxygen may be introduced either by a pump 
 drawing the gas from a holder or by using a compressed-gas 
 cylinder. In both cases the gas is used without drying, if 
 the combustible contains hydrogen in quantity enough to 
 saturate the gases formed with water produced by its combus- 
 tion. But if, on the contrary, the combustible has little or 
 no hydrogen, like wood-charcoal for instance, it is not im- 
 material whether the oxygen be dry or not. In this case it 
 is well to use the oxygen moist, or to put a little water in the 
 bomb on the internal walls. By this means a correction for 
 heat of vaporization of water formed by the combustion is 
 obviated. 
 
 Oxygen .compressed to 120 atmospheres is nearly dry. 
 Berthelot observes: "The oxygen is, in short, actually or 
 nearly dry, and if it contains aqueous vapor the tension is 
 reduced to one fourth or one fifth on account of the change 
 in volume of the gas during its passage through the bomb. It 
 may be nearly nullified by the cold produced at the instant of 
 filling the bomb. This admitted, we shall have to account in 
 most combustions for the evaporation of the water produced 
 in the bomb; an3 this is from 2 to 3.5 calories in a bomb of 
 -J litre (about 0.6 pint), or 5 to 6 calories in a bomb of 600 to 
 700 cubic centimetres (37 to 43 cubic inches). These are 
 rather small quantities, it is true ; but while they can be 
 neglected in industrial tests, they cannot in rigorously 
 scientific investigations. This correction may, however, be 
 neutralized by putting into the bomb 4 or 5 cc. of water, 
 which should be considered in the calculations. 
 
 When oxygen not previously compressed is used and 
 forced in by a pump, Berthelot recommends passing the gas 
 through a large red-hot copper tube filled with oxide of the 
 
BERTHELOT'S CALORIMETER. 53 
 
 same metal, so as to burn any oil which may have been taken 
 from the pump. 
 
 Operation. At the laboratory of the College of France 
 the successive operations are as follows : 
 
 1. Light the fire to heat the oxygen red-hot; 
 
 2. While the gas-holder is filling with oxygen, the fuel is 
 dried; 
 
 3. Weigh the fuel; 
 
 4. Place the fuel in the bomb; 
 
 5. Grease the cover slightly; tighten with the screw; 
 
 6. Begin to compress the oxygen by forcing the air out 
 with a few strokes of the piston ; pump slowly to prevent 
 heating the pump ; 
 
 7. Close the stop-cock of the pump ; break the connection 
 with the bomb, extinguish the fire, and replace the bomb on 
 its support so as to carry it to the calorimeter room ; 
 
 8. Pour the water into the calorimetric bath. 
 
 The apparatus is allowed to come to equilibrium, and the 
 readings of the thermometer taken for five minutes. The 
 iron coil is then heated by the electric current from a small 
 bichromate battery. It takes fire and kindles the combustible, 
 which generally burns without smoke or producing any car- 
 bonic oxide, as Berthelot has shown.* 
 
 The water condensed from the combustion contains small 
 quantities of nitric acid, showing imperfectly purified gas. This 
 may be determined by titration, if accurate results are sought, 
 and calculated 0.227 calories per gram of HNO,. The cor- 
 rection will be very small. A correction for the iron used 
 may be made at the rate of 1.65 calories per gram, this being 
 the heat of formation of the magnetic oxide. 
 
 * With very fat coals it sometimes happens after a combustion that the 
 platinum shows a black or brown mark, indicating a slight deposit of black 
 or tar which has escaped combustion. Occasionally, also, a trace of tar is 
 found at the bottom of the bomb. These may be prevented by using a 
 grating or perforated plate instead of the foil. This detail must be attended 
 to with a new coal. 
 
54 CALORIFIC POWER OF FUELS. 
 
 With substances containing nitrogen and sulphur, such as 
 coal, the corrections are more complicated, as a larger quantity 
 of nitric acid is formed and the sulphur forms sulphuric acid. 
 If exactness is sought, it will not be sufficient to make a volu- 
 metric test : the sulphuric acid must be determined separately. 
 Generally, however, this estimation may be dispensed with, if 
 for technical purposes only. When, on the contrary, ab- 
 solutely correct figures are desired, both acids must be con- 
 sidered. In the calculation the nitric acid is reckoned as 
 0.227 calorie per gram and the sulphuric acid as 1.44 calories 
 per gram. 
 
 But these two corrections are really unimportant even 
 with coal, as it contains usually only about I per cent of 
 nitrogen or sulphur. One per cent of nitrogen represents 4^ 
 per cent of HNO 8 , or 10 calories; one per cent of sulphur 
 represents 3 per cent of H a SO 4 , or 43 calories, both quite 
 small compared with 7000 to 8000 calories. 
 
 Below will be found the details of a complete combustion 
 taken from Berthelot's work. 
 
 HEAT OF COMBUSTION OF CARBON. 
 
 The wood charcoal, purified by chlorine at red heat to- 
 remove all traces of hydrogen (Favre and Silbermann's 
 method), is dried at 120 to 140 C. (248 to 284 F.), then 
 weighed in a closed tube after cooling in a sulphuric acid 
 desiccator. 
 
 0.437 gram carbon; cinders, 0.0028 gram (0.66 per cent); 
 real carbon, 0.4342 gram. 
 
 PRELIMINARY PERIOD. 
 
 o minute 17.360 
 
 ist " 17.360 
 
 2d " i 
 
 3d minute. 17.360 
 
 4th " 17.360 
 
BERl'HELOT'S CALORIMETER. 55 
 
 COMBUSTION. 
 
 5th minute 18.500' 
 
 6th " 18.782 
 
 ;th minute 18.820 
 
 8th " 18.818 
 
 SUBSEQUENT PERIOD. 
 Qthminute 18.810 I2thminute 18.785 
 
 loth " 18.802 
 
 nth " J8.795 
 
 Initial cooling per minute, 
 
 1 3th " 18.775 
 
 I4th " 18.768 
 
 Final cooling per minute, 
 
 Atn = + 0.008. 
 Correction for cooling, 
 
 At = + 0.056. 
 Variation of temperature, uncorrected, 
 
 18.818- 17.360 = 1.438. 
 Value of corrected temperature, 
 
 1.438 + 0.056= 1.484. 
 Value in water of the calorimeter (including oxygen), 
 
 m = 2398.4. 
 Weight of acid formed ; 
 HNO 3 = 5 cc. of ^ normal KHO = 0.0173 gram. 
 
CALORIFIC POWER OF FUELS. 
 
 Total heat observed, q l = 3.5562 calories. 
 
 Heat of iron coil, 22.4 ) 
 
 3.9 I 9 > = - 263 
 
 Real heat due to the carbon, 3.5299 " 
 
 or for one gram, = 8.1296 calories, 
 0.4342 
 
 or per kilogram, 8129.6 calories, 
 
 or 14871.0 B. T. U. per pound. 
 
CHAPTER VI. 
 
 THE CALORIMETRIC BOMB ADAPTED TO 
 INDUSTRIAL USE BY MAHLER. 
 
 THE calorimetric bomb of Berthelot costs considerably 
 more than can be paid by an industrial laboratory, owing to 
 its large amount of platinum. Mahler replaced the interior 
 platinum of the bomb by an enamel deposited on the steel. 
 The description given by him in his paper before the Socittt 
 d* Encouragement de Paris, in June, 1892, is as follows: 
 
 The apparatus is shown in Fig. 23. It consists essen- 
 tially of a steel shell, B, capable of resisting 50 atmospheres 
 
 FIG. 23. MAHLER CALORIMETER. 
 
 and 22 per cent elongation. This quality was carefully chosen, 
 not only on account of the pressure it must stand, but also as 
 it aids the enameling. The metal is very pure, containing but 
 
 57 
 
53 CALORIFIC POWER OF FUELS. 
 
 little phosphorus or sulphur. Tensile strength tests are the 
 best criterion of quality. 
 
 It has a capacity of 654 cc. (40 cubic inches) at 15 C. It 
 is gauged with a balance showing -g-o^-Q. The total weight 
 is about 4 kilograms (8.8 Ibs.) with the accessories.* The 
 metal of the walls is 8 millimetres (about 0.3 inch). 
 
 The capacity is greater than Berthelot's, and has the ad- 
 vantage of insuring perfect combustion of carbon in all cases, 
 due to a certain excess of oxygen, even when the purity of 
 this gas as bought is not quite satisfactory. Besides, it is 
 designed to study all industrial gases, even those containing 
 a large percentage of inert gas ; hence it must be able to use 
 a sufficiently large quantity to generate the required tempera- 
 ture. The contraction at the top aids in enameling. 
 
 The shell is nickeled on the outside, while internally it 
 has a coating of white enamel, resisting corrosion and oxidiz- 
 ing action of the combustion. f It does not, however, offer 
 resistance to the heat, being very thin, and it weighs only 
 about 20 grams (308 grains). 
 
 It is closed by an iron stopper made tight by a lead washer 
 (P, Fig. ^) and clamped down. This carries a conical-seated 
 stop-cock, R, of fine nickel a metal almost unoxidizable. 
 An electrode well insulated and reaching the interior by a plat- 
 inum wire runs through the stopper. 
 
 Fig. 24 shows most of the details. 
 
 Another platinum wire, also fixed on the cover, supports 
 the platinum disk or foil on which the fuel is placed. 
 
 The calorimeter, the non-conducting material, the support 
 for the shell in the water, and the agitator differ in numerous 
 details from those of Berthelot, and are much cheaper. 
 
 * Slight modifications have been made in the dimensions of the metal of 
 the bombs made lately by Golaz. 
 
 f Prof. W. O. Atwater finds that the enamel chips off in time, and that 
 after about 300 combustions it requires re-enameling. Hempel for coal 
 determinations uses one without any inside enamel. 
 
MA HLER S CA L OKI ME TER. 
 
 59 
 
 The calorimeter is of thin brass, and is quite large on ac- 
 count of the size of the combustion-chamber. It contains 
 2200 grams (4.85 Ibs.) of water, thus eliminating the causes of 
 error due to the loss of a few drops by evaporation.* The 
 agitator of Berthelot is supplanted by a very simple and gentle 
 cinematic combination called a drill 
 movement, and which can be worked 
 without fatigue. The source of elec- 
 tricity is a Trouve" bichromate pile (P, 
 Fig. 23) of 10 volts and 2 amperes. 
 
 The oxygen used is that furnished by 
 the Compagnie Continentale d'Oxygene. 
 This company supplies oxygen free from 
 CO,, but containing from 5 to 10 per 
 cent of nitrogen. This means of supply 
 simplifies the manipulation ; it also ob- 
 viates the introduction of grease, as 
 happens with oxygen compressed by a 
 pump in the laboratory. f 
 
 The cylinders vary in size, and con- 
 tain gas at a pressure of 120 atmospheres. 
 The average content is about 1200 litres 
 (about 40 cubic feet) compressed. They 
 have a uniform top, and hence the copper pipe connecting the 
 bomb with the manometer and the cylinder, once adjusted, 
 will fit all of them. 
 
 The method of working is very simple. 
 
 Weigh i gram of the substance to be tested in the cap- 
 sule. Fasten a small weighed iron wire (English gauge 26 or 
 30) to the electrode and to the support of the capsule. Put 
 the end in the bomb and fasten in the cover, which should be 
 held in a vise. Put the conical stop-cock in connection with 
 the oxygen cylinder, and open it carefully so as to allow suffi- 
 
 zfiffityar 
 
 FIG. 24. 
 
 * The evaporation never exceeds a gram per hour, 
 f This gas is also compressed by pumps at the works. 
 
60 CALORIFIC POWER OF FUELS. 
 
 cient oxygen to pass in for the required pressure. Close the 
 cock of the oxygen cylinder, carefully close the conical cock, 
 and break the connection between the bomb and the oxygen 
 cylinder. The substance, especially if coal, must not be too 
 fine, and the oxygen must flow in very slowly to avoid blow- 
 ing any of it from the capsule. 
 
 The bomb thus prepared is placed in the calorimeter, and 
 the thermometer and agitator adjusted. Pour in the previously 
 weighed water, agitate a few minutes to restore equilibrium of 
 temperature, and commence the observations. 
 
 The experimenter notes the temperature minute by minute 
 for four or five minutes, and determines the rate of the ther- 
 mometer before the combustion. Then he joins the elec- 
 trodes, and the combustion begins immediately, almost instan- 
 taneously; but the transmission of heat to the calorimeter 
 takes some time. 
 
 The temperature is taken one-half minute after kindling, 
 then at the end of the minute, then at each minute to the 
 time when the thermometer begins to lower regularly. This 
 is the maximum. The observations are continued for a few 
 minutes more to ascertain the rate of fall of temperature. 
 
 We now have all the elements needed for the calculation, 
 and particularly for the single correction necessary to make 
 under the circumstances. This is the correction for loss of 
 heat before reaching the maximum temperature, which is 
 quite small considering the short time and the large mass in- 
 volved. 
 
 It is not necessary to use the corrections of Regnault and 
 Pfaundler with this apparatus. Newton's law of cooling gives 
 sufficiently accurate results, even in rigorous investigations. 
 Special experiments made to determine the rate of cooling of 
 the water in the calorimeter, when the apparatus was set up as 
 usual, showed that the correction may be regarded as follow- 
 ing a simple law, but between comparatively large limits, 
 
MAHLER'S CALORIMETER. 6 1 
 
 even under a variation of several hundred grams in amount of 
 water used. 
 The law* is 
 
 1. The decrease in temperature observed after the maxi- 
 mum represents the loss of heat of the calorimeter before the 
 maximum and for a certain minute, with the condition that 
 the mean temperature of this minute does not differ more than 
 one degree from the maximum. 
 
 2. If the temperature considered differs more than one 
 degree but less than two degrees from the maximum, the 
 number representing the rate of decrease dimminished by 
 0.005 will be the correction. 
 
 The two preceding remarks suffice in all cases with Mah- 
 ler's apparatus. The variation of heat in the first half-minute 
 after kindling may also be corrected by the same law. 
 
 The agitator must be worked continually during the ex- 
 periment, being careful of the thermometer. 
 
 When through, the conical valve is opened and then the 
 bomb. Wash the inside with a little distilled water to collect 
 the acids formed. The proportion of acids carried away by 
 the escaping oxygen at the opening may be neglected. De- 
 termine the acids volumetrically. 
 
 When experimenting with substances low in hydrogen and 
 incapable of furnishing sufficient water to form nitric acid, it 
 is advisable to put a little water in the bomb, or hyponitric 
 acid would be formed. 
 
 All the data being obtained, we proceed to the calculation 
 of the calorific power Q. 
 
 Let A be the observed difference of temperature ; 
 a, the correction for cooling; 
 P, the weight of water in the calorimeter; 
 P', the equivalent in water of the bomb and acces- 
 sories ; 
 
 * It is evident that the rule must be modified for apparatus notably dif- 
 ferent from that used by Mahler. 
 
62 CALORIFIC POWER OF FUELS. 
 
 p, the weight of the nitric acid, HNO 3 ; 
 />', the weight of the iron ; 
 
 0.23 calorie, the heat of formation of I gram of nitric acid ; 
 and 1.6 calories, the heat of combustion of I gram of iron. 
 We then have 
 
 Q = (J + a)(P+P') - (0.23/4- i.6/). 
 
 In testing coal in this manner the small amount of sul- 
 phuric acid formed will be reckoned as nitric acid without 
 serious error, as it will be very small. The heat of the reac- 
 tion is 1.44 calories per gram of H a SO 4 formed. 
 
 The above details apply to liquids as well as solids. Heavy 
 liquids, such as the heavy oils, tars, etc., are weighed directly 
 into the capsule ; but light, easily vaporized liquids must be 
 placed in pointed glass bulbs. These are put into the capsule, 
 and just before closing the bomb are broken to allow access 
 of the oxygen to the liquid. An almost perfect combustion 
 is obtained in operating with a great variety of materials, 
 nothing but cinders remaining. 
 
 To determine the calorific power of gases the exact con- 
 tent of the bomb must be known. Fill it first with gas. 
 Then work the air-pump to reduce the pressure to several 
 millimetres of mercury, and then fill the bomb again with gas, 
 under atmospheric, pressure and at the laboratory temperature. 
 The bomb may then be considered full of pure gas. 
 
 The method of working with gases is the same as with 
 solids or liquids. The operator must not forget the need of 
 preventing too great dilution with oxygen, as then the mix- 
 ture will cease to be combustible. With illuminating gas 5 
 atmospheres of oxygen is sufficient, and with producer gas 
 only one-half atmosphere, as shown by the mercury gauge, is 
 needed. 
 
 The gases to be burnt are kept in gas-holders over water 
 saturated with gas, or over salt water, according to circum- 
 
MAHLER'S CALORIMETER. 63 
 
 stances, and are saturated with aqueous vapor when they enter 
 the bomb. From the calorific capacity of the different parts 
 we obtain that of the whole, the glass and enamel being 
 omitted. 
 
 Soft steel 3945 grams. 3945 X 0.1097 = 432.76 
 
 Brass 545 " 545XO.O93 = 50.68 
 
 Mercury, plati- 
 num, and lead 72 * 72X0.03 = 2.16 
 
 Sum 485. 60 grams. 
 
 The coefficient 0.1097 is the one adopted by the College 
 of France, from Berthelot and Vielle's experiments, for a steel 
 of similar quality. We have given above (page 14) the 
 calculations relative to the valuation in water. By direct 
 method of mixing water of different temperatures Mahler 
 found the equivalent to be 470 and 484, and assumed the 
 mean 481. 
 
 By the method of burning a body of known composition 
 and heat of combustion he obtained with naphthalin 9688 
 calories within -^Jinf ^ ^hat given by Berthelot (9692). 
 
 The equivalent in water may also be obtained by burning I 
 gram of known composition and heat of combustion naph- 
 thalin for instance.* We may alsoj after Berthelot, burn a sub- 
 stance of fixed composition at two trials with different weights 
 of water in the calorimeter. Two equations are thus formed, 
 from which the heat of combustion of the body used is elimi- 
 nated, and the heat sought obtained. 
 
 In using naphthalin care must be taken to weigh it only 
 after being gently fused in the capsule. It is so light that if 
 not agglomerated some would be blown away by the oxygen. 
 In practice the tests are made rapidly. The water equivalent 
 once determined may be verified by combustion of cane- 
 
 *This practical method has the advantage of automatically eliminating 
 causes of error. 
 
64 CALORIFIC POWER OF FUELS. 
 
 sugar (C^H^O,,), for which Berthelot and Vielle found 3961.7 
 calories. (Use 2 grams for a combustion.) 
 
 Examples of Calculations. 
 
 Mahler gives several types of calculations from his notes, 
 so as to show the different circumstances which may occur. 
 A. Colza Oil. Elementary analysis showed 
 
 Carbon 77.182 per cent. 
 
 Hydrogen 11.711 " " 
 
 Oxygen and nitrogen 11.107 " '* 
 
 100.000 " " 
 
 Weight taken, I gram. Calorimeter contained 2200 grams 
 water. Equivalent in water of bomb, etc., 481 grams. 
 Pressure of oxygen, 25 atmospheres. 
 
 The apparatus prepared as above was allowed to rest a 
 few minutes to gain equilibrium of temperature. Then com- 
 menced noting the temperatures. 
 
 PRELIMINARY PERIOD. 
 o minute 10.23 3 minutes 10.24 
 
 1 10.23 
 
 2 minutes 10.24 
 
 Rate of variation, 
 
 4 10.25 
 
 5 " 10.25 
 
 10.25 10.23 o 
 
 a. = - - = 0.004. 
 
 The electrodes are connected and the combustion begins. 
 COMBUSTION PERIOD. 
 
 5 J minutes 10. 8o c 
 
 6 " 12.90 
 
 7 minutes.. 13.79 
 
 .. 13.84 maximum.* 
 
 * Prof. Jacobus recommends plotting the temperatures and using, not 
 the maximum, but the one at the instant the curve of cooling becomes a 
 straight line. The difference is slight, but important in some cases. 
 
MAHLER'S CALORIMETER. 6 5 
 
 PERIOD AFTER MAXIMUM. 
 
 9 minutes 13.82' 
 
 10 " 13.81 
 
 12 minutes J 3-79 
 
 13 " 13.78 
 
 ii " .......... 13,80 
 
 Rate of variation after maximum is 
 13.84 13.78 
 
 
 = 0.012. 
 
 The thermometer observations now stopped. 
 The gross variation in temperature was 
 
 13.84- 10.25 = 3.59. 
 
 The corrections are as follows : 
 
 The system lost during the minutes (7, 8) and (6, 7) a 
 quantity of heat corresponding to 2a t . 
 
 2a t 0.012 X 2 = 0.024. 
 In the half-minute (5^, 6) it lost 
 
 \(a t 0.005) = 0.0035. 
 But during the half-minute (5, 5-^) it gained 
 
 0,004 
 ?a = = 0.002 . 
 
 2 
 
 Consequently, the loss for the minutes (5, 6) is 
 0.0035 0.002 = 0.0015. 
 
66 
 
 CALORIFIC POWER OF FUELS. 
 
 So that the system had lost, before reaching the maximum 
 temperature, 
 
 0,024 + 0.0015 = 0.0255, 
 
 which must be added to the 3.59 already found, making the 
 variation in temperature 3.615, neglecting the 4th decimal. 
 The quantity of heat observed, then, is 
 
 Q = (2200 + 481)3.615 = 2681 X 3.615 = 9.6918 calories. 
 From this number must be subtracted 
 
 1. The heat of formation of the o. 13 
 
 gram of HNO 3 0.13 X 0.23 = 0.0299 
 
 2. The heat of combustion of 0.025 
 
 gram of iron wire 0.025 X 1.6 =0.04 
 
 Total subtraction 0.0699 
 
 The final result is, then, 
 
 9.6918 0.0699 = 9.6219 calories, 
 or for I kilogram 962 1.9 calories, equivalent to 17319.4 B.T.U. 
 
 TECHNICAL EXAMINATION OF COAL. 
 
 The coal taken was a sample of Nixon's coal from South 
 Wales. 
 
 Preliminary Period. 
 
 Combustion. 
 
 After Combustion. 
 
 minutes, degrees, 
 o 15.20 
 I 15.20 
 2 15.20 
 3 15.20 
 
 minutes. degrees. 
 3& 16.60 
 4 n.92 
 5 18.32 
 6 18.34 
 maximum 
 oxygen pressure 25 
 atmospheres 
 
 minutes. degrees. 
 7 18 32 
 8 18.30 
 9 18.30 
 10 18.30 
 ii 18.26 
 18.34-18.26 
 
 
 
 
MAHLER'S CALORIMETER. 
 
 Difference of gross temperature . 3. 140 
 
 Correction (4, 5) (5, 6) 0.016 X 2 0.032 
 
 (4, 3i) 0-005 
 
 Corrected difference of temperature 3. 177 
 
 or 3.18. 
 
 Calories. 
 
 Heat disengaged 3.18. 3.18 X 2.681 = 8.5256 
 
 Iron wire 0.025. 0.025 X 1.6 =0.04 
 
 Nitric acid 0.15. 0.15 X 0.23 =0.0345 
 
 0.0745 
 
 For one gram 8.45 1 1 
 
 or 8451.1 for I kilogram, equivalent to 15212 B. T. U. 
 
 EXAMINATION OF A GAS. 
 
 Illuminating gas was examined under the following con- 
 ditions:* 
 
 Barometric pressure 761 mm. (29.6 inches). 
 
 Tension of aqueous vapor. 8 '* (0.314 inch). 
 
 Temperature of laboratory 18.5 C. (65.3 F.). 
 
 Volume of bomb 654 fee. (39.9 cubic inches). 
 
 " " " dry at o and 760 mm. 
 
 606 cc. (37 cubic inches). 
 
 The capsule was left in its usual place in the bomb to pre- 
 vent specks of iron oxide from dropping on the enamel and 
 injuring it. 
 
 * See Kroeker's calorimeter on page 73. 
 f Exactly 653.9 cubic centimetres. 
 
68 
 
 CALORIFIC POWER OF FUELS. 
 
 Preliminary 
 Period. 
 
 Combustion. 
 
 After Combustion. 
 
 Remarks. 
 
 minutes, degrees. 
 18.80 
 I 18.80 
 2 18.80 
 3 18.80 
 4 . 18.80 
 
 flo = 0.00 
 
 minutes, degrees. 
 4i I9-50 
 5 20.00 
 6 20.08 
 7 20.81 
 maximum 
 
 minutes. degrees. 
 8 20.07 
 9 20.06 
 
 10 20.06 
 
 II 20.055 
 12 20.05 
 20.08 20.05 
 
 Pressure of oxygen 
 5 atmospheres 
 grams. 
 Nitric acid. . . . 0.06 
 Iron wire 0.025 
 
 
 Gross difference of temperature, A 1.28 
 
 Correction as usual, a 0015 
 
 Difference, A -\- a 1-295 
 
 Calories. Calories. 
 
 Quantity of heat observed, 1.295 1.295X2.681= 3.47189 
 
 Heat of HNO 3 formation 0.06 X 0.23 = 0.0138 
 
 Heat of iron-wire combustion 0.025 X 1.6 = 0.04 
 
 0.0538 
 
 Heat of combustion of 606 cc. at o and 760 mm 3.41809 
 
 or per cubic metre at 760 mm. 5640, or 633.6 B. T. U. per cubic foot. 
 
 COMBUSTION USING AN AUXILIARY SUBSTANCE. 
 Sometimes an unconsumed residue is left while determin- 
 ing the heat of combustion of some difficultly burning sub- 
 stances, diamond or graphite for instance. In this case a 
 combustible auxiliary is used to obtain complete burning bf 
 the sample. The most convenient to use is naphthalin (C 10 H 8 ), 
 the heat of combustion of which is exactly known, 9692 cal- 
 ories. 
 
 Take petroleum coke, which is nearly allied to graphite. 
 It is mixed with a little naphthalin which has been previously 
 melted at a low heat and then cooled. After cooling the 
 weight of the naphthalin is taken. 
 The coke analyzed as follows: 
 
 Carbon 97-855 per cent. 
 
 Hydrogen 0.489 ' ' 
 
 Oxygen ... 1.196 " " 
 
 Nitrogen 0.260 " 
 
 Ash.. .. 0.200 " " 
 
 100.000 
 
MAHLER'S CALORIMETER. 
 The data obtained are as follows: 
 
 6 9 
 
 Preliminary 
 Period. 
 
 Combustion. 
 
 After 
 Combustion. 
 
 Remarks. 
 
 
 minutes, degrees. 
 
 minutes, degrees. 
 
 minutes, degrees. 
 
 
 grams. 
 Ooaj. 
 
 
 
 IJ. 2^ O^ 
 
 
 o 025 
 
 
 7 2H O2 
 
 
 Nitric acid 
 
 o 080 
 
 tfo = 0.002 
 
 8 25.13 
 9 25.14 
 maximum 
 
 at = 0.015 
 
 Water of calorimeter. 
 Equivalent in water. . 
 
 2 2OO. 
 4 8l. 
 
 Difference of temperature 25.14 22.04 = 3-ioo 
 
 Correction for minutes (9, 8), (8, 7), (7, 6). . 0.015 X 3 = 0.045 
 
 " " minute (5i, 6) =0.005 
 
 " i " (5, 5i) =o.ooi 
 
 Corrected temperature difference 
 Then, 
 
 Total heat developed 3.15 3.15 X 2.681 = 
 
 From this subtract 
 
 Heat due to naphthalin 0.034 X 9692 = 0.3295 
 
 " " " iron wire 0.025 X 1.6 = 0.04 
 
 " " HNO 3 0.08 X 0.23 =0.0184 
 
 Heat developed by the combustion of the coke, 
 or 8057.2 per kilogram, or 14503 B. T. U. 
 
 8.4451 
 
 0.3879 
 8.0572 
 
 When the combustible tested contains hydrogen, it must 
 be remembered that, while the gas in the bomb is dry at the 
 beginning, it is saturated at the close of the experiment. In 
 reality, the latent heat of vaporization of the small quantity 
 of water necessary to be added is inconsiderable. The mean 
 of several tests was 5 m 8500 calories observed, or only 
 T _i__. Still, when we test gases, which cause less marked 
 difference in temperature than solids or liquids, we must allow 
 for this heat of vaporization to be exact. 
 
 It may be asked if any allowance will be made for the 
 heat of the electric current at the moment of kindling. The 
 
70 CALORIFIC POWER OF FUELS. 
 
 heat developed by a current with intensity 7 and electro- 
 motive force E is 
 
 El 
 
 C= - 1, 
 4.17 
 
 t being reckoned in seconds. If / was appreciable, this should 
 be considered at least in exact determinations. But, actually, 
 / is very small ; the contact is hardly established before the 
 iron is burnt and the contact broken.* 
 
 Mahler cites two successive tests made on the same coal 
 with his bomb and with the bomb of the College of France, 
 as furnishing proof of the accuracy of his method. 
 
 The following results were obtained : 
 
 Scheurer-Kestner 
 
 at the Mahler. 
 
 College of France. 
 
 Coal (pure) from Bascoup, Belgium .... 8828 8813 
 
 The calculations may be rendered simpler and the obser- 
 vation more rapid, still being exact enough for industrial uses. 
 Take the equation 
 
 arranging the terms^in order of the corrections 
 
 a = 4(P+ P') + a(P+P) - (0.2 3 / + I.6/). (2) 
 It is clear that the calculation of the calorimetric operatioa 
 
 * In exact researches this heat can be easily determined if wished. It 
 will be sufficient to measure the electromotive force in volts. Then put 
 an amperemeter in the line which connects the bomb and kindle the com- 
 bustible as usual. The displacement of the needle shows the intensity of 
 the current under the conditions of the test, and also the time during which 
 
 r* j~ 
 
 the current was closed. The formula - / will give the quantity of heat 
 
 4.17 
 
 sought. 
 
ATWATER'S CALORIMETER. 71 
 
 reduces to the determination of a maximum and to one multi- 
 plication if we have 
 
 <*(/>+ /") = o.2 3 /+i.6/. .... (3) 
 
 Now from the tests made we readily see that whatever 
 value a may take, it increases with the quantity of heat gen- 
 erated in the bomb ; it is a little greater when the external air 
 is warmer than when it is cooler a fact which may be attrib- 
 uted to the influence of evaporation on the cooling of the 
 bath.* 
 
 On the other hand, the nitric acid appears to increase with 
 the quantity of heat generated, and tends to offset the cor- 
 rection from a. In short, /' is, within certain limits, at the 
 control of the observer, same as P '. We consider it then 
 possible to arrange once for all so as to have the expression 
 (3) sufficiently close for industrial purposes. 
 
 This can be done with Mahler's apparatus. Thus for oil 
 of colza the multiplication A(P -f- P) gave 9625 calories, 
 which is within 3-^ of the final number obtained after all 
 corrections ; with the Nixon's coal we found t lat d(P-\- P) = 
 8418 calories, which differed ^ from the correct number; 
 with coal-gas the product 2681 X 1.28 = 3432 calories, while 
 the corrected result was 3418, or ^^ difference. 
 
 ATWATERS CALORIMETER. 
 
 Prof. Atwater has considerably modified the bomb, so 
 that it seems to have some advantages for easy working. 
 Fig. 25 gives a sectional view of it in the calorimeter. The 
 steel used is the same as that used in the Hotchkiss guns, 
 
 * The rapidity of cooling in the apparatus employed by Mahler was, 
 according to experiments, between 15 and 20 C. 
 
 JB 
 
 = 0.005(7*- To), 
 
 To being the temperature at which cooling ceases. 
 
CALORIFIC POWER OF FUELS. 
 
 and having an unusually high tenacity, seems admirably fitted 
 for the purpose. A represents the bomb, C the screw-cap, 
 B the cover, which is placed on the bomb cylinder and held 
 down by the screw-cap. " The cover is provided with a neck 
 into which fits a cylindrical screw , holding another screw &.F 
 On the side of the neck is an aperture G, between the lower 
 end of D and the shoulder. In D is a washer of lead, on 
 which the lower edge of E fits. By opening or closing the 
 screw F the narrow passage from z is opened or closed. The 
 opening is used for admitting oxygen at a high pressure 
 through a narrow passage to charge the bomb. In B is an 
 aperture through which passes the platinum wire H, which is 
 separated from the metal of the cover 
 by insulating material. Hard vulcan- 
 ized rubber serves very well for this 
 purpose. Fastened to the lower side 
 of the cover is another platinum rod, /, 
 between which and H an electrical con- 
 nection is made with a very fine iron 
 wire. A screw- ring holds the small 
 platinum capsule, in which the sub- 
 stance to be burned is placed. At KK 
 are ball-bearings of hard steel to avoid 
 friction in screwing the cap down." 
 
 1 * The large cylinders N and O are 
 made of indurated fibre, and covered 
 with plates of vulcanized rubber. A 
 stirrer serves for equalizing the temper- 
 ature of the different portions of water 
 FIG. 25.-ATWATER BOMB. after the combustion is completed." * 
 
 The thermometer used is by Fuest 
 
 of Berlin, graduated to T -^ degree, and can be read with a 
 magnifying-glass to yoV<F degree. 
 
 *Prof. W. O. Atwater, in Bulletin No. 21, U. S. Dept. of Agriculture, 
 1895, pages 124 and 126. 
 
KROEKER'S CALORIMETER. 
 
 73 
 
 The apparatus has been used with success in making the 
 very numerous determinations made by Atwater on the heats 
 of combustion of food-products and other allied organic sub- 
 stances. 
 
 KROEKER'S CALORIMETER. 
 
 Kroeker has recently modified the bomb, making two in- 
 let channels instead of one. By this means he has a current 
 of oxygen gas passing in at one opening and waste gases 
 passing out at the other. It can thus be used for the same 
 purpose that a Junker calorimeter is used, and it is claimed 
 with just as satisfactory results. 
 
 The cylinder (Fig. 26) is bored out of a piece of Martin 
 steel, and has a closely-fitting screw-plug for cover, the depth 
 of the screw joint being 25 mm. The walls 
 of the cylinder are 10 mm. thick; external 
 diameter, 72 mm. ; internal diameter, 52 
 mm. ; height, 120 mm. ; contents, 200 cc. 
 It has four small legs on the under side, 
 which support it and keep it entirely sur- 
 rounded by the water of the bath. The 
 entire inside surface is enameled, or prefer- 
 ably platinized. The fuel, in the form of 
 compressed cylinders weighing one gram, 
 is put into the carrier, ignited as usual, 
 and the combustion gases collected and 
 examined. 
 
 He also has a method of heating the 
 calorimeter bomb in an oil-bath so as to 
 expel all the water of combustion and hy- FlG 2 6. KROEKER 
 dration. He thus obtains data for cor- CALORIMETER. 
 rections due to the usual method of determining the water, 
 i.e., considering the water as condensed. 
 
74 
 
 CALORIFIC POWER OF FUELS. 
 
 WALTHER-HEMPEL BOMB. 
 
 Two modifications of the Berthelot bomb are known 
 under this name. The larger one does not differ in enough 
 points to make a special mention of it necessary; but the 
 smaller one, the one intended for use in analysis, is worthy of 
 description. 
 
 It consists of a small cylinder of 33 cc. capacity (Fig. 27), 
 bored out of white cast iron and enameled inside. The walls 
 are 2 millimetres thick, and it is strong enough to resist eight 
 times the pressure generally used. The cover 
 is fastened on by means of a screw-clamp, 
 and through it passes the slanting opening a t 
 having the electric wire-carrier insulated by 
 a caoutchouc sheath. To the wire at the end 
 of this sheath is attached a platinum wire for 
 kindling the combustible. On the opposite 
 side of the cover is the oxygen tube d. The 
 platinum wire c is attached to the under side 
 of the cover, and supports the combustible- 
 carrier and its little fire-clay cylinder e. 
 
 The fuel is made into small cylinders by 
 compression, put into the fire-clay cylinder, 
 and ignited by the electric spark. The 
 products of combustion are collected and 
 weighed or measured : the water partly in the 
 bomb and partly by means of a calcium chlo- 
 ride tube; the nitric and sulphuric acids are 
 determined by titration with y^- normal alkali, 
 and afterwards separated if deemed necessary. It is claimed 
 to be capable of use the same as a large one. A full descrip- 
 tion of it is given in the Berliner Bericht for January, 1897. 
 
 FIG. 27. 
 WALTHER- 
 HEMPEL BOMB. 
 
CHAPTER VII. 
 SOLID FUELS. 
 
 COAL. 
 
 AMONG the first careful tests ever made, to determine the 
 heat value of different kinds of coal, are those made in 1843 an d 
 1844 by Prof. W. R. Johnson for the U. S. Navy. He 
 analyzed and tested all the kinds obtained from the United 
 States and England, which were then in use by the navy. 
 At the time they were made the calorimetric determinations 
 were not considered as of the importance they are now, 
 and his tests were limited to determining the evaporative 
 power of the coals. Mr. W. Kent reviewed them in the 
 Engineering and Mining Journal, 1892, and showed that up to 
 the time of the experiments nothing comparable with them 
 had been attempted, and that in many respects they compare 
 favorably with work done to-day. 
 
 In 1857 Morin and Tresca made numerous determina- 
 tions of the calorific power of coal and wood, and in 1853 
 they published a work on " Fuels and their Calorific Power," 
 in which they make many recommendations for more accurate 
 work. They wrote: " It would be extremely important if 
 experiments with the calorimeter could be made on most of 
 the fuels, by methods similar to those used by Favre and Sil- 
 bermann." 
 
 In 1868 such experiments were made by Scheurer-Kest- 
 ner, and continued by him later with the aid of Meunier- 
 Dollfus. They based their calculations on pure coal, i.e., with 
 moisture and ash deducted. This method, which has been 
 
 75 
 
?6 CALORIFIC POWER OF FUELS. 
 
 followed by many others, seems very logical, as it facilitates 
 comparison of different fuels by reducing them to the same 
 basis. Enormous errors due to comparison of values not 
 comparable are thus obviated. Coal having 5 per cent im- 
 purity has been compared with coal having only I per cent, 
 no account being made for the difference, and of course very 
 erroneous and misleading deductions obtained. 
 
 It is a simple task for the engineer or the workman even, to 
 determine approximately the proportions of moisture and ash 
 as given on the grate. Knowing these proportions and the 
 heat of combustion of the pure coal, they can render a state- 
 ment of the practical working. If, on the contrary, the ex- 
 perimenter is limited in such way that he neglects the com- 
 position of the coal, it is impossible to make a conjecture as 
 to its intrinsic or comparative value; still less can he judge of 
 it as a steam generator. 
 
 In 1879 Bunte made some experiments at Munich, using a 
 special apparatus devised by him for the occasion, which 
 was part calorimeter and part boiler. The tests were pub- 
 lished in Dingler's Polytechnisches Journal. Some of the 
 results are included in the tables of this book. 
 
 Since then numerous tests have been made on nearly all 
 the known coals. A collection of all available ones from 
 which the desirejd data could be obtained will be found far- 
 ther on. 
 
 The question as to the actual evaporative effect of each 
 coal can be settled only by actual tests made on the boiler 
 intended for use, as the same coal will give slightly different 
 results with different kinds of boilers ; also, and in a more 
 marked degree, with different methods of firing and handling. 
 The results in the tables cannot be taken, then, as absolute 
 for all boilers under all circumstances, but they can be 
 depended on for comparison of the different fuels with the 
 same boiler and under proper conditions. 
 
 The manner in which a coal acts under heat in a closed 
 
SOLID FUELS. 
 
 77 
 
 vessel is a most important indication, taken in connection 
 with its elementary composition. Gruner gave his opinion 
 that the real value of a coal could be determined better from 
 its proximate than from the ultimate composition. Speaking 
 of the Loire coal, he says : 
 
 " The proximate analysis, which consists in distilling coal 
 in a retort and incinerating the residue, allows direct valu- 
 ation of the agglomerating power as well as the nature and 
 proportion of the ash. Further, it is easy to show, especially 
 with the aid of the work of Scheurer-Kestner and Meunier- 
 Dollfus, that the calorific power varies with the proportion of 
 fixed carbon left by distillation. This is true at least for all 
 coal properly so called, but not always true for anthracite 
 and lignite." * 
 
 Gruner formed the following table based on the quantity 
 and nature of the coke furnished and the calorific power. He 
 held, from the results of S.-K. and M.-D., that if the heat 
 value of a coal increases with the proportion of fixed carbon 
 
 
 
 
 
 
 Industrial 
 
 
 
 Per Cent 
 
 
 
 CalorificPower. 
 
 Classes or Types 
 of Coal 
 properly so called. 
 
 Per Cent 
 Coke to 
 Pure Coal. 
 
 of 
 Volatile 
 Matter 
 in 
 
 Nature and 
 Appearance 
 of Coke. 
 
 CalorificPower, 
 Actual. 
 Calories. 
 
 Water at o 
 Vaporized at 
 112 per Kilo of 
 Pure Coal 
 
 
 
 Pure Coal. 
 
 
 
 Burnt, 
 
 
 
 
 
 
 in Kilograms. 
 
 i. Dry coals with | 
 long flame, ) 
 
 55 to 66 
 
 45 to 40 
 
 ( Powdery or 1 
 < slightly V 
 ( coked. I 
 
 8000 to 8500 
 
 6.7 to 7.5 
 
 
 
 
 f Completely ] 
 
 
 
 2. Fat coals with ) 
 long flame (gas V 
 coals), ) 
 
 60 to 68 
 
 40 to 32 
 
 agglomer- | 
 -{ ated, often- > 
 er caked, | 
 
 8500 to 8800 
 
 7.6 to 8.3 
 
 
 
 
 (.but porous. J 
 
 
 
 3. Fat coals, prop-] 
 erly so called 1 
 (" blacksmith " f 
 coals), 
 
 68 to 74 
 
 32 to 36 
 
 ( Caked and ) 
 -< more or less > 
 ( puffy. ) 
 
 8800 to 9300 
 
 8.4 to 9.2 
 
 4. Fat coals with } 
 short flamev 
 (coking coals), J 
 
 74 to 82 
 
 26 to 18 
 
 ( Coked, | 
 ( compact, j 
 
 9300 to 9600 
 
 9.2 to 10 
 
 
 
 
 ( Slightly ] 
 
 
 
 5. Lean coals or j 
 anthracite, j 
 
 82 to 90 
 
 18 to 10 
 
 J coked, 
 1 oftener j 
 
 9200 to 9500 
 
 9.0 to 9.5 
 
 
 
 
 [ powdery. J 
 
 
 
 * Annales des Mines, 1878, vol. iv. 
 
7 8 CALORIFIC POWER OF FUELS. 
 
 or coke formed, this increase is produced gradually by cutting 
 off the lean coals and dividing the fat coals into three classes 
 gas, forge, and coking. 
 
 Bearing on the advisability of having proximate analyses, 
 as well as ultimate analyses of coal, is the question recently 
 brought up by Mr. Kent, regarding the ratio of hydrogen and 
 carbon in coal. In discussing the results of Lord and Haas' 
 determinations of-Ohio and Pennsylvania coals, he thought he 
 had discovered the ratio, that the fixed carbon is nearly equal 
 to the total carbon minus five times the available hydrogen in 
 bituminous coals, and minus three times the hydrogen in 
 semi-bituminous ones. He gave a table showing results 
 which support the hypothesis. 
 
 LIGNITE. 
 
 From an industrial standpoint lignite is of considerable 
 importance. It occurs in most countries, and is used in a 
 great many for domestic and manufacturing purposes. 
 
 As a fuel it is inferior to coal, being less distantly 
 removed from woody fibre, and hence contains more hydro- 
 gen and, usually, considerable water. Most of the latter, 
 however, dries out on exposure to the air. In some cases 
 as much as 40 or 50 per cent of water is found in the 
 freshly mined lignite, of which at times 20 per cent remains 
 when air-dried. This greatly affects its value as fuel ; still 
 it is used in many of the Western States, and also in 
 Europe. In some European localities, when thoroughly 
 dried and compressed into blocks, especially in Italy and 
 Austria, it is used as fuel for producing gas and for evapo- 
 rating, with good results. In Austria it is burnt without 
 any preparation, except drying in the air for heating salt- 
 pans. 
 
 The amount of ash varies exceedingly, being in some 
 cases as low as 0.9 per cent, and in others as high as 58 per 
 
SOLID FUELS. 79 
 
 cent. It even varies in the same locality and in the same 
 bed. In burning lignite there is considerable loss in the waste 
 gases on account of the large quantity of air introduced, and 
 also from the moisture carried off from the fuel. 
 
 Brix published the following results with dried lignite : 
 
 Water Evap- Per cent 
 orated. Ash. 
 
 Lignite of Aussig, Bohemia 5.8 pounds 15.0 
 
 ' Perleberg, " 5.6 " 6.0 
 
 " Goldfuchs n. Frankfort... 5.5 " 9.1 
 
 " " Rauen 5.4 " 6.3 
 
 Bunte used two kinds of lignite in boiler-tests, and gives 
 the following results : 
 
 Neusattel. Chodan. 
 
 Calories in steam 42.8 49.2 
 
 " "gases 19.6 21. o 
 
 " " aqueous vapor 9.2 8.7 
 
 " "ash 9.0 6.1 
 
 " unaccounted for J 9-4 15.0 
 
 The grate used was a step grate (Treppen-Rost). 
 
 The lignite used on the railways in Italy contained 15 
 per cent of water, and gave a yield of heat equal to one half 
 its weight of coal. 
 
 Analogous to the lignites are certain shales or fossils 
 carrying bitumen. They are sometimes termed boghead 
 cannel, bituminous schist, etc. They are distilled in some 
 localities for oil, but are not much used as fuel. 
 
 Bunte determined the heat of combustion of a sample 
 from Australia, and analyzed one from Scotland. 
 
 Carbon. Hydrogen. O + N. Calories. 
 
 Boghead shale, Australia. 83.17 10.04 6.79 9134 
 Scotch Boghead 81.54 11.62 6.84 
 
 OF THB 
 
 UNIVERSITY 
 
8O CALORIFIC POWER OF FUELS. 
 
 Scotch Boghead generally contains 18 to 24 per cent of 
 ash. From its analysis as above, its heat of combustion 
 should be near that of the other one given. 
 
 PEAT. 
 
 Peat is formed by the agglomeration of vegetable debris, 
 and retains a large amount of water, which will not separate 
 without heat. Its composition varies but little from that of 
 wood, the principal difference being less oxygen and more 
 carbon. 
 
 The composition may be represented by 
 
 Carbon 60 
 
 Hydrogen 6 
 
 Oxygen and nitrogen 34 
 
 100 
 
 The heat of combustion is lower than that of coal or 
 lignite, as might be expected. The quantity of hydrogen 
 exceeds that necessary to form water with the oxygen. 
 
 It is usually dried before using, and when dry becomes 
 quite porous. It carries, however, in this state some 10 to 
 15 per cent of water, which can be expelled only by artificial 
 means. Large quantities of it are converted into charcoal in 
 special kilns, and, where the large amount of ash is no objec- 
 tion, it makes a good fuel. It cannot be used for metallurgical 
 purposes on account of its friability. From 30 to 40 per 
 cent of its weight is left in the charcoal as carbon, but at the 
 same time the ash increases to 15 to 25 per cent, and even 
 more. This consists principally of phosphates and sulphates, 
 with very little carbonates ; hence it is not as apt to clinker 
 as other fuel ashes. 
 
 Brix obtained with peat an evaporative power of 5.11 
 pounds of water. The peat used was from Flatow, and 
 contained 10.7 percent of ash. Another, from Buchfeld-Neu- 
 langen, contained 1.2 per cent of ash, and gave 5.12 pounds 
 
SOLID FUELS. 8 1 
 
 evaporated. Noury, using a special grate, obtained from the 
 Alsace peats 4 to 5 pounds evaporation (ashes deducted). 
 
 Bunte analyzed the gases produced by the combustion of 
 peat on the hearth of a salt-pan, and found, carbonic acid 13, 
 oxygen 6.4, nitrogen 80.6. 
 
 Karsten says that 2\ pounds of peat are equal to one of 
 coal. In some experiments made at St. Petersburg a fire- 
 grate of 32 square feet and 696 square feet of boiler heating 
 surface was used. The peat was compact, hand-moulded into 
 4-inch balls, and dried till moisture did not exceed 14 per cent. 
 4.26 pounds of coal were evaporated for I of peat. 
 
 Crookes and Rohrig, in their " Metallurgy," say: "One 
 pound of dry turf will evaporate 6 pounds of water. Now in 
 I pound of turf, as usually found, there are pound of dry 
 turf and J pound of water. The pound can evaporate 4^ 
 pounds of water; but out of this it must first evaporate the J 
 pound of water contained in its mass, and hence the water 
 boiled away by such turf reduces to 4^ pounds. The yield 
 is here reduced 30 per cent, a proportion which makes all the 
 difference between a good fuel and one almost unfit for use. 
 When turf is dried in the air under cover it still retains -^ of 
 its weight of water, which reduces its calorific power 12 per 
 cent; I pound of such turf evaporates 5j pounds of water." 
 
 COKE. 
 
 Coke usually met with is from three Sources : from gas- 
 coal, and made in gas-retorts; from gas or ordinary bituminous 
 coal, and made in special ovens; from petroleum, and made 
 by carrying the distillation of the residuum to a red heat. 
 
 Coke from gas-works is usually softer and more porous 
 than the other kinds, burns more readily, but does not give 
 as intense a heat. It has been used considerably for domestic 
 heating, and in factories where a high heat is not needed 
 but where a smokeless fuel is desirable. The oven coke is 
 usually in large columnar masses of a close texture and quite 
 
82 
 
 CALORIFIC POWER OF FUELS. 
 
 hard. It has a dead gray-black color and is not susceptible 
 of polish. It is principally used in furnaces requiring a 
 blast, although limited quantities of it have been used in 
 domestic heating, for which purpose it must be broken up 
 much finer than its usual size. Petroleum coke is generally 
 in large irregular lumps, perforated with cavities of greater or 
 less size, the interior of which is usually quite smooth and 
 shining. Its color is blacker than that of gas or oven coke, 
 and its hardness intermediate. It is used principally for mak- 
 ing electric carbons, although considerable quantities are used 
 for fuel. 
 
 With the exception of gas-coke very little use is made of 
 this fuel for steaming, the fire being too intense locally, and 
 hence very apt to burn out the boiler directly over it. In all 
 cases plenty of air is needed to keep up the combustion, which 
 is also a drawback for steaming purposes. For metallurgical 
 furnaces it is different. Here it is almost the ideal fuel, giv- 
 ing an intense reducing heat at just the part of the furnace 
 where most needed. It has been used in iron furnaces for 
 years, and is still the favorite fuel. It is superior to anthracite, 
 as it has no tendency to splinter and crack with the heat, and 
 bears its burden very well. Of course this does not apply to 
 ordinary gas-coke, which crushes easily. 
 
 Coke is essentially carbon, and the mineral portions of the 
 coal from which it is made. It contains small quantities of 
 hydrogen and nitrogen, as may be seen from the tables. The 
 percentage of these, however, is very low, so that the cal- 
 culated and observed heat-units are usually within the limits 
 of error, as is shown in the following table : 
 
 Name. 
 
 C. 
 
 H. 
 
 N. 
 
 Loss. 
 
 Calories 
 observed. 
 
 Calories 
 calculated. 
 
 Authority. 
 
 Sa.arbru.ck . 
 
 98.04 
 98.05 
 98.98 
 
 0-73 
 0.50 
 0.02 
 
 0.25 
 
 1-23 
 1. 2O 
 
 8200 
 8057 
 7901 
 
 8229 
 
 8151 
 8054 
 
 Bunte 
 
 Mahler 
 Berthelot 
 
 Petroleum coke 
 
 
 
 
SOLID FUELS. 
 
 WOOD CHARCOAL. 
 
 Wood charcoal always contains quantities of hydrocarbons 
 which have resisted the action of heat. That called forest 
 charcoal, made by burning in heaps, is the most charged with 
 them ; that obtained from distillation of wood in retorts con- 
 tains less. 
 
 The heat of combustion is very variable. According to 
 Berthier* commercial wood charcoal contains 10 per cent of 
 volatile matters and 2 per cent of ash (carbon 80 to 90, hy- 
 drogen 1.54). 
 
 Pure wood charcoal was first tested calorimetrically by 
 Favre and Silbermann, and since then by several experi- 
 menters. To obtain it pure it was calcined strongly and 
 treated with chlorine to remove all traces of hydrogen. In 
 this state wood-charcoal produces under constant pressure 
 8080 calories, F. & S., or 8100 S.-K. & M.-D. ; with con- 
 stant volume Berthelot and Petit obtained 8137 calories. 
 
 Several years ago Berthier pointed out that half-burnt 
 charcoal, charbon roux or Rothkohle, was superior in combus- 
 tible content to that perfectly burnt. Sauvage has confirmed 
 this, and gives the following results: 
 
 ioo Ibs. of wood (^ 
 charred for ) 
 
 3 hours. 
 
 4 hours. 
 
 5 hours. 
 
 5} hours. 
 
 6 hours. 
 
 Mound 
 Charcoal. 
 
 Weighed 
 
 65.4 Ibs. 
 
 ^.o Ibs. 
 
 47.0 Ibs. 
 
 41. c Ibs 
 
 an i Ibs 
 
 17 2 Ibs 
 
 loocu. ft. measured 
 
 86 cu. ft. 
 
 76 cu. ft. 
 
 58 cu. ft. 
 
 55 cu. ft. 
 
 52 CU. ft. 
 
 33 cu. ft. 
 
 and 
 
 cubic foot wood contained of combustible matter 908 parts. 
 
 883 " 
 904 " 
 
 " 3 hours' heating " 
 
 5 
 
 it j- 1 H it 
 
 a tt 
 
 IO9I 
 
 11 
 
 ti ftl it it 
 
 tt a 
 
 1136 
 
 < t 
 
 " charcoal " 
 
 i i a tt 
 
 1069 
 
 tt 
 
 *Traite des essais par la voie seche, vol. i, p. 286. 
 
84 CALORIFIC POWER OF FUELS. 
 
 So that the amount of combustible matter does not increase 
 after 5 hours' heating, and a continuance of the heat diminishes 
 it. 
 
 The principal use of charcoal is in iron furnaces, where it 
 has been used for years, and produces the highest grades of 
 iron, being free from sulphur and phosphorus. A small 
 amount is used in private dwellings and hotels for heating 
 and cooking. For boiler heating it has been used only 
 experimentally. 
 
 Scheurer-Kestner and Meunier-Dollfus experimented with 
 it in boiler-heating and found very little combustible gas in 
 the products. Beech charcoal was used, and an evaporative 
 effect of 7.62 pounds of water was obtained. The waste 
 gases contained: 
 
 Carbonic acid .:. 11.16 per cent. 
 
 Carbonic oxide o. 37 ' ' 
 
 Oxygen 8.72 " 
 
 Nitrogen 79.75 " 
 
 100.00 
 
 Brix, using wood and peat charcoal, obtained the follow- 
 ing results : 
 
 Wood charcoal 7.55 pounds evaporated. 
 
 Peatcharcoal 6.85 
 
 Schwackhofer burnt charcoal from hard and soft wood in 
 his calorimeter and obtained (constant volume) 7140 calories 
 for the soft charcoal and 7071 calories for the hard. The 
 charcoal in both cases was the ordinary unpurified charcoal as 
 sold. 
 
 WOOD. 
 
 Wood consists of a compact tissue more or less hard, 
 formed of cellulose and a so-called incrusting substance. 
 
SOLID FUELS. 85 
 
 Wood contains, besides, small quantities of mineral matter and 
 hygroscopic water varying from 15 to 30 per cent, according 
 to dryness. Air-dried, it contains about 15 per cent of water, 
 which it gives up easily on exposure to a heat of 100 C. 
 
 The composition of wood may be represented by the 
 
 following : 
 
 Carbon. Hydrogen. Oxygen. Ash. Water. 
 
 Wood dried at 1 00 49.5 6.0 43.5 i.o o.o 
 
 " in the air 29.6 4.8 34.8 0.8 29.0 
 
 Regarding wood from its ultimate composition, we may 
 consider it as a hydrate of carbon, that is, as carbon united to 
 water, the proportion of hydrogen and oxygen being nearly 
 the same as in water. But regarded from its proximate com- 
 position, it is entirely different. What has been said of soft 
 coal can be repeated for wood ; that, those having a similar 
 ultimate composition behave differently in distillation in a 
 closed retort and produce very different proportions of carbon 
 (as charcoal) ; hydrocarbons, liquid or gaseous ; acid products, 
 resin, and tar. It was supposed that the heat of combustion 
 differed also, and this has been verified by experiments. 
 
 Berthelot and Vielle determined the heat of combustion of 
 cellulose, and found 680 calories for the molecular weight of 
 wood, or about 4200 calories per kilogram. 
 
 Hard wood gives less heat than soft wood. According to 
 Gottlieb's experiments, pine-wood has a heat value of 5000 
 calories, while oak gave only 4620 calories. Mahler's exper- 
 iments confirm a difference in favor of pine, but in less pro- 
 portion. 
 
 Two determinations made by Mahler are (cinders and water 
 
 deducted) : 
 
 Fir. Oak. 
 
 Carbon 5 1 .08 50.43 
 
 Hydrogen 6.12 5.88 
 
 Oxygen with trace of nitrogen.. .. 42.90 43-69 
 
 100.00 100.00 
 
 Heat of combustion 4828 4689 
 
86 
 
 CALORIFIC POWER OF FUELS. 
 
 Gottlieb obtained the following numbers, using a calo- 
 rimeter of constant pressure, in which he burnt 2 grams of 
 wood in the space of two or three minutes. The composition 
 of the gas produced was not determined ; he was satisfied 
 that he had perfect combustion, and his figures do not appear 
 very far from the truth. For cellulose he obtained 4155 
 calories. 
 
 Name. 
 
 C. 
 
 H. 
 
 N. 
 
 0. 
 
 Ash. 
 
 Calories. 
 
 B. T U. 
 
 Oak 
 
 CQ. 16 
 
 6. 02 
 
 O.OQ 
 
 43 36 
 
 O. 37 
 
 4620 
 
 8316 
 
 Ash 
 
 4Q. l8 
 
 6.27 
 
 O.O7 
 
 43-QI 
 
 O. e,7 
 
 47 1 1 
 
 8480 
 
 Elm 
 
 4.8. QQ 
 
 6. 20 
 
 O.O6 
 
 44' 25 
 
 0.50 
 
 4728 
 
 8510 
 
 Beech 
 
 4.Q.O6 
 
 6. ii 
 
 O.OQ 
 
 44.17 
 
 0.57 
 
 4774 
 
 8591 
 
 
 48.88 
 
 6.06 
 
 o. 10 
 
 44.67 
 
 0.29 
 
 4771 
 
 8586 
 
 Fir 
 
 CQ. ^6 
 
 c .02 
 
 O.OC, 
 
 4.-1 . -JQ 
 
 0.28 
 
 e.o'JC. 
 
 0063 
 
 Pine 
 
 CO. ^1 
 
 6. 20 
 
 O.O4 
 
 4^.08 
 
 O.37 
 
 co8 e, 
 
 QIC-I 
 
 
 
 
 
 
 
 
 
 Gottlieb's results are 69 calories less than Mahler's for oak 
 and 207 more for fir. 
 
 In burning wood for steaming the fire is easily controlled ; 
 combustion is more complete ; the products of combustion 
 contain only very small quantities of unburnt gases; and the 
 ashes are generally free from carbon. The countries using 
 wood for this purpose are growing less in number yearly, on 
 account of improvement in transportation and the discovery 
 of new coal seams ; w petroleum oils for fuel have also become 
 more common, especially in Russia, the United States, and 
 Canada. 
 
 Morin and Tresca, in their tests, found that one pound 
 of wood was equivalent to 0.368 pound of coal. Scheurer- 
 Kestner's experiments in 1871 show results more favorable 
 for wood. The wood used was Vosges fir, which had been 
 piled under cover for half a year. A cubic foot weighed 
 19.76 Ibs. It was burnt in the same boiler used in his 
 previous experiments, with the result that I pound of wood 
 evaporated 4.4 pounds of water. The ratio was 0.490, or 
 nearly one half that of Ronchamp coal. 
 
SOLID FUELS. 87 
 
 Brix made a number of experiments in using wood for 
 heating, and found that dry pine gave the best results 5 
 pounds per pound of fuel. Elm gave 4.6 pounds; birch, 
 4.6; oak, 4.56; ash, 4.63; and beech, 4.47. 
 
 Wood should be dry as possible, as otherwise it has to 
 furnish heat to vaporize, not only the water formed from its 
 hydrogen, but also that already existing as moisture. We 
 have seen that this loss with coal is considerable, it is still 
 greater with wood. Suppose the wood to be ordinary air-dried, 
 containing 20 per cent of water. If this wood, when per- 
 fectly dry, could evaporate 5 pounds of water, it now has 
 only % of that power, or power to evaporate 4 pounds ; but it 
 already carries -J- of its weight of water, which must be vapor- 
 ized. Hence the available power is 4 pounds less ^ pound = 
 3| pounds, or 76 per cent of its dry value. Hence the 
 economy of using only dried, and even artificially dried, wood. 
 
CHAPTER VIII. 
 LIQUID FUELS. 
 
 SHALE-OILS. PETROLEUM. 
 
 THE mineral oils comprehend the liquid hydrocarbons 
 extracted from bituminous schist or coal and its congeners by 
 distillation, as well as the oils which exist already formed in 
 the earth, and called by the special name of petroleum. 
 
 While the former are seldom employed in heating, petro- 
 leum has become an important fuel in the countries which 
 produce it. Its special qualities, light weight, and low price 
 per calorie compared with other fuels insure a great future. 
 The knowledge of its heat of combustion has become, then, of 
 considerable interest. 
 
 Its ultimate percentage composition varies within rather 
 close limits, yet it is of a very complex proximate composi- 
 tion. The industry of refining crude petroleum extracts from 
 it some 50 per cent of refined oil for use in lamps, and hav- 
 ing a density of 45 to 47 Beaume, boiling-point 170 C. 
 (328 F.); 10 per cent of naphtha with a lower density and 
 boiling-point ; and 20 per cent of paraffin oil of a higher den- 
 sity and boiling-point. 
 
 Crude petroleum contains a large number of hydrocarbons 
 of the general formula C M H 2M+2 , and running from CH 4 to 
 C,,H 34 , with many isometric modifications. The industrial 
 treatment modifies it profoundly. Hydrocarbons containing 
 95 per cent of carbon have been found in the products of 
 distillation.* 
 
 *Wurtz, Dictionnaire de Chimie, Supplement. 
 
 88 
 
LIQUID FUELS. 89 
 
 The first calorimetric experiments were published by Ste.- 
 Claire Deville in 1868 or 1869, using a large calorimeter 
 especially constructed for the work. Mahler used the bomb. 
 The liquids were burnt in the bomb under nearly the same 
 conditions as solids, when they had no appreciable vapor ten- 
 sion. When they had considerable vapor tension (light oils, 
 for instance) Berthelot placed them in a closed vessel, the 
 bottom being platinum and the top formed by a pellicle of 
 gun-cotton. 
 
 Heating by oil is quite recently introduced, but is 
 already developed to a high degree in Russia and on this 
 continent, and is gaining in other localities. The small 
 volume occupied in comparison with its high calorific power 
 renders it a formidable competitor with coal. 
 
 To burn petroleum, atomizers fed by steam or compressed 
 air are used. They generally consist of a horizontal pipe un- 
 der the boiler, fed with oil from an elevated reservoir placed at 
 a presumably safe distance. The steam enters inside the oil- 
 pipe, and, mixing with the oil, throws it into a spray and pro- 
 duces a flame several feet long. At the Chicago Exposition 52 
 tubular boilers were exhibited heated by oil, developing a 
 power of 25000 H.P., and yielding a total evaporation of 12000 
 cubic feet per hour. The oil used was the heavy portion of 
 petroleum (the lighter ones having been distilled off for 
 illumination), and it was fed under a pressure of one-fourth 
 atmosphere. The result was an evaporation of about 15 
 pounds of water per pound of oil. 
 
 In 1889 Albert Hubner ran a whole battery of boilers 
 with oil at his works in Moscow. He used Baku Nafta, or 
 <4 Mazoute," which contained carbon 86.3, hydrogen 13.6, 
 and oxygen o. I per cent. The density was 0.910 to 0.914. 
 
 At Petrolea and Oil City, Canada, the heavy residuum 
 from the stills is used as fuel under boilers and stills. The 
 burners used are very simple, and run without producing 
 smoke. In the United States, the Standard Oil Company has 
 
QO CALORIFIC POWER OF FUELS. 
 
 pushed the sale of fuel-oil made of Ohio crude, and large 
 quantities of it have been used ; large quantities of a special 
 grade are also made for use in enriching water gas. 
 
 The calorific power of petroleum residuum is, according 
 to Sainte- Claire Deville, 11460 calories (20628 B. T. U.), 
 the evaporation at 5 pounds pressure being 15 pounds. This 
 compared with the heat of combustion shows a useful effect 
 of over 86 per cent, while the entire absence of smoke, un- 
 burnt gases, ashes, and irregularity in air-supply add to its 
 advantages still more. 
 
 Some experiments made at the Hecla Engineering Works,. 
 Preston, England, and lasting two days, used a marine boiler. 
 The first day natural draft was used, the second a Korting 
 blower. The oil was blast-furnace oil from Sheffield, and 
 contained : 
 
 Per cent. 
 
 Carbon 83.54 
 
 Hydrogen IO-S9 
 
 Oxygen $.94 
 
 Sulphur 0.09 
 
 100. 16 
 
 By Thompson's calorimeter its value was 16080 B. T. U. 
 
 Equivalent to w^ater at 2 1 2 F 1 6. 66 pounds. 
 
 The results were: First day, 14.97 Ibs. ; second day, 14.21 
 Ibs., a yield of 89.87 and 85.25 per cent of the theoret- 
 ical. 
 
 A series of tests made at South Lambeth with a Cornish 
 boiler showed 20.8 Ibs. evaporation; average of several days, 
 19.5 Ibs. The same boiler with the best Aberdeen coal 
 yielded 6.5 Ibs., an advantage of 3 to I in favor of the 
 oil. 
 
 The following analyses of the waste gases from boilers using 
 oil show how perfect the combustion is, and that little if any 
 excess of air is needed : 
 
LIQUID FUELS. 9 1 
 
 CO, 
 
 14.10 
 
 18.08 
 
 CO 
 
 $.20 
 
 O. 34 
 
 o 
 
 0.78 
 
 0.^4 
 
 Hydrocarbons... . 
 H 
 
 1.30 
 Not determined. 
 
 None. 
 None. 
 
 N., 
 
 78/53 
 
 81.24 
 
 To have the best results, the burner must be so regulated 
 as to have a flame bordering on, but not quite, smoky. Thus 
 sufficient and not too much air is obtained. The quantity of 
 steam needed to atomize the oil at Moscow is 4 per cent of the 
 water evaporated. The use of compressed air has been tried 
 in some places with very satisfactory results : the atomizing 
 is good, but the cost is higher, and the probable chemical 
 effect of the steam is wanting. 
 
 Nothing but a bare mention need be made of animal and 
 vegetable oils, as they are not used in the arts for heating 
 purposes except, perhaps, on very exceptional occasions. 
 The calorific power of all of them is high, as m,ay be seen 
 from Table I. 
 
CHAPTER IX. 
 GASEOUS FUELS. 
 
 THE heat of combustion of gaseous combustibles has been 
 determined for a great many compounds, definite and pure. 
 That of the industrial gases has been determined by different 
 operators and in different ways, with more or less happy 
 results. Its determination is often one of the greatest com- 
 mercial interest, since it is used in domestic heating as well 
 as in industrial appliances, where it is necessary to obtain 
 definite, regular working. It serves also to furnish motive 
 power to gas-engines, in which the heat of combustion is not 
 without importance. Finally, it is well to know the heat 
 produced in air or water-gas apparatus, if we wish to reach 
 the best condition for their production and use. 
 
 For heating steam-boilers gas has given good results and 
 a very high evaporative effect. It is easily regulated, and 
 thus any required heat can be produced by simply turning a 
 valve. No smoke is generated, no soot or deposit of any 
 kind produced in the flues, and no ashes to take out of the 
 ash-pit. The fireplace needs repairing but seldom, and 
 the boiler is Heated evenly and regularly, there being no 
 danger of burning out in strongly heated spots, as no such 
 spots exist. 
 
 In metallurgical furnaces, gas possesses a decided advan- 
 tage in its long, clean, easily managed, intense flame, and this 
 advantage has been long recognized. A flame of 25 feet or 
 more in length is easily produced, and it is practically uniform 
 for its whole extent. Part of the heat usually lost up the 
 chimney can be utilized to heat the air-supply, and no more is 
 supplied than just enough for perfect combustion. 
 
 Using gas as fuel enables the metallurgist to use poor 
 
 92 
 
GASEOUS FUELS. 93 
 
 grades of coal, and all variations in quality may be eliminated, 
 a uniform product being had by storing the gas in a holder, or 
 by making proper arrangement of different generators so that 
 an average will be obtained. In several cases where hand-fed 
 coal fires have been tried against fires burning gas from the 
 same coal, better results have been obtained, due to the possi- 
 bility of more closely adjusted regulation. The tests made 
 at Brieg may be cited. Here each boiler had 141.25 square 
 feet of heating-surface and steam-pressure 6 to 7 atmospheres. 
 No. I boiler was hand-fired ; No. 2 was gas-fired. The 
 evaporation in pounds per pound of fuel was : 
 
 No. 1 8.34 8.74 8.28 4.02 2.569 2.764 
 
 No. 2 9.86 9.73 10.07 5-44 3-251 3.158 
 
 Increase... \%% \2% 20$ 35$ 25$ 
 
 HEAT OF COMBUSTION OF GASES FROM ANALYSIS. 
 
 When the chemical composition of a gas is known exactly, 
 its heat of combustion can be correctly calculated; but in 
 absence of a correct analysis, the calorimeter must be used. 
 
 Knowing the proximate composition of a combustible 
 gas, that is, the proportion of chemically defined components 
 as well as their heats of combustion, it is sufficient to add the 
 numbers obtained for each constituent gas. Take, for 
 example, the analysis of illuminating gas of Manchester as 
 given by Bunsen: 
 
 Hydrogen 45-58 
 
 Marsh gas (CH 4 ) 34-9 
 
 Carbonic oxide 6.64 
 
 Ethylene (C 2 H 4 ). 4.08 
 
 Butylene (C 4 H 8 ) 2.38 
 
 Sulphydric acid 0.29 
 
 Nitrogen 2.46 
 
 Carbonic acid 3.67 
 
 100.00 
 
94 CALORIFIC POWER OF FUELS. 
 
 The calculation is as follows : 
 
 Components. 
 
 No. of Litres per 
 Cubic Metre. 
 
 Weight per Cubic 
 Metre at o and 
 70 mm. 
 Grams. 
 
 Heat of 
 Combustion per 
 Cubic Metre. 
 
 Calculated 
 Calories. 
 
 
 455-8 
 369 
 40.8 
 23-8 
 66.4 
 2.9 
 
 cubic metre 
 
 89.61 
 715.58 
 1251.94 
 2503.88 
 1251.50 
 2551.99 
 
 3066 
 9340 
 14980 
 29042 
 
 3057 
 II4OO 
 
 1395 
 3169 
 611 
 690 
 
 201 
 
 33 
 6099 
 
 Marsh gas, CH 4 
 
 
 
 Sulphydric acid, H 3 S... 
 Total calories per 
 
 
 City of Manchester gas, as analyzed by Bunsen, gives, 
 then, with complete combustion, 6099 calories per cubic 
 metre (685 B. T. U. per cubic foot). 
 
 If, however, only the actual ultimate composition of the 
 gas is known or the total percentage of carbon, hydrogen, 
 oxygen and nitrogen, then the calculated result will differ from 
 the experimental one. This is because the heat units of the 
 elements added together do not make those of the compound, 
 as the heat of combination of the different constituent gases 
 is not allowed for. If this factor is known, then it can be 
 used as a correction and the correct heat determined. 
 
 This heat of combination of the elements to form the 
 component gases will be seen in comparing the calculated and 
 the actual heat <of combustion of the following gases : 
 
 Gases. 
 
 Formulae. 
 
 Carbon. 
 
 Hydro- 
 gen. 
 
 Calculated 
 Heat. 
 
 Actual 
 Heat 
 
 Differ- 
 ence. 
 
 Marsh gas 
 
 CH 4 
 
 75. 
 
 25. 
 
 14685 
 
 iq-ija 
 
 ~F I 34 2 
 
 
 C 2 H 4 
 
 85.7 
 
 14. -i 
 
 Il85Q 
 
 I2I82 
 
 323 
 
 
 C 2 H 2 
 
 02.^ 
 
 7.7 
 
 IOII4 
 
 I2I42 
 
 2028 
 
 Benzene . 
 
 C 6 H 8 
 
 Q2 "I 
 
 7 7 
 
 101 14 
 
 I24IO 
 
 2206 
 
 
 
 
 
 
 
 
 It will also be seen, that although two gases may have the 
 same percentage composition of the elements, yet the heat of 
 combustion may be different owing to the action of the various 
 physical forces at work in molecular condensation, etc. 
 
GASEOUS FUELS, 95 
 
 COAL GAS. 
 
 The heat of combustion of illuminating gas obtained from 
 the distillation of coal in closed retorts is very variable. It 
 depends not only on the nature of the fuel, but also on the 
 rapidity of the distillation and the heat by which it is accom 
 plished. The heat of combustion varies from 5200 to 6300 
 calories per cubic metre. It cannot be represented by any 
 average number. 
 
 According to Witz, at the same gas-works and with the 
 same fuel, yields may occur from 4719 to 5425 calories. 
 According to Bueb-Dessau, the illuminating gas of the same 
 city during the same day will sometimes vary 20 per cent. 
 Dr. Birchmore reports the same result from his examinations 
 of the gas of Brooklyn, N. Y. 
 
 We are not certain that the composition assigned to coal 
 gas by analysis corresponds always to the gas as obtained by 
 distillation ; in Europe, especially, a portion of the heavy 
 hydrocarbons is taken out for sale separately, and the deficiency 
 supplied by cheaper oils. 
 
 From several experiments which he made, Bueb-Dessau* 
 thought that the heat of combustion of illuminating gas was 
 directly proportional to the candle power; but in addition to 
 this being opposed to the theory of heat, the experiments of 
 Aguitton show the contrary. He concluded from his deter- 
 minations that each illuminating gas of different candle power 
 has a definite heat of combustion which corresponds to the 
 intensity of the light. His experiments were carried on with 
 more than a hundred samples, rich and poor, the former kind 
 from cannel coal, the latter from the end of the run carried to 
 an extreme. He represents by the following formula the 
 
 * Bueb-Dessau cites the following among others: 
 
 Candle-power. Heat-value. 
 
 Gas of Dessau 14. 4400 calories 
 
 Gas of Bremen 21.9 5977 
 
 Gas from cannel coal 26.0 6559 
 
g6 CALORIFIC POWER OF FUELS. 
 
 relation between candle power and heat of combustion of a 
 gas: 
 
 c = i X 35 2 -6 + 2280, 
 
 in which c represents the heat of combustion and i the candle 
 power. The formula seems to be applicable only between 
 limits at which it has been verified from 5 to 15 candles. 
 Aguitton's determinations were made with the calorimetric 
 bomb. 
 
 The following table gives a rdsumt of his observations : 
 
 ~ ,, p Heat of Combustion 
 
 5 * 4043 
 
 6 4395 
 
 7 4748 
 
 8 5101 
 
 9 5453 
 
 10 5 806 
 
 ii 6158 
 
 12 6511 
 
 13 6864 
 
 14 72 16 
 
 15 7569 
 
 75 9 4043 _ 352^ coefficient adopted. 
 
 The three samples of illuminating gas, analyzed and burnt 
 in the bomb by Mahler and given in the table below, call for 
 the following observations: Gas from Niddrie cannel coal, the 
 most calorific per cubic metre is the least calorific per kilo- 
 gram, because the density is greater than that of the other 
 two. The richest in hydrogen by volume (Lavillette) is the 
 poorest in calorific power per cubic metre, while the poorest 
 in hydrogen by weight is the richest in calories per cubic 
 metre. These are due to the low density of hydrogen, which 
 
GASEOUS FUELS. 
 
 97 
 
 is less calorific by volume than the other hydrocarbons occur- 
 ring in illuminating gas. 
 
 
 
 Analysis by Weight. 
 
 Heat of Combustion 
 
 
 
 2 
 
 
 
 
 a" 
 
 V 
 
 rt 
 
 
 
 
 t 
 
 
 | 
 
 o 
 
 h 
 
 u 
 
 
 Name. 
 
 
 E 
 
 
 X 
 
 U 
 
 
 s 
 
 rt 
 
 
 
 C eft 
 
 d 
 
 O 
 
 < 
 
 g 
 
 :i 
 
 i 
 
 
 >-, 
 z 
 
 C 
 
 c o 
 
 II 
 
 | 
 
 2 
 
 1 
 
 '5 
 1 
 
 - 
 Kg 
 
 fa 
 
 u 
 
 
 
 
 & 
 
 n y 
 U 
 
 >> 
 
 ffi 
 
 a 
 
 u 
 
 9 
 
 u 
 
 5 rt 
 
 
 
 2 
 
 Niddrie cannel. . 
 
 0.6367 
 
 43-33 
 
 I3-50 
 
 16.84 
 
 9.26 
 
 14.96 
 
 6365 
 
 7735 
 
 Commentry coal. 
 
 o . 4046 
 
 43-74 
 
 21.46 
 
 24.96 
 
 7.08 
 
 5-75 
 
 5834 
 
 1 1 100 
 
 Lavillette gas. . . 
 
 0.4033 
 
 42.25 
 
 21-34 
 
 21.23 
 
 6.83 
 
 8.33 
 
 5602 
 
 10764 
 
 A cubic metre of hydrogen develops 3091 calories in 
 burning; a cubic metre of marsh gas develops 10038 calories; 
 a cubic metre of olefiant gas, 15250 calories. 
 
 GAS OF GASOGENES. 
 
 The gasogenes, instead of transforming the fuel into car- 
 bonic acid and water in a single combustion, produce this 
 change in two distinct burnings, the first being to make a 
 combustible gas and the second to burn this gas with air. 
 
 In the first furnace, the coal, for example, is burnt in such 
 a manner by feeding with an insufficient supply of air that a 
 gaseous mixture is produced, containing principally carbonic 
 oxide, besides nitrogen from the air. As the combustion has 
 been well or poorly managed, it contains a less or greater 
 quantity of carbonic acid, the production of which is avoided 
 as much as possible. This is done by giving to the fuel only 
 just enough air to form carbonic oxide, and not enough to 
 form carbonic acid, even partially, and by making the bed of 
 fuel quite deep. 
 
 The heat produced by this combustion is not used, and 
 consequently an important part of the calories of the coal is 
 lost. Gasogene gas is then lower in calories, and inferior to 
 coal gas, as commonly made by distillation. 
 
98 CALORIFIC POWER OF FUELS. 
 
 One kilogram of carbon burnt to carbonic oxide disen- 
 gages 2489 calories, while I kilogram of carbon burnt to car- 
 bonic acid generates 8137 calories. There is lost, then, in 
 burning carbon to carbonic oxide in a gasogene about 30 per 
 cent of the available calories. 
 
 At first sight this method of working seems irrational, but 
 for obtaining high temperatures there are practical advantages, 
 whose importance far exceeds the loss of heat in the gaso- 
 gene. It permits much more elevated temperatures, and the 
 recovery of a large portion of the heat, which in direct sys- 
 tems of heating in high temperature furnaces passes to the 
 chimney as complete loss. There is actually an economy in 
 the ordinary metallurgical methods even with this loss. 
 
 By means of gasogenes, we produce three kinds of gaseous 
 fuel : the gas called producer or air gas, formed by the incom- 
 plete combustion of the fuel, with production of a mixed gas 
 containing carbonic oxide and hydrogen compounds ; the gas 
 called water gas, from the decomposition of water by carbon at a 
 high temperature, with production of carbonic oxide, hydrogen, 
 and hydrogen compounds ; and the gas called mixed gas, 
 from the mixture of the two preceding ones by a process 
 which combines the production of the two gases in the same 
 furnace. 
 
 % . PRODUCER OR AIR GAS. 
 
 We have said that air gas results from incomplete com- 
 bustion, and that its formation causes a loss of one third of 
 the calories resulting from the complete combustion of the 
 fuel. These gases contain, naturally, the nitrogen of the air 
 used, to which must be added that of the air necessary to 
 change the carbonic oxide and the hydrogen to carbonic acid 
 and water. 
 
 The heat of combustion and the composition determined 
 by different experimenters varies considerably, showing that 
 they did not always work with average samples. 
 
GASEOUS FUELS. 99 
 
 The proportion of nitrogen in these gases reaches 56 to 
 60 per cent ; that of carbonic oxide, 2 1 to 32 per cent ; that of 
 of hydrogen, from traces to 17 per cent. The theoretical 
 calculation for the combustion of carbon in air to a gas con- 
 taining only carbonic oxide and nitrogen gives for the first 
 34.7 and for the second 65.3 per cent. 
 
 By adopting for the composition of air the round numbers 
 79 and 21, and for the weight of oxygen 1.430 grams per 
 litre, for carbon the atomic weight of 12, and for oxygen 16, 
 
 12 : 16 = 1000 grams : 1333 grams. 
 
 A kilogram of carbon needs, then, i-J- kilograms of oxygen. 
 A litre of oxygen weighing 1.430 grams, 1333 grams would 
 occupy 932 litres. These 932 litres will give with carbon a 
 double volume, or 1864 litres carbonic oxide. Multiplying 
 932 litres by the coefficient 4.77 (see Table XIV), we obtain 
 the volume of the air corresponding, or 4445 litres. The 
 gases of combustion will be composed then of these 4445 
 litres of air and the 932 litres of increase in volume, or 5377 
 litres for I kilogram of carbon. The 4445 litres of air will 
 contain (at 79 per cent) 3513 litres of nitrogen, or 65.3 per 
 cent.* 
 
 The calculation is more complicated when we have fuel 
 containing hydrogen, as one portion of the oxygen disappears 
 by its combination with the hydrogen to form water. Take 
 for example, a coal containing 90 per cent of carbon, 5 per 
 cent of hydrogen, and 5 per cent of oxygen. Suppose I 
 kilogram of this coal, under theoretical conditions, burnt in a 
 gasogene, i.e., with perfect transformation of the carbon into 
 carbonic oxide and no residues. This coal contains 900 
 grams carbon, 50 grams hydrogen, 50 grams oxygen. 900 
 
 * One pound of carbon requires 1.333 Ibs. of oxygen; I cubic foot of 
 oxygen weighs 0.08926 Ib. ; 1.333 Ibs. measure 14.93 cu. ft. These would 
 give 2g.86of CO. 14.93 X 4-77 = 71.216, and 71.216 -f 14.93 = 86.146, volume 
 of gases of combustion. These contain 56.26 cu. ft. of nitrogen. 
 
IOO CALORIFIC POWER OF FUELS. 
 
 grams carbon produce 2100 grams carbonic oxide, requiring 
 1 200 grams oxygen. 1200 grams oxygen occupy 839 litres. 
 50 grams hydrogen produce 450 grams water, and require 
 400 grams oxygen. These 400 grams oxygen occupy 279 
 litres. But the coal itself contains 50 grams oxygen, occupy- 
 ing 35 litres. 
 
 We have, then, 839 -j- 279 35 = 1083 litres of oxygen 
 required, and to calculate the amount of air needed multiply 
 by 4.77. This gives 5163 litres of air needed for the incom- 
 plete combustion of I kilogram of carbon. These 5163 litres 
 contain 4080 litres of nitrogen. 
 
 To obtain the total volume of gases produced by the 
 incomplete combustion, we may add to the volume of the air 
 introduced the volume due to the formation of carbonic oxide, 
 and this is equal to the volume of the oxygen used, or 839 
 litres. We have, then, 5163 + 839 = 6002 litres. But a 
 quantity of oxygen has disappeared corresponding to the 
 formation of the water, or 279 35 =244 litres (35 litres 
 exists in the coal as above), and 6002 244 =5758 litres of 
 gas produced by the incomplete combustion of I kilogram of 
 coal. 
 
 Now, then, 5163 litres of air contain 4079 litres of nitro- 
 gen, which would form 1_Z?, or 70.8 per cent of the total 
 
 5758 
 gas. All these numbers are at o and 760 mm. pressure.* 
 
 Generally gasogenes contain less nitrogen, different causes 
 producing diminution, among which are the use of a lower 
 
 *One pound of coal would be 6300 grains carbon, 350 grains oxygen, 
 and 350 grains hydrogen; 0.90 Ib. carbon produces 2.1 Ibs. carbonic oxide, 
 and needs 1.2 Ibs. oxygen; 1.2 Ibs. oxygen occupies 13.44 cu. ft.; 0.050 Ib. 
 hydrogen produces 0.450 Ib. water, and needs 0.400 Ib. oxygen, or 4.48 cu. 
 ft. The 0.05 Ib. of oxygen in the coal occupies 0.56 cu. ft. Then 13.44 + 
 4.480.56=17.36 of oxygen required 17.36X4.77 = 82.81 cu. ft. of air, 
 containing 65.41 cu. ft. nitrogen. Total gases, 82.81 -f- 13.44 3-Q2 = 92.33 
 total volume of gas, and 
 
 65 41 
 
 -2- 70 .8 per cent. 
 
 92.33 
 
GASEOUS FUELS. IOI 
 
 hydrogen coal than we have taken, and the decomposition of 
 the fuel in the body of the furnace with a certain quantity of 
 aqueous vapor formed during the combustion, or from the 
 moisture in the air supplied. 
 
 Mahler determined the heat of combustion of a sample of 
 gas from the Follembray glass-house, and found its composi 
 tion per volume, using coal from Be"thune, to be : 
 
 Marsh gas 2 
 
 Hydrogen 1 2 
 
 Carbonic oxide 21 
 
 Carbonic acid 5 
 
 Nitrogen 60 
 
 100 
 The heat of combustion calculated from its composition is : 
 
 Marsh gas 0.02 X 10038= 200.8 
 
 Hydrogen O.I2X 3091= 370.9 
 
 CO 0.2 1 X 3043 = 639.0 
 
 1210.7 
 With the bomb he found 1212 calories. 
 
 WATER GAS AND MIXED GAS. 
 
 Water gas is produced when water is decomposed at high 
 temperatures by fuels containing but little hydrogen, such 
 as anthracite, charcoal, or coke. Mixed with hydrocarbon 
 vapors, added to enrich it, or which may have been decom- 
 posed with the aqueous vapor, it serves for the illumination 
 of a great number of cities, principally in America. But this 
 is not its only use, as it is used for heating, and also for gas- 
 engines. Mixed with producer gas, it has become a powerful 
 means of heating, especially where high temperatures are 
 wanted. 
 
 Water gas contains but little nitrogen : this is its main 
 distinction from producer gas, and that which gives it a 
 special value from an economical heating point of view. 
 
IO2 CALORIFIC POWER OP FUELS. 
 
 We have previously stated (page 97) that during the 
 combustion of carbon in a gasogene, there occurs a genera- 
 tion of nearly one third of the total heat were the fuel com- 
 pletely burnt. Besides this, the combustion produces a gas 
 containing about one third its weight of combustible gas and 
 two thirds inert gas (nitrogen), which is mixed with it. 
 
 These are important causes of two sources of loss in 
 calories. In an air-gasogene one third of the calories is lost, 
 since the gaseous products give up most of their sensible heat 
 before being used. The 66 per cent of inert gas carries off 
 an enormous quantity of heat to the chimney, and thence to 
 the open air. It was with the idea of regaining or stopping 
 these losses, or at least a large portion of them, that water 
 gas originated. 
 
 Aqueous vapor and carbon, when submitted to a high 
 temperature, produce carbonic oxide and hydrogen. Theo- 
 retically these are free from nitrogen ; but there is always 
 present a small percentage for various causes. In the air 
 gasogene 12 kilogram of carbon and 1 6 kilograms of oxy- 
 gen (atomic weights) unite to form 28 kilograms of carbonic 
 oxide. On the other hand, 12 kilograms of carbon and 18 
 kilograms of water form 28 kilograms of carbonic oxide and 
 2 kilograms of hydrogen. Then I kilogram of carbon fur- 
 nishes 2.5 kilograms of gas composed of carbonic oxide and 
 hydrogen. 
 
 One kilogram of hydrogen has a caloric energy of 29042" 
 calories.* These calories represent also the quantity of heat 
 necessary to decompose the water; in the case of the water 
 gas gasogene they are formed by the carbon burnt. The 12 
 kilograms of carbon will have to furnish, then, the calories 
 necessary to decompose 18 kilograms of water; that is, 
 
 2 X 29042 = 58084 calories. 
 * Water being considered as vapor. 
 
GASEOUS FUELS. 1 03 
 
 But 12 kilograms of carbon, in burning, generate only 
 12 X 2473 = 29676 calories. 
 
 To decompose the water, then, there is a shortage of 
 force of 
 
 58084 29676 28408 calories 
 
 for 2 kilograms of hydrogen, or 14204 calories for I kilo- 
 gram. The heat must be furnished by an external source. 
 In other terms, to gasify I kilogram of carbon there must be 
 supplied 
 
 14204 -T- 6 = 2367 calories. 
 
 As may be easily seen, this operation absorbs much heat, 
 and the combustion of the water gas can give only the calo- 
 ries used at first in forming it. The heat necessary for the 
 decomposition of the water is actually taken from that of the 
 preparatory period of the air gasogene, which makes a loss of 
 one third of the total calories. In burning the water gas 
 made under these conditions we utilize a part of the heat 
 which would have been lost by the air gasogene only. 
 
 The decomposition of water by carbon is not as simple as 
 would appear from the equation 
 
 H a O + C = CO + H a . 
 
 The lower portion of the fuel of the gasogene undergoes 
 ordinary combustion on account of air being present ; while 
 in the upper portion the reaction takes place between the 
 gaseous products formed in the lower portion and the heated 
 carbon. The carbonic acid is then in contact with the heated 
 carbon and is reduced to carbonic oxide : 
 
 C -{ CO, = 2CO. 
 
IO4 CALORIFIC POWER OF FUELS. 
 
 Thus, the reaction with the water would be 
 
 5 H a O + 3 C = 2CO, + CO + IOH ; 
 
 carbonic acid being reduced to carbonic oxide in the final 
 reaction, as in the case with the air gasogene. 
 
 Nine kilograms of aqueous vapor and 6 kilograms of 
 carbon produce I kilogram of hydrogen and 14 kilograms of 
 carbonic oxide, that is, a mixed gas is produced containing 
 about one half its volume of each gas. 
 
 One cubic metre of hydrogen weighs 85.5 grams; one of 
 carbonic oxide, 1194 grams. Then the volumes occupied by 
 each gas would be 11.69 for hydrogen and 11.13 f r car ~ 
 bonic oxide, or 51.23 per cent of hydrogen and 48.77 per 
 cent of carbonic oxide. 
 
 From the foregoing account, it will be seen that the inter- 
 mittent flow is a cause of great loss of caloric in the working 
 of the water gasogene ; but when a gas is wanted solely for 
 heating at high temperatures, it may be obtained by a mixed 
 system working continuously. The gasogene is filled with 
 a mixture of air and steam, the air being employed in 
 the proper proportion to keep up the heat necessary, or, in 
 other words, to furnish by the combustion of part of the 
 carbon, the number of calories necessary to the gasifica- 
 tion of the other part. 
 
 We have seen (page 103) that to gasify I kilogram of 
 carbon 2367 calories were needed. To maintain the heat 
 this quantity must be produced by the action of the air. 
 Mixed gases are poorer than water gas, as they contain more 
 nitrogen and carbonic oxide and less hydrogen. Theo- 
 retically, we should attain the result of furnishing the heat to 
 the gasogene necessary to maintain the temperature by sup- 
 plying the steam sufficiently superheated ; a gas very poor in 
 nitrogen would then be made. But the superheating of 
 steam causes new losses of heat. 
 
GASEOUS FUELS. 
 
 NATURAL GAS. 
 
 Natural gas has been known for thousands of years in 
 Asia, on the Caspian Sea, where it has long been a feature in 
 religious services, but it is only recently that it has become 
 of any use to man and played any part in the fuel world. 
 
 The natural gas output in the United States has attracted 
 considerable attention since 1875, and especially since 1880. 
 This gas always accompanies petroleum, although petroleum 
 does not always accompany the gas. The wells are situated 
 in various portions of New York, Pennsylvania, Ohio, 
 Indiana, West Virginia, Kentucky, Tennessee, Colorado, Cal- 
 ifornia, and on the Canadian side also in numerous locations. 
 
 Natural gas is not of a constant or uniform composition, 
 varying very much according to the locality from which it is 
 taken. The individual constituent gases vary between wide 
 limits, hydrogen at some places being almost wanting, while 
 at others it is as high as 35 or 40 per cent. Marsh gas is in 
 every case the principal constituent, but this runs down as 
 low as 40 per cent in some analyses. Nitrogen is some- 
 times absent, and when present in large amounts, it is suppos- 
 able that the gas analyzed was contaminated with atmospheric 
 air. 
 
 The Ohio and Indiana fields yield gas of nearer a uniform 
 composition than any of the others. The following table is 
 typical: 
 
 
 
 Ohio. 
 
 
 
 Indiana. 
 
 
 
 Fostoria 
 
 Findlay. 
 
 St.Mary's 
 
 Muncie. 
 
 Anderson 
 
 Kokomo. 
 
 
 i 80 
 
 I 64 
 
 I Q4 
 
 2 35 
 
 I 86 
 
 I 42 
 
 
 Q2 84 
 
 Q-7 -3 C 
 
 Q-3 85 
 
 QO 67 
 
 Q3 O7 
 
 Q4..I6 
 
 Olefiant gas 
 
 O 2O 
 
 O 35 
 
 O 2O 
 
 O25 
 
 O/17 
 
 O 3O 
 
 
 O 35 
 
 *-" JD 
 O 3Q 
 
 O 35 
 
 O 35 
 
 O 42 
 
 O. 3O 
 
 Carbonic oxide 
 
 O. 55 
 
 O 41 
 
 O 44 
 
 O.45 
 
 0. 73 
 
 O. 55 
 
 Carbonic acid 
 
 O 2O 
 
 O25 
 
 O23 
 
 O25 
 
 o 26 
 
 O 2Q 
 
 Nitrogen 
 
 o 82 
 
 3J.I 
 
 2 08 
 
 353 
 
 3 O2 
 
 2 80 
 
 Hydrogen sulphide 
 
 0.15 
 
 0.20 
 
 0.21 
 
 0.15 
 
 0.15 
 
 0.18 
 
io6 
 
 CALORIFIC POWER OF FUELS. 
 
 In addition to difference in composition in different local- 
 ities, the composition of the gas varies considerably from 
 time to time in each well. This is shown by the following 
 analyses made at different times within a period of three 
 months from a well at Pittsburgh, Pa. : 
 
 
 1 
 
 2 
 
 3 
 
 4 
 
 5 
 
 6 
 
 j-jyd rocren 
 
 964 
 
 14 d^ 
 
 2O O2 
 
 26 16 
 
 2Q O7 
 
 oc QO 
 
 Marsh gas 
 
 C7 ge 
 
 7C j6 
 
 72 18 
 
 5c 2^ 
 
 60 7O 
 
 AQ ^8 
 
 Olefiant gas 
 
 o 80 
 
 o 60 
 
 0. 7O 
 
 o So 
 
 o 98 
 
 o 60 
 
 
 e. 20 
 
 A 8O 
 
 3.60 
 
 e CQ 
 
 7 Q2 
 
 12 3O 
 
 
 2 IO 
 
 I 2O 
 
 I IO 
 
 o 80 
 
 o 78 
 
 o 80 
 
 
 I OO 
 
 o 30 
 
 I OO 
 
 o 80 
 
 o 58 
 
 
 
 O OO 
 
 o 30 
 
 o 80 
 
 o 60 
 
 O OO 
 
 
 
 2.1. AT. 
 
 2 89 
 
 O OO 
 
 O OO 
 
 O OO 
 
 O OO 
 
 
 
 
 
 
 
 
 The quantity of gas used daily in the town of Findlay, 
 Ohio, in 1890, was estimated by Professor Orton to be, for 
 
 Glass-furnaces 10000000 cubic feet. 
 
 Iron mills 10000000 " " 
 
 Other factories 6000000 *' " 
 
 Domestic use 4000000 " " 
 
 Total per day 30000000 ' ' 
 
 In Indiana, large wells have been opened and used as in 
 Ohio. In Pennsylvania, several of the large rolling-mills and 
 glass-houses near Pittsburg were formerly supplied with mill- 
 ions of feet per day ; but the supply, used so lavishly, became 
 exhausted. In Canada, at Fort Erie and Windsor are wells, 
 the gas from which is piped across the river to Buffalo and 
 Detroit respectively. All through the oil regions gas wells 
 are to be found more or less, accompanying every well sunk. 
 
 From the composition of the gas, it will readily be seen 
 that it is a valuable source of heat, the calorific power reach- 
 ing 10000 calories or 1 100 B. T. U. per cubic foot. It is used 
 for domestic purposes, steam, glass making, iron mills, brick 
 burning, and numerous other ways, and until recently used 
 wastefully in all. 
 
GASEOUS FUELS. IO/ 
 
 As compared with coal, 57.25 pounds of coal or 63 pounds 
 of coke are about equal to 1000 cubic feet of the gas. The 
 actual equivalent in steaming or furnace work varies with the 
 furnace, and probably with the people using it. Equivalent 
 values of 14000 to 25000 cubic feet per ton of coal are 
 reported, and hardly any two users will give the same yield. 
 It seems to be especially adapted to glass-making, giving a 
 long, clean, ashless, smokeless flame, and hundreds of glass- 
 pots were set up in the neighborhood of the wells, especially 
 in Ohio. Each pot consumes from 58000 to 61000 cubic feet 
 per 24 hours in window-glass works and from 31000 to 49000 
 cubic feet in flint-glass works, the difference being of 
 course due to difference in burners and men, the gas being 
 the same. 
 
 In all cases where this gas is used the chief claim made, in 
 addition to those of gases generally, has been cheapness, and 
 it has been sold without any regard to its actual value. A 
 comparison of its value with that of other gases is given by 
 McMillin in the Report of the Ohio Geological Survey, vol. 
 VI, page 544, as follows: 
 
 1000 feet natural gas will evaporate 893 pounds of water. 
 
 " " coal " " " 591 " 
 
 11 " water " " " 262 " " 
 
 " " producer gas " " 115 " " 
 
 OIL GAS. 
 
 There are several processes for producing gas from oil, 
 usually petroleum or its derivatives. Some of them decom- 
 pose the oil by means of heat alone, while others use steam, 
 or steam and air together. The most successful pure oil 
 process is the Pintsch ; this is used extensively in the large 
 cities of Europe and America to obtain a gas for illuminating 
 cars on railways. The gas is made by allowing the oil to fall 
 drop by drop on a strongly heated surface. Complete decom- 
 
108 CALORIFIC POWER OF FUELS. 
 
 position occurs, and a gas of high candle-power is formed. 
 This is collected, and after compression supplied to the con- 
 sumers. It loses some 20 per cent of the illuminating power 
 during compression. As a source of heat, its use is, so far, 
 very limited. An analysis and heat test will be found in the 
 tables. 
 
 The Archer gas process is somewhat similar to the Pintsch, 
 but the products of decomposition are generated at a com- 
 paratively low temperature, and then superheated subse- 
 quently so as to make the gas permanent. This gas is used 
 for metallurgical purposes, but its use for heating boilers is 
 very limited. 
 
 The other gases made with steam or steam and air have 
 been advertised or pushed as fuel gases for several years. 
 Many plants have been established and failed. A few of the 
 most prominent are mentioned in the tables. 
 
 OTHER GASES. 
 
 Gas has been obtained from destructive distillation of 
 wood, rosin, fats, and other materials. They were used prin- 
 cipally for illumination, and seldom if ever for heat. They 
 are now made only in very exceptional cases. 
 
CHAPTER X. 
 
 CALORIFIC POWER OF COAL BURNT UNDER 
 A STEAM-BOILER. 
 
 FUEL USED AND WATER EVAPORATED. 
 
 DISTRIBUTION OF THE HEAT PRODUCED. 
 
 EXPERIMENTS in heating steam-boilers have to deter- 
 mine : 
 
 1. How much water is vaporized by a given quantity of 
 coal, so as to compare it with other coals or fuels ; 
 
 2. The evaporative power of the steam-boiler used; 
 
 3. A comparison of the various styles of grates or meth- 
 ods of heating applied to steam-boilers. 
 
 In this book we will consider only the first case, the 
 others being outside of its scope. 
 
 The knowledge of the heat of combustion of coal and 
 other fuels is closely connected with experiments in heating 
 steam-boilers. It is not enough to know the proportion of 
 water which the apparatus or the fuel tested will vaporize : 
 we must also determine the number of calories lost. We 
 must know, besides, the composition of the coal and its heat 
 of combustion, to determine the proportion of calories used to 
 that possible with perfect combustion. 
 
 The first work in this direction worth mentioning was 
 probably that done by Peclet in 1833, but his results were 
 very crude, and are of no account now. The next were those 
 made by Prof. Johnson, in 1842 and 1843, for the U. S. 
 Navy Department, to determine the steaming powers of the 
 
 109 
 
1 10 CALORIFIC POWER OF FUELS. 
 
 coals then in use. He analyzed and tested some thirty-five 
 different coals, domestic and foreign. The tests were made 
 with a specially built boiler, and careful and copious notes 
 were taken all through. The chimney gases were analyzed, 
 and an attempt made to determine their quantity. In 1891 
 Mr. W. Kent* reviewed his work, and found that, with correc- 
 tions for the constants employed by Johnson, the tests were 
 comparable with those made at the present time. The 
 figures given in the tables as Johnson's are with Kent's 
 corrections. 
 
 The first experiments based on the knowledge of the 
 composition and heat of combustion of coal were published 
 in 1868 and 1869 in the Bulletin de la Soctittf Industrielle 
 de Mulhouse. Scheurer-Kestner remarks in the first part of 
 this work, which he prosecuted later on with assistance of 
 Meunier-Dollfus (loc. cit. p. i): 
 
 "It is necessary to analyze the great difference found 
 between the theoretical heat of combustion (at that time 
 no actual determinations had been made) and the practical 
 yield. 
 
 " Several elements of the calculation aid in making this 
 shortage. The principal ones are : 
 
 " The heat of combustion of the coal; 
 
 " The composition of the coal; 
 
 11 The composition of the cinders as drawn from the 
 ash-pit ; 
 
 "The quantity of water vaporized and the temperature 
 of the steam produced ; 
 
 "The volume of gases introduced under the grate, and 
 their temperature when they leave the boiler to pass into the 
 chimney ; 
 
 "The composition of the gaseous products of combus- 
 tion ; 
 
 * Engineering and Mining Journal, Oct. 1891. 
 
WEIGHT OF FUEL. 1 1 1 
 
 "The temperature of the cinders at the time of dumping; 
 
 " The loss of caloric by radiation from the setting of the 
 boiler." 
 
 We must refer to mineral and organic as well as gas 
 analysis to obtain the necessary elements for the distribution 
 of the caloric produced by the combustion of the coal on a 
 steam-boiler grate. 
 
 To avoid referring to them, we will consider the composi- 
 tion and heat of combustion of coal as known. (See tables-.) 
 
 WEIGHT OF FUEL. 
 
 The coal used in the test should be kept under cover 
 away from moisture and heat, so that the hygroscopic water 
 it contains shall vary as little as possible from the time of 
 taking the sample. Weigh the coal in the gross, and then 
 weigh portions of about 100 kilograms (220 Ibs.) on a scale 
 sensible to -^Vir- 
 
 Where practicable, a box open at the top and holding 
 500 pounds of coal should be provided for each 25 square 
 feet grate area, and in proportion for larger grates. It 
 should be placed on the scales, and conveniently located for 
 shoveling into the fire. 
 
 The exact time of weighing should be noted and the 
 exact weight set down. The weight should be taken at the 
 instant of closing the fire-door. The box should be com- 
 pletely emptied each time. The difference of weight at each 
 firing will give the several quantities fired ; the differences of 
 time will give the intervals between firing; and the differ- 
 ence of time between successive charges will serve as a check 
 on the record c f the test. A chart or diagram should be 
 made showing the regularity of the working, and it is well to 
 keep the records in tabular form ; weights in one column, time 
 in another. 
 
112 CALORIFIC POWER OF FUELS. 
 
 SAMPLING THE COAL. 
 
 In all experiments for determining heat of combustion of 
 fuels, the sampling must be done with the utmost care, espe- 
 cially if the laboratory and working test are to be made at 
 the same time. Samples accurately representing the coal of 
 the working test must be kept in the laboratory, and when 
 coal is tested which contains foreign matter and considerable 
 moisture, too much care cannot be taken to prevent errors. 
 
 The official method of the American Society of Mechanical 
 Engineers is given in the Appendix, and answers the purpose 
 very well. If very large quantities are to be sampled, remove 
 a portion from each cart-load and then re-sample these as per 
 directions above mentioned. 
 
 It is not always necessary to resort to these methods. 
 When the coal comes from the same pit and level, experience 
 has shown that a piece which seems to agree with the general 
 character is usually sufficient. Care must be taken to avoid 
 samples having too much hanging-wall or bed-rock. For 
 twenty years the pure coal of Ronchamp taken from the 
 same pit has given the same calorimetric test, when it con- 
 tained from 10 to 20 per cent of ash. Lord and Haas* 
 showed that the same was true of many American mines, 
 especially in Ohio and Pennsylvania. This being true, we 
 could consider tfiat in sampling we did not sample the coal, 
 but the impurities ; and that a sariiple showing the average 
 impurities would give all that was needed, as we would know 
 what the coal was. 
 
 Care must be taken with regard to the moisture, and any 
 coal showing much external moisture must be examined as 
 near as possible to the original condition. For example, a 
 coal containing 10 per cent of moisture in the pile may, after 
 sampling, crushing, and resampling, lose all but 4 or 5 per 
 cent. If the moisture was determined in this coal while in as 
 
 * Trans. Am. Inst. Min. Eng., Feb. 1897. 
 
ANALYSIS OF COAL. 113 
 
 large pieces as possible, this moisture would all be accounted 
 for. 
 
 In spite of all precautions, samples do not always agree in 
 mineral content with the mass. The difference seems to be due 
 not only to the unequal distribution of the foreign mineral 
 matter throughout the coal, but principally to the difference 
 in specific gravity between the coal and this mineral, so that 
 the purer the coal the more satisfactory the sampling. 
 
 Sometimes a coal is rich in foreign matter, and is contained 
 in a tube open at one end. From this samples may be drawn 
 showing differences of several per cents; as for example, 12.49 
 and 16.74 per cent obtained in two successive cases. The 
 following experiment shows how this happens and how to 
 prevent it : 30 grams of coal, finely pulverized, and contain- 
 ing 20 per cent of mineral, was put into a glass tube, which 
 was closed with a cork and placed vertically, giving it slight 
 taps to settle it down. In a short time most of the foreign 
 material was at the bottom of the tube, the upper portion 
 being nearly free. To avoid such an error the sample must 
 be drawn only after thorough mixing, and without any shaking 
 or jarring of the tube. It is well to use pastilles made up 
 immediately after thorough mixing. A sample containing 
 only 13 to 14 per cent of foreign matter has given from a 
 tube, 12. 20, 12. 81, 13.12, 13.50, 14.42 per cent. 
 
 ANALYSIS OF THE COAL. 
 
 No attempt will be made to treat the methods of ana- 
 lyzing coal ; still, as this usually accompanies a calorimetric 
 determination, some hints may be useful. Scheurer-Kestner 
 usually burns the coal in tubes of white glass placed on an 
 iron gutter. The same tube may thus serve several times if 
 asbestos cloth be placed between the tube and the iron and 
 the cooling be properly regulated. His tubes are 70 to 75 
 centimetres (27 to 29 inches) long and 15 to 20 millimetres 
 
114 CALORIFIC POWER OF FUELS. 
 
 (0.6 to 0.8 inch) inside diameter. They are filled with copper 
 oxide in small pieces, except at the front end, which has a 
 small piece of metallic copper, and at the back, where the 
 platinum boat containing the coal is placed. Usually half a 
 gram is used for a test, the coal having been previously dried 
 at 100 to 105 C. (212 to 221 F.). 
 
 Before putting in the sample the tube is heated to redness 
 and thoroughly dried by means of a current of dry oxygen. 
 The combustion is carried on so as to allow time enough for 
 all the gas to be absorbed by the potash, during the first half 
 of the time the bubbles passing through very slowly. There 
 is no risk then of unburnt gases passing off. An iron or a 
 platinum tube may be used in place of the glass one, but glass 
 allows inspection at all times. 
 
 An analysis should show the carbon, hydrogen, oxygen, 
 nitrogen, sulphur, ash, and moisture, and they should be so 
 given that the carbon, hydrogen, oxygen, nitrogen, sulphur, 
 and ash should equal 100 per cent, the moisture being 
 determined separately, or if preferred all but ash and moisture 
 may foot up 100, and those two be given separately. This 
 latter method is the one which is followed by many of the 
 European engineers, and will be found so in the tables given 
 at the end of this book. If possible the approximate analysis 
 should also be given. 
 
 In determining the moisture too much care cannot be 
 taken to expel all of it. With many coals, and especially our 
 Western ones, the ordinary heating to 110 C. is not suffi- 
 cient. Kent, Carpenter, Hale, and others have investigated 
 this question, and find that a much higher temperature is 
 needed, and must be employed. In some cases as high as 
 140 to 150 C. may be used with safety, and such tempera- 
 tures are recommended by Carpenter, no appreciable amount 
 of volatile matter being driven off. 
 
DURATION OF THE TEST. 
 
 ANALYSIS OF THE CINDERS. 
 
 The cinders and ashes produced by the combustion of the 
 coal are collected so as to weigh and sample them. After 
 drying and determining the water the sample is put into a 
 glass tube as with coal. As the quantity of hydrogen is 
 usually very small, it need not be determined, and the 
 calcination for the carbon can be performed in the open air. 
 The following table contains the results of the tests made 
 by Scheurer-Kestner and Meunier-Dollfus on steam-boiler 
 cinders: 
 
 
 i 
 
 2 
 
 3 
 
 4 
 
 Carbon 
 
 Q 2O 
 
 12 65 
 
 6 77 
 
 8 92 
 
 Hydrogen 
 
 007 
 
 O 29 
 
 O 21 
 
 O27 
 
 Ash 
 
 80 Q5 
 
 86 50 
 
 Q2 6d. 
 
 QI d.2 
 
 
 
 
 
 
 
 99-52 
 
 99-44 
 
 99-58 
 
 99.61 
 
 The proportion of carbon in cinders may be as low as 7 
 per cent, but is usually higher, and 10 to 12 per cent may be 
 called good practice. 
 
 DURATION OF THE TEST. 
 
 A test should continue at least a whole day on account of 
 certain irregularities and causes of error which are constant. 
 The level of the water should be the same at the end of the 
 test as at the beginning, since a slight difference in level 
 means considerable water. 
 
 The condition of the combustion at the time of stopping 
 cannot always be ascertained, and this produces a cause of 
 uncertainty. Another cause is from the temperature of the 
 water in the boiler, and especially in the economizer. On 
 short runs these sources of error cause very faulty results. 
 
Il6 CALORIFIC POWER OF FUELS. 
 
 THE WATER EVAPORATED. 
 
 The feed-water is preferably held in a gauged reservoir, or 
 else weighed, meters not being certain unless checked fre- 
 quently. Use only cold water or water whose temperature 
 will vary but little during the test, so as to avoid corrections 
 of temperature and expansion. The temperature usually 
 varies so little that no account of this variation need be taken. 
 Pump to the boiler with as much regularity as possible, and 
 keep accurate record. 
 
 To have the same level at the end as at the beginning, 
 keep up the initial pressure and feed very carefully. The 
 mean temperature of the feed-water is referred to o C., con- 
 sidering that the specific heat is constant. Otherwise we may 
 use Regnault's formula, 
 
 Q = t o. 00002 f -|- 0.0000003 A 
 
 But when the temperature of the water varies no more than 
 10 degrees, no appreciable error will be made by calling t 
 equal to the temperature. 
 
 TEMPERATURE OF THE STEAM. 
 
 We may measure the temperature of the steam directly by 
 a thermometer in the boiler, or indirectly by observing the 
 pressure. Both methods should be used. . 
 
 To take the temperature directly, the thermometer is 
 placed in an iron tube closed at one end and reaching to the 
 middle of the boiler. The tube should be filled with paraffin 
 or some analogous substance. The temperature of the 
 steam or the water may be taken as desired by changing the 
 position of the thermometer in the tube. See Figure 39. 
 Vertical maximum and minimum thermometers are very use- 
 ful, preventing too hasty observations. 
 
MOISTURE IN THE STEAM. II 7 
 
 To measure the temperature by pressure an air-thermom- 
 eter is used. A registering manometer aids the work consid- 
 erably, as observations should be taken regularly at frequent 
 and equal intervals. The temperature is calculated by means 
 of tables of vapor-tension.* 
 
 MOISTURE IN THE STEAM. 
 
 The percentage of moisture should be ascertained by 
 means of a throttling or a separating calorimeter, directions 
 for the use of which will be furnished by the makers. They 
 should easily and completely separate the water in a manner 
 convenient for measuring, or better, for weighing. It is ad- 
 visable to use two or three at the same time, thus serving as 
 checks for each other. 
 
 " The throttling steam-calorimeter was first described by 
 Professor Peabody in the Transactions,-^ vol. X. page 327, 
 and its modifications by Mr. Barrus, vol. XI. page 790; vol. 
 xvn. page 617; and by Professor Carpenter, vol. XII. page 
 840 ; also the separating-calorimeter designed by Professor 
 Carpenter, vol. XVII. page 608. These instruments are used 
 to determine the moisture existing in a small sample of steam 
 taken from the steam-pipe, and give results, when properly 
 handled, which may be accepted as accurate within 0.5 per 
 cent (this percentage being computed on the total quantity of 
 the steam) for the sample taken. The possible error of 0.5 
 per cent is the aggregate of the probable error of careful ob- 
 servation, and of the errors due to inaccuracy of the pressure- 
 gauges and thermometers ; to radiation ; and, in the case of 
 the throttling-calorimeter, to the possible inaccuracy of the 
 figure 0.48 for the specific heat of superheated steam, which 
 
 * For full details regarding setting up an open-air manometer, see paper 
 by Scheurer-Kestner and Meunier-Dollfus in the Bulletin de la Soci^te 1 in- 
 dustrielle de Mulhouse, 1869, page 241; also Trans. A. S. M. ., vol. VI. 
 pages 281 and 282. 
 
 f Transactions A. S. M. E. 
 
Il8 CALORIFIC POWER OF FUELS. 
 
 is used in computing the results. It is, however, by no means 
 certain that the sample represents the average quality of the 
 steam in the pipe from which the sample is taken. The prac- 
 tical impossibility of obtaining an accurate sample, especially 
 when the percentage of moisture exceeds two or three per 
 cent, is shown in the two papers by Professor Jacobus in 
 Transactions* vol. XVI. pages 448, 1017. 
 
 " In trials of the ordinary forms of horizontal shell and of 
 water-tube boilers, in which there is a large disengaging sur- 
 face, when the water-level is carried at least 10 inches below 
 the level of the steam outlet, and when the water is not of a 
 character to cause foaming, and when in the case of water- 
 tube boilers the steam outlet is placed in the rear of the mid- 
 dle of the length of the water-drum, the maximum quantity 
 of moisture in the steam rarely, if ever, exceeds two per cent ; 
 and in such cases a sample taken with the precautions speci- 
 fied in article XIII. of the Code may be considered to be an 
 accurate average sample of the steam furnished by the boiler, 
 and its percentage of moisture as determined by the throttling 
 or separating calorimeter maybe considered as accurate within 
 one half of one per cent. For scientific research, and in all 
 cases in which there is reason to suspect that the moisture 
 may exceed two per cent, a steam-separator should be placed 
 in the steam-pipe, as near to the steam outlet of the boiler as 
 convenient, well covered with felting, all the steam made by 
 the boiler passing through it, and all the moisture caught by 
 it carefully weighed after being cooled. A convenient method 
 of obtaining the weight of the drip from the separator is to- 
 discharge it through a trap into a barrel of cold water stand- 
 ing on a platform scale. A throttling or a separating calo- 
 rimeter should be placed in the steam-pipe, just beyond the 
 steam-separator, for the purpose of determining, by the 
 sampling method, the small percentage of moisture which 
 may still be in the steam after passing through the separator. 
 
 transactions A. S. M. E. 
 
QUALITY OF STEAM. 1 19 
 
 " The formula for calculating the percentage of moisture 
 when the throttling-calorimeter is used is the following: 
 
 H- h- MTt) 
 w=ioox T- , 
 
 in which w = percentage of moisture in the steam, //" = total 
 heat and L = latent heat per pound of steam at the pressure in 
 the steam-pipe, h = total heat per pound of steam at the pres- 
 sure in the discharge side of the calorimeter, k = specific heat 
 of superheated steam, T= temperature of the throttled and 
 superheated steam in the calorimeter, and t temperature 
 due to the pressure in the discharge side of the calorimeter, = 
 212 Fahr. at atmospheric pressure. Taking = 0.48 and 
 / = 2 12, the formula reduces to 
 
 H- 1146.6 o.48(r 212) 
 w = i oo X - ? - 
 
 CORRECTIONS FOR QUALITY OF STEAM, f 
 
 Given the percentage of moisture or number of degrees of 
 superheating, it is desirable to develop formulae showing what 
 we have termed " the factor of correction for quality of steam," 
 or the factor by which the * ' apparent evaporation, " determined 
 by a boiler-test, is to be multiplied to obtain the " evaporation 
 corrected for quality of steam." It has been customary to call 
 the proportional weight of steam in a mixture of steam and 
 water ''the quality of the steam," and it is not desirable to 
 change this designation. The same term applies when the 
 steam is superheated by employing the " equivalent evapora- 
 tion," or that obtained by adding to the actual evaporation the 
 
 * William Kent in the Report of the Committee on Boiler-tests, A. S. 
 M. E., 1897. 
 
 f C. E. Emery in the Report of Committee on Boiler-tests, A. S. M. E., 
 1897. 
 
120 CALORIFIC POWER OF FUELS. 
 
 proportional weight of water which the thermal value of the 
 superheating would evaporate into dry steam from and at the 
 temperature due to the pressure. "The factor of correction 
 for quality of steam " in a boiler-test differs from the * ' quality " 
 itself, from the fact that the temperature of the feed-water 
 is lower than that of the steam. 
 Let 
 
 Q = quality of moist steam as described above ; 
 Q l = the quality of superheated steam as described above ; 
 P = the proportion of moisture in the steam ; 
 k == the number of degrees of superheating; 
 F= the factor of correction for the quality of the steam 
 
 when the steam is moist * 
 F l = the factor of correction for the quality of the steam 
 
 when the steam is superheated ; 
 
 ff= the total heat of the steam due to the steam-pressure; 
 L = the latent heat of the steam due to the steam-pressure ; 
 T = the temperature of the steam due to the steam-pressure ; 
 T^ = the total heat in the water at the temperature due to 
 
 the steam-pressure;* 
 J = the temperature of the feed water; 
 J l =. the total heat in the feed- water due to the temperature.* 
 
 Therefore, for moist steam, 
 
 Q=i-P, (i) 
 
 P = I -- Q, (2) 
 
 Q + P=* (3) 
 
 See also equation (6). 
 
 * Most tables of the properties of steam and of water are based on the 
 total heat of steam and water above 32 degrees Fahr. For such tables the 
 total heat in the water at a given temperature is equal approximately to 
 the corresponding temperature minus 32 degrees. Exact values should, 
 however, be taken from the tables. 
 
QUALITY OF STEAM. 121 
 
 With both the condensing and throttling calorimeters the 
 water and steam are withdrawn from the boiler at the temper- 
 ature of the steam, and with a separator the water can only be 
 accurately measured when under pressure, so that the difference 
 between the steam and the moisture in the steam, as they leave 
 the boiler, is simply that the former has received the latent 
 heat due to the pressure, and the latter has not. There is, 
 however, imparted to the water in the boiler not only the 
 latent heat in the portion evaporated, but the sensible heat 
 due to raising the temperature of all the water from that of 
 the feed -water to that of the steam due to the pressure. 
 
 In equation (3) the proportional part Q receives from the 
 boiler both the sensible and the latent heat, or the total heat 
 above the temperature of the feed = Q(H /,) thermal units, 
 and the part Pthe difference insensible heat between the tem- 
 peratures of the steam and of the feed-water ~ P(T l J^) 
 thermal units. If all the water were evaporated, each pound 
 would receive the total heat in the steam above the tempera- 
 ture of the feed, or H y,. " The factor of correction for 
 the quality of the steam," when there is no superheating, is 
 therefore 
 
 - , ,, __ 
 
 - Q 
 
 The superheating of the steam requires 0.48 of a thermal 
 unit for each degree the temperature of the steam is raised, 
 so for k degrees of superheating there will be 0.48^ thermal 
 units per pound weight of steam, and the " factor of correc- 
 tion for the quality of the steam " with superheating. 
 
 _ 
 
 See also equation (7). 
 
122 CALORIFIC POWER OF FUELS. 
 
 With the throttling-calorimeter the percentage of moisture 
 P, or number of degrees of superheating, are determined as 
 explained before. 
 
 Since the invention of the throttling-calorimeter the use 
 of the original condensing, or so-ealled barrel, calorimeter is 
 no longer warranted. Accurate results should, however, be 
 obtained by condensing all the steam generated in the boiler, 
 and this plan has been . followed in certain cases. It has, 
 therefore, been thought desirable to add other formulae ap- 
 plicable to condensing-calorimeters. The following additional 
 notation is required: 
 
 W= the original weight of the water in calorimeter, or 
 weight of circulating water for a surface condenser. 
 
 w '= the weight of water added to the calorimeter by blow- 
 ing steam into the water, or of " water of condensation " with 
 a surface condenser. 
 
 t = total heat of water corresponding to initial tempera- 
 ture of water in calorimeter. 
 
 /, = total heat of water corresponding to final temperature 
 in calorimeter. 
 
 Evidently, then : 
 
 W(t l t} = the total thermal units withdrawn from the 
 boiler and imparted to the water in calorimeter. 
 
 W 
 
 (Vj /) = the thermal units per pound of water with- 
 drawn from the boiler and imparted to the water in calorim- 
 eter, from which should be deducted T v /, to obtain the 
 number of thermal units per pound of water withdrawn from 
 the boiler at the pressure due to the temperature T. 
 
 Since only the latent heat L is imparted to the portion of 
 the water evaporated, the quality Q, or proportional quantity 
 evaporated, may be obtained by dividing the total thermal 
 units per pound of water abstracted at the pressure due to the 
 temperature T by the latent heat L. Hence, as given in 
 
QUALITY OF SUPERHEATED STEAM. 123 
 
 Appendix XVII., 1885 Code, with some differences in nota- 
 tion, 
 
 <2 and 0, = J\^(t,-t)-(T. -'. 
 
 The value Q applies when the second term is less than 
 unity. P may be derived therefrom by substitution in equa- 
 tion (2) and F from equation (4). 
 
 <2 4 applies when the second term of the above equation is 
 greater than unity, which shows that the steam is superheated, 
 and, as in this case, the heating value of the superheat has 
 already been measured by heating the water of the calorim- 
 eter; the proportional thermal value of the same, in terms 
 of the latent heat Z, is represented directly by Q l I, and 
 we have as the factor of correction for the quality of the steam 
 with superheating, 
 
 i} L(Q, - i) 
 
 H-J, 
 
 See also equation (5). 
 
 When the quality is greater than I, or equals Q l , the num- 
 ber of degrees of superheating, 
 
 - (8) 
 
 THE QUALITY OF SUPERHEATED STEAM.* 
 
 The quality of the superheated steam is determined from 
 the number of degrees of superheating by using the following 
 formula : 
 
 L + o. 4 8(T-t) 
 
 * G. H. Barrus in Report of Committee on Boiler-tests, A. S. M. E., 
 1897. 
 
124 CALORIFIC POWER OF FUELS. 
 
 in which L is the latent heat in British thermal units in one 
 pound of steam of the observed pressure ; T the observed 
 temperature, and t the normal temperature due to the pres- 
 sure. This normal temperature should be determined by ob- 
 taining a reading of the thermometer when the fires are in a 
 dead condition and the superheat has disappeared. This tem- 
 perature being observed when the pressure as shown by the 
 gauge is the average of the readings taken during the trial, 
 observations being made by the same instrument, errors of 
 gauge or thermometer are practically eliminated. 
 
CHAPTER XL 
 
 AIR SUPPLIED AND GASEOUS PRODUCTS OF COM- 
 BUSTION. 
 
 VOLUME OF AIR NECESSARY TO COMBUSTION. 
 
 Four elements are to be considered in calculating the 
 theoretical volume of air for combustion: carbon, hydrogen, 
 oxygen, sulphur. The last is sometimes wanting in coal, but 
 not usually. 
 
 Carbon. The atomic weights of carbon and oxygen are 
 as 12 and 1 6, and 2 atoms of oxygen are needed to form car- 
 bonic acid with I atom of carbon. Then 
 
 12 : 32 = i : 2.666. 
 
 i kilogram of oxygen occupies 0.699 cubic metre (Table IV); 
 i kilogram of carbon needs 
 
 0.699 X 2.666 = 1.863 cubic metres of oxygen. 
 
 Hydrogen. The atomic weights of hydrogen and oxygen 
 being respectively i and 16, and water being formed of 2 
 atoms of hydrogen and i of oxygen, we have 
 
 2 : 16 = i : 8; 
 
 and as i kilogram of oxygen occupies 0.699 cubic metre, I 
 kilogram of hydrogen requires 
 
 8 X 0.699 = 5.592 cubic metres of oxygen. 
 
 125 
 
126 CALORIFIC POWER OF FUELS. 
 
 Sulphur. The atomic weights of sulphur and oxygen 
 being as 32 to 16, and sulphurous acid containing I atom of 
 sulphur and 2 atoms of oxygen, we have 
 
 32 : 32 = i : i. 
 
 I kilogram of oxygen occupies 0.699 cubic metre; I kilo- 
 gram of sulphur needs, then, to form sulphurous acid 
 
 i X 0.699 0.699 cubic metre of oxygen. 
 
 As most fuels have some oxygen in their composition, we 
 must deduct this at the rate of 0.699 cubic metre per kilo- 
 gram. 
 
 Then multiplying these results by 4.77 (Table XIV) we 
 obtain the number of cubic metres of air required. 
 
 A similar method of calculation will give 
 
 For one pound of carbon 29.86 cubic feet of oxygen. 
 
 " " " " hydrogen 89.60 " " " 
 
 " " " " sulphur 11.20 " " " 
 
 As an example, take a coal containing 90$ C, 5$ H, 3.5$ 
 O, o. \% N, and 0.5$ S. 
 
 C 0.900 X 1.863 = J -677 cubic metres. 
 
 H 0.040X5.592=0.224 
 
 S . . . r, 0.005 X 0.699 = 
 
 Total oxygen 
 
 O . ...0.035 X 0.699 
 
 1.880 
 
 i. 880 X 4-77 = 8.967 cubic metres of air per kilogram of 
 coal; or 143.98 cubic feet of air to the pound of coal. 
 
 This result of course is only approximate, as complete 
 combustion is not attained with coal and solid fuels. With 
 liquid fuels, and especially gases, however, the combustion is 
 usually complete. 
 
VOLUME OF WASTE GASES BY ANALYSIS. 127 
 
 Tables V and VI gives the coefficients to be employed in 
 the calculations. 
 
 Table XIII gives the theoretical quantity of air required 
 for the combustion of various fuels; the actual quantity 
 used depends on the conditions of firing, fuel, etc, and is 
 seldom less than twice the amount shown in the table, except 
 perhaps with gases. 
 
 VOLUME OF WASTE GASES BY ANALYSIS. 
 
 For a long time efforts have been made to determine the 
 quantity of air used by comparison of the analyses of the 
 waste gases with those of the fuel used. Many analyses 
 have been published, but the results showed so little regu- 
 larity, and were so contradictory even, that it was impossible 
 to form any conclusion further than that waste gases from 
 coal may contain at the same time both combustible gas and 
 an excess of air. 
 
 Peclet, in 1827, published the first analyses, made with 
 samples collected from a boiler-stack by means of an inverted 
 flask containing water. Ebelmen, in 1844, published a 
 memoir on the composition of gases from industrial furnaces. 
 He analyzed the gases from a metallurgical furnace, the gas 
 being collected by an aspirator. In 1847 Combes made a 
 report on methods of burning or preventing smoke, giving 
 analyses by Debette. In these the first attempts were made 
 to obtain average samples, they being drawn at certain deter- 
 mined stages of the heat and the fuel. 
 
 In 1862 Commines de Marcilly published analyses of 
 gases from locomotives, as well as from stationary boilers, 
 but the author said the time of collection lasted only a few 
 seconds. In 1866 Cailletet showed that, to obtain correct 
 results, the gas should not be collected till somewhat cooled ; 
 otherwise, on account of dissociation, a larger proportion of 
 combustible gas is found than when cooler. 
 
 But, on account of the defective methods of sampling 
 
128 CALORIFIC POWER OF FUELS. 
 
 used, no conclusion other than that stated above can be 
 drawn from these analyses, and no possible idea can be 
 deduced as to the actual composition of the gases as a whole. 
 When we try to use laboratory methods of control in practi- 
 cal workings, the first necessity is to obtain correct samples 
 for analysis, that is, average samples. In this respect all the 
 above - quoted authors are deficient. The tests made by 
 Scheurer-Kestner, published in 1868, were the first to con- 
 form to this requirement. His samples were drawn by a 
 system analogous in principle to that described for sampling 
 coal. 
 
 It is not always necessary to resort to such a complicated 
 operation in case of a permanent gas; samples taken from 
 the general current by means of an ordinary aspirator or an 
 oil-aspirator (page 132) will usually do if drawn at a sufficient 
 distance from the fire. If the gases have passed through a. 
 long flue, especially one with several bends, they are suffi- 
 ciently mixed, and may be considered as a homogeneous gas. 
 We must remember, however, that as we recede from the 
 fire the infiltration of air, if not prevented, becomes greater. 
 In careful experiments, the method to be described of frac- 
 tionating a large volume is preferable. 
 
 GAS SAMPLER. 
 
 In principle the apparatus consists of a falling-water 
 aspirator, and a second mercury aspirator drawing a small 
 fraction of the gases from the current of the first in a con- 
 stant regular manner and keeping it in a mercury gas-holder, 
 A (Fig. 28), which is a strong glass flask of 3 litres capacity, 
 holding about 40 kilograms (88 Ibs.) of mercury. The 
 gas-holder is connected by the tube a with the tube c for 
 sampling the gas, the flask A and its accessories acting as 
 a Mariotte flask. It is closed at the top by a stopper 
 hollowed out conically below and having holes for two 
 tubes, a and b. This hollowing is to permit filling without 
 
GAS SAMPLER '. 
 
 I2 9 
 
 any air-bubbles. The tubes a and b have glass stop-cocks, 
 but the one in a may be omitted. The manometric tube c 
 shows the pressure. Tube d, like c, passes through a rubber 
 stopper, closing the horizontal tubulature of the gas-holder. 
 
 t 
 
 FIG. 28. GAS SAMPLER. 
 
 FIG. 29. SAMPLER TUBE. 
 
 This tube can be rotated in the stopper to the position shown, 
 or to one 180 from such position. The flask is graduated on 
 the side into millimetres. Tube a fits the hole of the stopper 
 tightly, and can be moved up or down as desired to suit the 
 quantity of gas in the flask. All joints are covered with 
 paraffin, tube a being greased to facilitate movement. 
 
 Fig. 29 shows the gas sampling tube. It consists of a 
 platinum cylinder, rs, 10 millimetres (0.4 inch) diameter and 
 700 millimetres (27.5 inches) long, having a longitudinal slot 
 of several centimetres length. The end r is closed with a 
 
J3O CALORIFIC POWER OF FUELS. 
 
 platinum cap ; the end s is soldered to a copper tube, sy, pass- 
 ing into a Liebig condenser having two tubes, 00', for the 
 water. In most cases the platinum tube may be replaced 
 without trouble by one of copper, or even iron, the platinum 
 being necessary only when the gases are drawn at a tempera- 
 perature high enough to cause oxidation of the other metals. 
 With iron or copper a portion of the oxygen is removed in 
 the passage through the tube. 
 
 The tube ry is open at/, and has a side tube h. Aspira- 
 tion is carried on through the opening in the platinum tube. 
 A movable rod, ik, carrying a platinum scraper is attached 
 to one end of the tube, and moves in the slot to clean it, as 
 occasion requires, from soot, etc. The disk/) serves to hold the 
 cement used in fastening it to the stack or chimney, and pre- 
 vents ingress of external air. The rod mn passes through a 
 caoutchouc bearing fastened between the disks / and q. 
 
 Fig. 28 represents a front view of the apparatus. Fig. 30 
 represents a side view in elevation. The tube ry is intro- 
 duced through an opening made for the purpose in the 
 masonry, the part rs being exposed inside. The end y, is 
 connected with a lead pipe, v, by a rubber tube; this pipe is 
 soldered to another one, yz. On opening the cock y t water 
 flows from a reservoir and empties at z. Suction in yrs 
 should amount to several millimetres of mercury, and is regu- 
 lated by the cocks/ and x controlling the water-flow, and also 
 by the length of yz. The gas drawn in by yvx may be meas- 
 ured by collecting it at z, and should amount to 4 or 5 litres 
 (25 to 30 cubic inches) per minute. 
 
 The gas-holder is supported by a piece of sheet iron with 
 upturned edges forming a shelf. Any mercury spattered 
 over or spilled is thus easily collected. The mercury tank is 
 supported from the wall of the chimney in such position as to 
 facilitate refilling the flask through a siphon. The tubes dd' 
 serve to feed the condenser. 
 
 While the current is passing through yr a small quantity 
 
GAS SAMPLER. 
 
 is drawn out by the tube /*, and this should be so regulated 
 by the cock d that only from ^\-^ to -j-J-^- is collected. 
 
 Whenever the level of the mercury lowers, it shows a 
 
 FIG. 30. GAS SAMPLER. 
 
 clogging in the slot, and it should be cleaned by moving the 
 rod. This always indicates when cleaning is necessary, and 
 it sometimes keeps clean for hours. 
 
 When a sufficient sample has been obtained turn up the 
 tube d, and then the gas-holder can be carried away. 
 
 The method recommended by the American Society of 
 Mechanical Engineers is to have a "box or block of gal- 
 vanized sheet iron equal in thickness to one course of brick," 
 and secure in it a series of J-inch gas-pipes, all alike at the 
 ends and of equal lengths, in such manner that the open ends 
 may be evenly distributed over the area of the flue A (Fig. 
 32), and their other open ends enclosed in the receiver B. 
 
 OF THB 
 
 UNIVERSITY 
 
132 
 
 CALORIFIC POWER OF FUELS. 
 
 FIG. 31. OIL ASPIRATOR. 
 
 If the flue-gases be drawn off from the receiver B by 
 four tubes, CC, into a mixing-box, 
 Dy beneath, a good mixture can be 
 obtained. Two such samplers, one 
 above the other, a foot apart, in the 
 same flue will furnish samples of 
 gases which show the same compo- 
 sition by analysis. 
 
 The oil gas holder (Fig. 31) con- 
 sists of a bottle tubulated at the 
 bottom and connected with the sup- 
 ply of gas at the upper opening. It 
 may contain some 10 litres (600 
 cubic inches), and is filled with 
 water having on it a layer of 10 
 centimetres (4 inches) of oil. The 
 water running out from the tubu- 
 lature at the bottom draws the gas 
 in at the top. The stopper at the top has two openings, 
 through one of which passes a funnel-tube, through which 
 water may be poured to expel the gas when portions of it 
 are needed. The gas then passes out by the same tube 
 through which it was drawn into the bottle. 
 
 With all kirxis of aspirators or gas holders especial care 
 must be taken to prevent entrance of air into the flue after 
 leaving the fire, since the correct analysis will show not only 
 the quantity of unburnt gases, but also the excess of air, and 
 any mixture of outside air will vitiate the result and cause 
 faulty deductions as to the working of the fire ; and conse- 
 quently the waste calories. 
 
 To prevent this, all joints in the masonry must be exam- 
 ined and repaired if necessary. In case of dampers, which 
 must be used, the bearings can be made in stuffing-boxes, as 
 recommended by Burnet. Generally, the gas can be sampled 
 before it arrives at a damper, as the course of the boiler-flue 
 
GAS SAMPLER. 
 
 133 
 
 is usually sufficient to cause a thorough mixing of the gases. 
 In case there are several dampers, the first one may be dis- 
 pensed with for the time being. 
 
 When the gases are taken quite near the fire, they must be 
 drawn very slowly in order to gradually cool them down and 
 
 FIG. 32. 
 
 avoid dissociation. In this case a stoneware tube may be 
 used for suction. If this precaution is neglected the gases 
 collected may be entirely different from those passing off at 
 the chimney. Metal tubes are inadmissible, since they 
 abstract oxygen, and hence cause a change in composition. 
 
 ANALYSIS OF THE GASES. 
 
 The collected gases contain nitrogen, oxygen, carbonic 
 acid, carbonic oxide, hydrocarbons, and occasionally free 
 hydrogen. To determine all these a eudiometric method 
 
134 
 
 CALORIFIC POWER OF FUELS. 
 
 must be used ; but usually only the oxygen, carbonic oxide, 
 and carbonic acid are required. In normal combustion with 
 sufficient air the quantity of hydrocarbons is very trifling, and 
 need not be considered. This occurs usually with a supply 
 of 15 cubic metres of air per kilogram (240 cubic feet per 
 pound) of coal, and should produce a waste gas containing 10 
 to 14 per cent of carbonic acid, in which case the unburnt 
 hydrocarbons amount to less than I per cent. 
 
 The Orsat apparatus or its modifications may be used to 
 determine the oxygen, carbonic acid, and carbonic oxide. By 
 using Winckler's modification the hydrocarbons may be deter- 
 mined. For exact analyses of the gases the Hempel apparatus 
 may be used. For general work, however, the Orsat appa- 
 ratus or -the Orsat-Muencke is the best and most easily 
 transported and handled. Directions for using this apparatus 
 need not be given here, as they can be found in all works on 
 gas analysis, or can be had of the dealers. 
 
 The following table gives analyses made by Scheurer- 
 Kestner of waste gases from Ronchamp coal. The gases for 
 examination were collected by means of the apparatus described 
 above (pp. 128^ seq.} and shows the average for. a whole 
 day's run. 
 
 
 Percentage Composition of the Gases. 
 
 p 
 
 o 
 
 io 
 
 
 . 
 
 U 
 
 8, 
 
 9 
 
 
 
 
 
 
 
 
 T3 
 
 
 <u 
 
 a 
 
 Hydrocarbons. 
 
 3 
 
 l5 
 
 U 
 
 83 
 
 
 
 
 
 
 
 (j 
 
 o 
 
 8 
 
 
 <; 
 
 
 
 
 
 . 
 
 
 
 
 M 
 
 H 
 
 c 
 
 1 
 
 .a 
 
 I 
 
 c 
 
 u 
 
 1 
 
 | 
 
 c 
 
 1 
 
 Sjfj 
 
 "o 
 
 O 
 
 c 
 
 ^ 
 
 * 
 
 6 
 
 X 
 
 
 
 3 
 
 U 
 
 ffi 
 
 o^ 
 
 u 
 
 1 
 
 1" 
 
 6.60 
 
 80.38 
 
 14.87 
 
 I.4I 
 
 0.84 
 
 1. 15 
 
 1-35 
 
 Lbs. 
 8.19 
 
 Lbs. 
 15-4 
 
 5' 
 
 10.47 
 
 80.60 
 
 14.16 
 
 2.18 
 
 0.97 
 
 0.98 
 
 I. II 
 
 9.625 
 
 30.8 
 
 8' 
 
 I3.32 
 
 80.66 
 
 14.63 
 
 2.80 
 
 0.86 
 
 0.49 
 
 0.56 
 
 9.625 
 
 15-4 
 
 4' 
 
 17.61 
 
 81.52 
 
 13-34 
 
 3-77 
 
 0.86 
 
 0.46 
 
 O.gi 
 
 8.19 
 
 15.4 
 
 3' 
 
 20.94 
 
 80.23 
 
 13-43 
 
 4.42 
 
 0.24 
 
 0.32 
 
 I.4I 
 
 8.19 
 
 30.8 
 
 10' 
 
 26.18 
 
 80.34 
 
 12.89 
 
 5-53 
 
 0.24 
 
 0.28 
 
 0.96 
 
 4.71 
 
 15.4 
 
 8' 
 
 42.84 
 
 79.76 
 
 10.87 
 
 8.99 
 
 0.24 
 
 0.19 
 
 0.19 
 
 18.94 
 
 15-4 
 
 2' 
 
 53.78 
 
 79.86 
 
 8.23 
 
 11-35 
 
 0.24 
 
 o 04 
 
 O.52 
 
 3.41 
 
 13.2 
 
 10' 
 
GAS SAMPLED. 
 
 135 
 
 The following table gives some analyses by Bunte of gas 
 samples from coal burnt in his experimental apparatus at 
 Munich : 
 
 
 Mm. and 
 Max. 
 of Air. 
 
 CO, 
 
 CO 
 
 H 
 
 
 
 N 
 
 
 
 10.26 
 
 O 53 
 
 O.OI 
 
 IO.OO 
 
 7Q.2O 
 
 Do 
 
 
 16.45 
 
 I Q4 
 
 1.45 
 
 1.52 
 
 78.64 
 
 Do 
 
 
 i^ 40 
 
 o 48 
 
 o. 30 
 
 6.52 
 
 VQ.^O 
 
 Do 
 
 
 11.45 
 
 1.22 
 
 0.78 
 
 7.27 
 
 70.28 
 
 Do (grate more open) 
 
 
 8 15 
 
 O IO 
 
 O.OI 
 
 1 1. 60 
 
 80, 14 
 
 Do Do 
 
 
 6.12 
 
 O.8q 
 
 O.IO 
 
 14.21 
 
 78.68 
 
 Coal from Saarbruck: Koenig.. 
 " " Tremosna: Bohemia 
 11 Hausham: Bavaria. 
 " " Miesbach: Bavaria. 
 
 j Min. 
 \ Max. 
 Min. 
 Max. 
 Min. 
 Max. 
 j Min. 
 1 Max. 
 1 Min. 
 
 15 12 
 7.07 
 
 13.78 
 
 7-94 
 10.48 
 
 5-71 
 11.46 
 
 5 42 
 17.48 
 
 1.09 
 
 0.18 
 
 4.69 
 
 0.03 
 0.07 
 
 0.14 
 
 0.07 
 0.03 
 
 1. 21 
 
 I. O2 
 
 o.oo 
 o. 16 
 0.09 
 0.19 
 0.08 
 0.07 
 
 O.O2 
 
 0.06 
 
 2.64 
 
 12.57 
 
 I.IO 
 
 11.03 
 9.28 
 
 14.86 
 
 8.66 
 15.00 
 
 3-13 
 
 80.13 
 80.25 
 80.27 
 80.91 
 79.98 
 79.21 
 79-74 
 
 79-53 
 78.12 
 
 " the Ruhr: General 
 
 1 Max. 
 j Min. 
 1 Max 
 
 12.20 
 16.45 
 
 3QC 
 
 ? 
 1-94 
 
 o 06 
 
 0.30 
 1.45 
 
 o oo 
 
 7.87 
 1.52 
 
 16 41 
 
 ? 
 78.64 
 
 70 eg 
 
 " the Ruhr : Gelsen- 
 
 j Min. 
 ( Max. 
 
 10.46 
 
 5.44 
 
 O.I I 
 O 12 
 
 O.II 
 
 O IO 
 
 8.58 
 14.15 
 
 80.74 
 8O. IQ 
 
 " " Saarbruck : Saint- 
 
 Min. 
 Max. 
 
 10.73 
 7.48 
 
 0.15 
 
 O.O7 
 
 0.30 
 
 O.IO 
 
 7.36 
 
 II. QI 
 
 81.46 
 80.44 
 
 " Saarbruck: Mittel- 
 bexbach . 
 
 j Min. 
 ( Max 
 
 13-30 
 
 8 44 
 
 0.61 
 o 19 
 
 0.33 
 
 o 16 
 
 4-13 
 
 10 58 
 
 81.63 
 80 63 
 
 " " Saarbruck : Heinitz 
 " " Saarbruck: mixed.. 
 ' " Bohemia 
 
 j Min. 
 I Max. 
 j Min. 
 / Max. 
 j Min. 
 
 14.62 
 
 6-49 
 IO.22 
 8.21 
 I5-50 
 
 2 07 
 0.07 
 0.22 
 0.04 
 0-74 
 
 1. 00 
 
 0.06 
 0.07 
 
 O.O2 
 
 0.33 
 
 2.07 
 12.70 
 8.57 
 10.64 
 1.67 
 
 80.24 
 80.68 
 80.92 
 81.09 
 81.66 
 
 < i i 
 
 "j Max. 
 ( Min. 
 
 8.48 
 9.6l 
 
 0.08 
 
 o. 16 
 
 0.07 
 0.08 
 
 9.69 
 9-47 
 
 81.68 
 80.68 
 
 " " Saxony 
 
 ( Max. 
 j Min. 
 
 7.00 
 
 13.80 
 
 O. II 
 
 0-33 
 
 0.05 
 0.30 
 
 12.70 
 4-36 
 
 80.14 
 
 81.21 
 
 Silesia 
 
 "j Max. 
 j Min. 
 
 7 .60 
 II-4 
 
 0.16 
 o 15 
 
 0.09 
 0.04 
 
 11-53 
 7.45 
 
 80.62 
 81.22 
 
 " " Bavaria : Peissen- 
 
 | Max. 
 ] Min. 
 { Max. 
 
 8.07 
 13.96 
 
 7.85 
 
 O.IO 
 
 1.46 
 
 O.O7 
 
 0.09 
 
 0.79 
 
 O. 13 
 
 10.73 
 2-93 
 10.57 
 
 Sl.OI 
 80.86 
 81.38 
 
 
 jMin. 
 
 14.91 
 
 1.04 
 
 0.60 
 
 2.92 
 
 80.53 
 
 Coke from Saarbruck 
 
 \ Max. 
 j Min. 
 
 6.36 
 14.87 
 
 o. 16 
 0.13 
 
 0.23 
 
 0.09 
 
 13.15 
 4.16 
 
 80.10 
 80.75 
 
 
 ( Max. 
 
 8.01 
 
 0.03 
 
 o.oo 
 
 10.87 
 
 81.09 
 
 The data in the above table show that when air to the 
 amount of 15 cubic metres and over per kilogram (200 cubic 
 
136 CALORIFIC POWER OF FUELS. 
 
 feet per pound) is used, corresponding to a maximum of 14 
 per cent of carbonic acid in the waste gases, the loss in hydro- 
 gen is very small. With 12 per cent of carbonic acid the 
 hydrogen loss amounts to only a few thousandths. 
 
 CALCULATION OF THE VOLUME FROM ANALYSIS. 
 
 To calculate this volume, determine the weight of carbon 
 in a unit of volume, and knowing the weight of carbon fur- 
 nished by the coal, determine the volume corresponding to 
 the unit of weight. The unit of volume for the gas is the 
 cubic metre, and the unit of weight, the kilogram. 
 
 Carbon exists in the waste gases as carbonic acid, carbonic 
 oxide, and hydrocarbons ; when we do not know the compo- 
 sition of the hydrocarbons, we consider the carbon and hydro- 
 gen as free, and that the carbon is in the state of vapor. 
 
 To determine the weight of carbon contained in these 
 different gases, reduce their volumes to kilograms, and by 
 means of their molecular (or equivalent) weights and that of 
 carbon make the calculation. 
 
 i litre of CO a at o and 760 mm. weighs 1.966 grams. 
 T '* " CO <4 il ' ' *' *' tl I 2^1 t( 
 I " " C vapor " " " 1.072 
 
 Molecular weight of carbon 12 
 
 " CO, 44 
 
 " CO 28 
 
 The weight of a volume v of carbonic acid is v X 1.966, 
 and as 44 of carbonic acid contain 12 of carbon, then the 
 weight of carbon would be as 44 : 12 or as 11:3. Then 
 
CALCULATION OF THE VOLUME FROM ANALYSIS. 137 
 
 The weight of carbonic oxide of volume v' is 1. 251^', and 
 as 28 of carbonic oxide contains 12 of carbon, the ratio be- 
 comes 28: 12 = 7:3. We then have 
 
 The weight of a volume of carbon vapor is v" X 1.072. 
 
 To calculate the weight of carbon in a cubic metre of gas r 
 multiply the added volumes of CO 3 and CO by the coefficient 
 0.536. Multiply the volume of carbon vapor by 1.072, and 
 add this product to that obtained above. The sum is the 
 weight of carbon per cubic metre, 
 
 C = 0.536(z; + V 1 ) + 1.072V". 
 
 If the gas contains, per cubic metre, 60 litres of carbonic 
 acid, 10 of carbonic oxide, and I of carbon vapor, we will 
 have 
 
 c = 0.536(60 + 10) -{- 1.072 X I = 38.592 grams carbon. 
 
 From the ratio of carbon of the coal consumed and that in 
 the gas the volume of combustion gases is deduced. 
 
 To calculate this, subtract the carbon of the cinders from 
 that of the original coal. If the coal contains 81 percent 
 carbon and leaves 6 percent of cinders containing 10 percent 
 of carbon, then the amount of carbon burnt will be 
 
 81 (o.io X 6.0) = 81 0.6 = 80.4. 
 We then have 
 
 38.592: 1000= 804:20.830 litres. 
 
 A kilogram of coal produces, then, 20.83 cubic metres of gas 
 at o and 760 mm. 
 
 The general formula is 
 
 v _ Cc 
 
 " (v + v')o. 536+1 .0721;" ' 
 
138 CALORIFIC POWER OF FUELS. 
 
 in which 
 
 V = volume of waste gases at o and 760 mm. in cubic metres; 
 v = " " CO 3 in litres per cubic metre of gases; 
 
 v"= " " carbon vapor per cubic metre of gases ; 
 
 C = weight of carbon in grams, contained in i kilogram of 
 
 coal; 
 c = weight of carbon in grams, contained in cinders from I 
 
 kilogram of coal. 
 
 NOTE. The above calculation in English units would be as follows: 
 
 Weight of i cubic foot of carbonic acid o. 12274 lb. 
 
 " " " " oxide 0.07811 " 
 
 " " carbon vapor 0.06693 " 
 
 v X 0.12274 X 3 
 
 ii 
 v' X 0.07811 X 3 
 
 = 0.0335Z/. 
 = 0.0335*/. 
 
 7 
 
 0.06693^" = weight of carbon in vapor. 
 C o.0335(z/ -f- ' 
 
 1000 cubic feet of gases having 60 cubic feet of CO 2 , 10 cubic feet of CO 
 and i cubic foot of C vapor would give 
 
 C = 0.0335(60 -J- 10) 4- 0.06693 X i = 2.412 Ibs. carbon. 
 I pound of coal has 80.4 per cent carbon; then 
 
 2.412 : looo =0.804 : 333^ cubic feet of gases produced from i Ib. of coal. 
 The general formula is 
 
 r. ^-^4- 
 
 in which 
 
 V = volume in cubic feet of gases produced; 
 
 v =. " of CO 2 in cubic feet per 1000 cubic feet; 
 
 v' = " " CO " " " " 
 
 v" = " " carbon vapor in cubic feet per 1000 cubic feet; 
 
 C = weight of carbon in coal in thousandths of a pound; 
 
 c = " " " " cinders per pound of coal in thousandths. 
 
CALCULATION OF VOLUME OF AIR SUPPLIED. 139 
 
 CALCULATION OF VOLUME OF AIR SUPPLIED. 
 
 The volume of combustion-gases just determined is less 
 than that of the air supplied. Oxygen in forming carbonic 
 acid produces a volume equal to itself; hence there is no 
 change. 
 
 C + O, = CO, 
 
 2 VOls. 2 VOls. 
 
 Oxygen in forming carbonic oxide produces twice the 
 volume. 
 
 C + O = CO 
 
 I VOl. 2 VOls. 
 
 Hence there is an increase in volume. 
 
 Carbon vapor and hydrogen as free gases or as hydro- 
 carbons increase the volume but slightly. In forming sul- 
 phurous acid with sulphur there is no change of volume. 
 
 s + o, = so, 
 
 2 VOls. 2 VOls. 
 
 Another slight cause of increase is setting free the nitrogen 
 of the coal ; but this is inappreciable. I per cent of nitrogen 
 forms only o. I per cent of the entire volume of gases formed. 
 
 It might be said that, excepting the oxygen changing to 
 water and disappearing by condensation, all the modifications 
 of gaseous volume may be neglected, the increase being more 
 than compensated by the loss due to oxygen. This elimina- 
 tion of oxygen must be allowed for, however. 
 
 A coal containing 4 per cent of hydrogen requires eight 
 times such weight to form water, or 40 grams of hydrogen 
 need 320 grams of oxygen. I litre of oxygen weighs 1.430 
 grams, then 320 grams measure ^~ =223.7 litres (7.9 cubic 
 feet). (Or I Ib. of such coal would need 3.6 cubic feet of 
 oxygen.) 
 
 These 223 litres must be added to the volume of the 
 waste gases produced by the coal to obtain the original 
 
I4O CALORIFIC POWER OF FUELS. 
 
 volume of air introduced. A coal containing 5 per cent of 
 hydrogen would use 279 litres. 
 
 The volume of oxygen needed for various percentages of 
 hydrogen is as follows : 
 
 Per kilo of coal. Per Ib. of coal. 
 \% hydrogen uses of oxygen 55.9 litres, 0.9 cubic feet. 
 
 2 " " " 112 " 1.8 " " 
 
 3 " " " 168 " 2.7 " 
 
 4 " " " 223 " 3.6 " " 
 
 5 " " ft 279 " 4.5 " " 
 Calling H the per cent of hydrogen, the formula given 
 
 above becomes 
 
 / __ C-c' _ 
 V/ = (v 4-^)0.563+ i. 
 or 
 
 Cc f 
 V/ = 
 
 0.0335(^+2/0 + 0.06693^' " 
 
 To make this applicable to normal air saturated with 
 moisture at o C. and 760 mm. (32 F. and 29.922 inches) 
 containing 0.4 per cent of CO a , we must divide by 99.12, 
 the composition of air being: 
 
 Nitrogen .................... ............. 78.35 
 
 Oxygen ...... , ........................... 20. 77 
 
 Water ........ ," ........... , ........ 0.84 
 
 Carbonic acid , 0.04 r 
 
 100.00 
 And 100 0.88 = 99. 12. The formula then becomes 
 
 tf __ C-c' _ 
 V// = (v+ 2/00.567 + 1.0806*;" + 55-9 H, 
 or 
 
 C-S 
 
 n 
 V ' ~ 
 
 0.0337^ + z/) + 0.06752^ 
 
CALCULATION OF WEIGHT OF WASTE GASES. 14! 
 
 CALCULATION OF WEIGHT OF WASTE GASES FROM 
 ANALYSIS.* 
 
 Two methods of calculating from the analysis by volume 
 of the dry chimney gases the number of pounds of dry chim- 
 ney gases per pound of carbon, or the weight of air supplied 
 per pound of carbon, have been given by different writers. 
 These may be expressed in the shape of formulae as follows: 
 
 (A) Pounds dry gas per pound C = 
 
 (B) Pounds air per pound C = $.% 2(C 
 
 Formula A may be derived from the method of computa- 
 tion given in Mr. R. S. Hale's paper on " Flue Gas Anal- 
 yses," Transactions A. S. M. E. r vol. XVIII. p. 901, and 
 formula B from the method given in Peabody and Miller's 
 Treatise on Steam-boilers. Both are based on the principle 
 that the density, relatively to hydrogen, of an elementary gas 
 (O and N) is proportional to its atomic weight, and that of a 
 compound gas (CO and CO 2 ) to one half its molecular weight. 
 Both formulae are very nearly accurate when pure carbon is 
 the fuel burned ; but formula B is inaccurate when the fuel 
 contains hydrogen, for the reason that that portion of the 
 oxygen of the air-supply which is required to burn the 
 hydrogen is contained in the chimney gas as H 2 O, and does 
 not appear in the analysis of the dry gas. 
 
 The following calculations of a supposed case of combus- 
 tion of hydrogenous fuel illustrates the accuracy of formula A 
 and the inaccuracy of formula B : Assume that the coal has 
 the following analysis: C, 66.50; H, 4. 55 ; O, 8.40; N, i.oo; 
 water, 10.00; ash and sulphur, 9.55; total, 100. Assume 
 
 * William Kent in Report of Committee on Boiler-tests, A. S. M. E., 
 1897. 
 
142 
 
 CALORIFIC POWER OF FUELS. 
 
 also that one tenth of the C is burned to CO, and nine tenths 
 to CO,; that the air supply is 20 per cent in excess of that 
 required for this combustion ; that the air contains one per 
 cent by weight of moisture ; and that the S in the coal may 
 be considered as part of the ash. We then have the follow- 
 ing synthesis of results of the combustion of 100 pounds of 
 coal : 
 
 O from N = Total rr . rn TT n 
 
 Air. O X JJ. Air. "a H ' 
 
 59.85 Ibs. C to CO a X 2$ 159-60 534.31 693.91 219.45 .......... 
 
 6.65 " C to CO X ii 8.87 29.70 38.57 ...... 15.52 ..... 
 
 3.50 " H to H 2 O X 8 28.00 93.74 121.74 ........... 31.50 
 
 196.47 657.75 854.22 ................ 
 
 1.05 " H to H 2 ) 
 8.40 " H to H 2 O f 
 10.00 " Water ............................. 10.00 
 
 i. oo " N ...... i. oo ...................... 
 
 9.55 " Ash and S ................................. 
 
 100.00 .................................. 
 
 Excess of air 20 per cent. 39.29 131.55 170.84 ................ 
 
 ............ 1025.06 ................ 
 
 Moisture in air i per cent .............................. 10.25 
 
 Total wt. of gases, 1125.67 = 39.29 790.30 ...... 219.45 15.52 61.20 
 
 Total dry gases, 1064.56 
 
 O N C0 a CO 
 
 Total dry gases, by weight, % 3.69 74.24 ...... 20.61 1.546 ..... 
 
 Total dry gases, by volume, % 3.508 80.656 ...... 14.252 1.584 ..... 
 
 Total gases 1125. 76 + ash and S 9.55 = 1135.31 total products. 
 
 Total air 1025.06 -f- moisture in air 10.25 + coal 100 = 1135.31. 
 
 Dry gas per pound coal 10.6456; per pound carbon = 10.6456 -f- 665 = 16.008. 
 
 Dry air per pound coal 10.2506; per pound carbon = 10.2506 -f- 665 = 15.414. 
 
 Computation of the weight of dry gas and of air per pound C: 
 
 Formula A : 
 
 14.252X11 + 3.508X8 + 82.240X7 
 Dry gas per pound C = - :--= - - -- - - - = 16.008 pounds. 
 
 3(14.252 + 1.584) 
 
 Formula B : 
 
 Air per pound C = 5.8 
 
 The error in the last result is 15.414 13.589 = 1.825 pounds. 
 
WASTE GASES BY THE ANEMOMETER. 143 
 
 Prof. Jacobus recommends the use of the formula 
 
 ;N 
 
 Pounds of air per pound C = / rrt , rn x -5- 0.77 ; 
 
 3v^^ a i *A/J 
 
 and in the case given above, where the actual quantity used 
 was 15.414 per cent, his calculated one is 15.434 per cent, 
 practically the same, and as near as errors of analysis would 
 allow a calculated result. 
 
 VOLUME OF WASTE GASES BY THE ANEMOMETER. 
 
 The fan-wheel anemometer is an instrument to measure 
 the force or rapidity of a current of gas. It consists of a 
 fan-wheel rotated by the moving gas, and which transmits 
 such motion to an index showing the number of revolutions. 
 Burnat used this apparatus to measure the quantity of air 
 passing in under the grate of steam-boilers. 
 
 The coefficient to be used in calculating the flow is differ- 
 ent for each machine, and must be determined by actual 
 experiment. Burnat's formula, 
 
 v = o. 120 + o. 130/2, 
 
 means that the velocity is found by multiplying the number 
 of revolutions per second by 0.130 and adding 0.120 to the 
 product. 
 
 To obtain satisfactory results with the anemometer, it 
 must be placed in the axis of a perfect cylinder at the depth 
 of a metre, as the indications vary with the position in the 
 flue. The formula needs correction for temperature, but the 
 correction of the apparatus much exceeds this. Burnat com- 
 pared his results with those obtained from a formula depend- 
 ing on the depression if under the grate (see page 147), and 
 found differences of not more than 5 per cent. 
 
144 
 
 CALORIFIC POWER OF FUELS. 
 
 FLETCHER'S ANEMOMETER. 
 
 Fletcher's anemometer (Fig. 3$) is used in England to 
 ascertain the speed of flow in chimneys and flues. In its 
 simplified form it is quite serviceable. It is based on the 
 movement of a column of ether in a U-tube. 
 
 The ends of the glass tubes a, b are placed in the flue a 
 little less than one sixth of its diameter. The straight end a 
 
 FIG. 33. FLETCHER'S ANEMOMETER. 
 
 should be parallel to the direction of the current, the end b 
 being at right angles to this. Hunter proposed bending 
 both ends in opposite directions, to obviate the error caused 
 if the tubes were not so placed. These tubes communicate 
 with the ether tube cd. The draught across the tubes causes 
 the ether to rise in a by aspiration and to fall in b by pres- 
 sure. The difference of level is read, and then the tubes are 
 turned around 180, so as to reverse their positions, and the 
 difference of level read again. The sum of the two differ- 
 ences is called the anemometer reading, and by means of 
 tables the velocity of the current is ascertained. 
 
 The same trouble is common to all anemometer methods. 
 The flue feeding the fire receives only the air passing in 
 
HI RAr'S METHOD. 
 
 145 
 
 under the 
 
 FIG. 34. 
 
 SEGUR GAUGE. 
 
 grate. Whatever passes in by the doors or 
 through cracks escapes accounting. On account 
 of this it is certain that the calculations based on 
 anemometer readings are lower than th al 
 
 air supply. 
 
 SEGUR'S DIFFERENTIAL GAUGE. 
 This gauge (Fig. 34) consists of a U-tubeof 
 J-inch glass, surmounted by two chambers of 2 J 
 inches diameter. Two non-miscible liquids of 
 different colors, usually alcohol and paraffin oil, 
 are put into the two arms, one occupying the 
 portion AB, the other the portion BCD. The 
 movement of the line of demarcation is pro- 
 portional to the difference in area of the chambers 
 and the tube adjoining. A movement of 2 
 inches in the column represents J-inch difference 
 pressure or draft. 
 
 HIRN'S METHOD. 
 
 The apparatus used by Burnat as a check on his own 
 calculations was devised by Hirn, and is based on the formula 
 of the rate of flow of compressed gases from a reservoir, 
 friction being neglected. The coefficient of reduction used 
 is 0.9, the one given by Dubuisson in his treatise on hydraulics. 
 
 The main difficulty consists in measuring the difference of 
 pressure of the atmosphere in the ash pit and that outside, 
 for the depression in the flues in some cases does not exceed 
 a few millimetres of water. Hirn's apparatus removes this 
 difficulty. 
 
 Burnat describes it as follows : 
 
 When making a test the doors of the ash pit are removed 
 and replaced by a piece of sheet iron, A (Fig. 3^]*, which com- 
 pletely shuts out all access of air except through the opening 
 in the middle, to which is fitted the pipe CD, 13.8 inches 
 
146 
 
 CALORIFIC POWER OF FUELS. 
 
 diameter and 59 inches long. A tube leads from the front 
 to the apparatus E, devised by Hirn, placed on a table or 
 against the boiler-wall. This apparatus consists of a little 
 gas holder whose upper surface is just one decimeter (3.9 
 
 
 FIG. 35- 
 
 inches) on a side. Inside this and above the water level the 
 tube A opens. The bell dips into a vessel of water and is 
 suspended from a balance arm. 
 
 The balance being in equilibrium when the atmospheric 
 pressure acts on both sides of the bell, if the interior is con- 
 nected with the ash-pit the weight needed to restore equili- 
 brium will give a measure of the difference in pressure. The 
 weight of half a gram (7.7 grains) represents one-twentieth 
 millimetre (0.002 inch) of water. 
 
 The formula'adopted by Hirn is 
 
 = 5X0 
 
 V : 
 
 x 0.76(1 + 0.0037*), 
 
 0.0013.5 
 
 in which 
 
 V volume of air introduced under the grate in cubic 
 
 metres ; 
 5 = section in square metre of pipe-opening leading air to 
 
 the ash-pit ; 
 0.9 = coefficient of reduction; 
 
DASYMETER. 147 
 
 h = difference of pressure expressed in height of water; 
 B = barometric pressure in the room ; 
 
 t = temperature of the room ; 
 g = acceleration of gravity = 9.8088 metres. 
 
 VOLUME BY AUTOMATIC APPARATUS. 
 DASYMETER. 
 
 Siegert and Durr * devised an apparatus called the 
 Dasymeter, which has been introduced in several large works 
 in Europe, where it gives satisfaction. 
 
 It consists of a balance enclosed in a cast-iron box with 
 a glass side (Fig. 36). At one end of the beam is a very 
 
 FIG. 36. DASYMETER. 
 
 light glass balloon holding 2 to 3 litres, sealed by fusion. 
 The other end carries a weight balancing the balloon. This 
 weight is formed of a U-tube, //, containing mercury, and is 
 open at one end; the other end is expanded into a bulb con- 
 taining air, which is submitted to the variations of pressure 
 and temperature through the mercury. If the pressure of 
 the air increases or diminishes, the mercury rises or falls, and 
 increases or diminishes the weight on the lever. Suppose an 
 
 * Oesterreichische Zeitschrift filr B.- und H.-Wesen, xvi. p. 291. 
 
148 CALORIFIC POWER OF FUELS. 
 
 increase of pressure and a lowering of temperature which 
 would diminish the density of the air one half. A corres- 
 ponding quantity of mercury passes into the arm of the tube, 
 and the original compensating weight is diminished by that 
 amount. A graduated index shows the variations of weight, 
 and hence the variations of density in the gases. An inge- 
 nious arrangement allows regulation by rotating the U-tube 
 on the axis pn. The tube is turned slowly around till 
 adjusted, thus changing the length of the lever-arm. 
 
 A difference of I per cent of carbonic acid causes a differ- 
 ence in weight of 20 milligrams. One litre of air at o and 
 760 millimetres weighs 1294 milligrams; I litre of carbonic 
 acid weighs 1967 milligrams; the difference is 673 milligrams. 
 If the gas contains I per cent of CO 2 , each litre increases 6.73 
 milligrams in weight; and as the balloon contains 3 litres, it 
 supports an external pressure of more than 3 X 6.73 = 20.19 
 milligrams (0.311 grains). 
 
 To prevent action of sulphurous acid the bearings are 
 made of sapphire, onyx, bloodstone, etc., and metallic parts of 
 phosphor-bronze. 
 
 To set up the dasymeter, connect pipe e with the boiler- 
 flue before the damper; the tube pleads to the chimney. By 
 this means a current of gas passes through the box, and shows 
 at any time the* percentage of carbonic acid. .Siegert gives 
 the following results obtained with it, and the corresponding 
 results by analysis : 
 
 j Dasymeter, 13.0, 13.0, 12.0, 6.25, 2.2, 16.3, 7.5, 12.5 
 2 1 Analysis, 13.0, 12.7, 12.2,6.00,2.0, 16.0,8.0, 13.0 
 
 ECONOMETER. 
 
 H. Arndt has invented what he calls the " Econometer" 
 (Fig. 37), which is on a similar principle.* It consists of a 
 tight cast-iron shell, NN, containing a gas-balance. A pipe, 
 
 * Zeitschrift des Vereines Deutscher Ingenieure, xxxvu. p. 801. 
 
ECONOMETER. 
 
 149 
 
 v'y 0.4 inch in diameter leads to the inside of the flue before the 
 damper; a second pipe, z/', communicates with the interior of 
 the. same flue beyond the damper. In the interior, the tube i' 
 is connected to the upright pipe f t which leads the gas to bell 
 /, and the tube i' to the tubulure g. i' and i" are of rubber. 
 
 FIG. 37. ECONOMETER. 
 
 The balance is very sensitive, the beam carrying at one 
 end the gas-holder e' , open below and containing about 30 
 cubic inches, and at the other end a second holder of similar 
 size and weight as the first. Attached to the bottom of this 
 one is a pan to hold the balancing weights. 
 
 The tube/" conducts the gas to the balloon /, which, open 
 below, is freely movable in the cylinder g, by which it pro- 
 duces suction in the tube i" . 
 
 Carbonic acid being heavier than common air (1.96 to 
 1.29) as well as the other associated gases, it follows that the 
 density of the gases passing through the tubes depends on the 
 carbonic acid content. The scale is divided so that each 
 division shows one per cent of CO 2 in the gases. 
 
150 
 
 CALORIFIC POWER OF FUELS. 
 
 GAS-COMPOSIMETER. 
 
 The gas-composimeter of Uehling is an apparatus for 
 automatically and continuously determining the quantity of 
 carbonic acid contained in waste gases. 
 
 It is based on the laws governing the flow of gas through 
 small apertures. 
 
 B 
 
 G ' 
 
 FIG. 38. 
 
 If two such apertures, A and B (Fig. 38), form respectively 
 the inlet and outlet openings of chamber C, and a uniform 
 suction is maintained in the chamber C f by the aspirator D r 
 the action will be as follows : 
 
 Gas will be drawn through the aperture B into the cham- 
 ber C f , creating suction in chamber C, which in turn causes 
 gas to flow through the aperture A. The velocity with 
 which the gas enters through A depends on the suction in the 
 chamber C, and the velocity at which it flows out through B 
 depends upon the excess of the suction in chamber C' over 
 that existing in chamber C, that is, the effective suction in C'. 
 As the suction in C increases, the effective suction must 
 decrease, and hence the velocity of the gas entering at A 
 increases, while the velocity of the gas passing out through B 
 decreases, until the same quantity of gas enters at A as passes 
 
TEMPERATURE OF THE WASTE GASES. \*>\ 
 
 out at B* As soon as this occurs no further change of suc- 
 tion takes place in the chamber C, providing the gas entering 
 at A and passing out at B be maintained at the same tem- 
 perature. 
 
 If from the constant stream of gas, while flowing through 
 chamber C, one of its constituents is continuously removed by 
 absorption, a reduction of volume will take place in chamber 
 C and cause an increase in suction, and consequently a de- 
 crease in the effective suction in C'. Hence the velocity of 
 the gas through A will increase, and the velocity through B 
 will decrease, until the same quantity of gas enters at A as 
 is absorbed by the reagent, plus that which passes out at 
 aperture B. 
 
 Thus every change in the volume of the constituents we 
 are absorbing from the gas causes a corresponding change of 
 suction in the chamber C. 
 
 The apparatus is connected with a regulator, a manom- 
 eter, and automatic recording register. 
 
 TEMPERATURE OF THE WASTE GASES. 
 
 As in analyzing coal, cinders, and gases we must have 
 average samples, so in treating of waste gases we need average 
 temperatures. It is not enough to take the temperature 
 occasionally with the thermometer; it varies too much from 
 time to time, even if the readings are taken frequently. We 
 must have some method of obtaining the average temperature 
 of the gas current, and this can be accomplished by means of 
 a heat reservoir introduced into the flue. 
 
 For this purpose one was devised by Scheurer-Kestner of 
 a type which has been repeatedly copied and modified. It 
 consists of an iron tube, bb (Fig. 39), placed in the flue so 
 that the upper end, covered with an insulating material, is let 
 into the wall to about one half its thickness, the remainder 
 hanging free in the flue. This tube is filled with paraffin, 
 
152 
 
 CALORIFIC POWER OF FUELS. 
 
 and in this is inserted the thermometer. The large mass of 
 the paraffin is acted on by the mean temperature, but is unin- 
 fluenced by any slight momentary changes which may occur. 
 A self-registering thermometer is very advantageous, but 
 readings at intervals of half an hour are sufficient ordinarily. 
 Of course the opening around the tube should be packed so 
 as to prevent all possible ingress of cold external air. 
 
 FIG. 39. FLUE THERMOMETER. 
 
 Occasionally mercury is used instead of paraffin. This 
 renders the average of the heat more exactly, perhaps, but 
 has the disadvantage of being much heavier and much more 
 expensive. There are also many difficulties in handling it 
 which do not obtain with paraffin. The paraffin should be 
 well refined, and have a high melting-point. 
 
 THE PNEUMATIC PYROMETER. 
 
 Uehling's pneumatic pyrometer is based on a principle 
 analogous to that of the gas-composimeter, and is now in use 
 in many places, automatically measuring the temperatures of 
 chimneys and furnaces for all temperatures up to 3000 F., 
 and registering the same on cards. The apparatus has been 
 tested at the Stevens Institute of Technology, and the 
 indications pronounced reliable. It cannot be safely used 
 
THE PNE UMA TIC P YROME TER. 1 5 3 
 
 continuously for temperatures above 2500, but at that tem- 
 perature and lower it works well and satisfactorily for months 
 without requiring any readjustment. The automatic register 
 is very sensitive, and can be easily adjusted for a new range of 
 temperatures at any time. 
 
 An explanation of the principle of its working is given in 
 the inventor's own words: 
 
 1 ' The Pneumatic Pyrometer is based on the laws govern- 
 ing the flow of air through small apertures. 
 
 "If two such apertures A and B (Fig. 38) respectively 
 form the inlet and outlet openings of a chamber C, and a uni- 
 form suction is created in the chamber C' by the aspirator D, 
 the action will be as follows : 
 
 "Air will be drawn through the aperture B into the 
 chamber C' , creating suction in chamber C, which in turn 
 causes air from the atmosphere to flow in through the aper- 
 ture A. The velocity with which the air enters through A 
 depends on the suction in the chamber C, and the velocity 
 at which it flows out through B depends upon the excess of 
 suction in C' over that existing in the chamber C, that is, the 
 effective suction in C' . As the suction in C increases, the 
 effective suction must decrease, and hence the velocity at 
 which air flows in through the aperture A increases, and the 
 velocity at which air flows out through the aperture B de- 
 creases, until the same quantity of air enters at A as passes 
 out at B. As soon as this occurs no further change of suc- 
 tion can take place in the chamber C. 
 
 "Air is very materially expanded by heat. Therefore 
 the higher the temperature of the air the greater the volume, 
 and the smaller will be the quantity of air drawn through a 
 given aperture by the same suction. Now if the air as it 
 passes through the aperture A is heated, but again cooled to 
 a lower fixed temperature before it passes through the aper- 
 ture B, less air will enter through the aperture A than is 
 drawn out through the aperture B. Hence the suction in C 
 
154 CALORIFIC POWER OF FUELS. 
 
 must increase and the effective suction in C' must decrease,. 
 and in consequence the velocity of the air thiough A will 
 increase and the velocity of the air through B will decrease, 
 until the same quantity of air again flows through both aper- 
 tures. Thus every change of temperature in the air entering 
 through the aperture A will cause a corresponding change of 
 suction in the chamber C. If two manometer-tubes p and q, 
 Fig. 38, communicate respectively with the chambers C and 
 C' , the column in tube q will indicate the constant suction in 
 C' and the column in tube/ will indicate the suction in the 
 chamber C, which suction is a true measure of the tempera- 
 ture of the air entering through the aperture A. 
 
 DETERMINATION OF THE CARBON IN SMOKE. 
 
 SOOT or black forms from quick cooling of the hydro- 
 carbons, temporarily dissociated by high temperatures. Fuels 
 having no hydrogen as hydrocarbons, never produce smoke ; 
 pure charcoal, coke, or graphite never smokes. Soft coal, on 
 the contrary, produces more as the air-supply grows less. 
 
 Sainte-Claire Deville proved that a compound gas when 
 heated sufficiently separates into its elements ; a sudden cool- 
 ing now will give a simple mixture instead of the original 
 combination. A slow cooling, however, reproduces the 
 original gas. Berfhelot proved, on the other hand, that new 
 compounds are formed on heating the hydrocarbons to high 
 temperatures, a part of the carbon being deposited as soot. 
 These two phenomena undoubtedly go on together in smoke 
 production.* 
 
 If a metal tube be put in the gas current over a grate at 
 a short distance from the fire, the hottest gases will be col- 
 
 *Bunte gives some analyses of smoke-black: 
 
 C H 
 
 I ,...,.., 97.2 2.8 
 
 2 97-3 2.7 
 
 3 98.5 1.5 
 
DETERMINATION OF THE CARBON IN SMOKE. 155 
 
 lected. Pass a stream of cold water through a pipe in this 
 gas-current and a large quantity of black will be deposited. 
 On stopping the water flow and inclining the tube a little 
 the carbon disappears gradually, and when the temperature 
 of the tube attains that of the gas, no black will be deposited. 
 Cool it again, and more black forms immediately. 
 
 Combustion gases meet with surfaces relatively cold in 
 the boiler sides or flues, or even in colder currents of gas or 
 air passing in through the grate. This produces a quick cool- 
 ing, and consequent formation of black. 
 
 Experiments made at Mulhouse in 1859 by Burnat 
 showed an advantage gained in steaming by producing smoke, 
 rather than introducing too great excess of air. The experi- 
 ments showed that the loss in carbon was quite small, and 
 these results have been confirmed by others since. E. R. 
 Tatlock of Glasgow finds 60 per cent combustible matter in 
 soot, and obtained 51.46 grains per cubic foot of furnace 
 gases. 
 
 To determine the amount of carbon in smoke, Scheurer- 
 Kestner used a glass organic analysis apparatus, the tube 
 having in the middle loosely packed asbestos for about 8 
 inches, which was kept in place by platinum spirals. One 
 end was drawn out to connect with the absorption apparatus, 
 and the other end placed in the flue. After igniting and 
 cooling the asbestos the small end is connected with an 
 aspirator and the gas drawn slowly through. The carbon is 
 all stopped by the asbestos, which becomes black for a short 
 distance. When sufficiently collected, dry the tube at 100 
 C., heat to redness, and pass a stream of oxygen through it, 
 collecting the carbonic acid formed. 
 
 As an example Scheurer-Kestner gives the following: 
 
 Waste gases, reduced to o and 760 mm. 86 litres. 
 Time of sampling I hour. 
 
CALORIFIC POWER OF FUELS. 
 
 Composition of gas : 
 
 CO 3 8. 5 per cent. 
 
 Excess of air 53.4 
 
 Nitrogen and residue 38. 1 
 
 CO 2 from the combustion 0.070 gram. 
 
 Equivalent to carbon 0.019 " 
 
 By the analysis of the gases and that of the coal the 
 quantity of air consumed was calculated. Knowing the 
 volume of air used for the coal, its composition, and the pro- 
 portion of carbon as black in the gases, the loss due to such 
 formation was calculated. 
 
 Kind of Coal. 
 
 Waste Gases per 
 Pound of Coal. 
 
 Black. 
 
 Per Cubic Foot 
 of Gas. 
 
 Per Cent Calories 
 of Heat of 
 Combustion. 
 
 
 cubic feet. 
 135 
 143 
 169 
 184 
 189 
 205 
 
 163 
 217 
 
 233 
 
 278 
 
 293 
 129 
 
 155 
 
 grains. 
 15-43 
 7.41 
 0.72 
 
 6.74 
 1.19 
 2.03 
 20.49 
 6.79 
 5-71 
 648 
 3.70 
 i. 08 
 6.64 
 
 I.I 
 0.6 
 0.07 
 
 0.2 
 O.I 
 O.I 
 2.1 
 
 0.8 
 0.7 
 
 I.O 
 
 o 6 
 
 O.I 
 
 0.8 
 
 
 i 
 
 < 
 
 , 
 
 , 
 
 
 
 
 
 
 
 . 
 
 Miesbach 
 
 
 
 Under the most unfavorable conditions for feeding the 
 air, the loss due to formation of black does not exceed 2 per 
 cent, even with smoky coal. Ronchamp coal gave the fol- 
 lowing results : 
 
 Feeding 240 cubic feet of air per pound of coal gave a 
 gas containing 8.5 per cent of carbonic acid, excess of air 53 
 per cent, and loss of carbon as black 0.485 per cent. 
 
 Feeding 112 cubic feet of air per pound of coal gave a 
 
DETERMINATION OF THE CARBON IN SMOKE 1 57 
 
 gas containing 14.8 per cent carbonic acid, 6.7 per cent excess 
 of air, and 0.96 per cent of black. 
 
 Saarbruck coal supplied with 155 cubic feet of air per 
 pound gave a gas having 12.8 per cent of carbonic acid, 28.5 
 per cent excess of air, and 2.03 per cent of black. 
 
 These show that in addition to being a sign of diminution 
 in combustible gases, smoke cannot cause a notable saving 
 in fuel if such saving is accompanied by increased waste 
 gases. The sensible heat of a larger volume compensates 
 easily for the advantages resulting from the more perfect 
 combustion of the carbon. 
 
 Bunte publishes the following determinations of black : 
 
 Several methods have been devised for approximating to 
 the actual quantity of carbon contained in smoke. One is 
 based on the amount of soot deposited on a given surface 
 placed in the chimney. The soot deposits on the upper sur- 
 face away from the direct current. After being exposed for 
 a few hours the deposit is brushed off and weighed. Another 
 method is by using smoked glasses of different degrees of 
 opacity and ascertaining what depth of color is necessary to 
 make the smoke invisible. An improvement on this method 
 is now being worked out by one of our manufacturers of 
 optical goods, by means of which the glasses are held in a 
 tube and so arranged as to gradually produce the effect, and 
 in such way that it can be measured. 
 
 Another method is that devised by Ringelmann, by means 
 of which the blackness of the smoke is compared with a set of 
 ruled lines, so scaled in width of line and space as to produce 
 six different gradations from smokeless through gray and 
 gray-black to dead black. He recommends the preparation 
 of cards 8 inches square, and have them suspended 50 feet 
 from the observer, at which distance the individual lines 
 become indistinct, and only a general tint is observable. The 
 intensity of the smoke is then compared with the cards and re- 
 corded as agreeing with card No. I, 2, or whatever it may be. 
 
158 
 
 CALORIFIC POWER Of FUELS. 
 
 The cards are shown in Fig. 40, reduced in size, the actual 
 lines and spaces being as follows: 
 
 FlG. 40. RlNGELMANN SMOKE SCALE. 
 
 Card o, all white. 
 
 Card i, black lines I mm. thick, 10 mm. apart between 
 centres, leaving spaces 9 mm. square. 
 
 Card 2, lines 2.3 mm. thick; spaces 7.7 mm. sq. 
 Card 3, lines 3.7 mm. thick; spaces 6.3 mm. sq. 
 Card 4, lines 5.5 mm. thick; spaces 4.5 mm. sq. 
 Card 5, all black. 
 
CHAPTER XII. 
 CALCULATION OF THE HEAT UNITS. 
 
 HEAT OF THE AQUEOUS VAPOR. 
 
 THE quantity of heat contained in a kilogram or pound of 
 steam at any temperature is 
 
 or 
 
 Q 606.5 + -35^ calories, 
 
 Q = 1091.7 + o.305(/ - 32) B. T. U. 
 
 allowing the specific heat of water to be constant. The 
 number of heat units is considered the same as the tem- 
 perature. 
 
 So that, allowing the average temperature of aqueous 
 vapor to be 150 C., each kilogram at o has absorbed a quan- 
 tity of heat equal to 
 
 606.5 +0.305 X 150 652.25 calories 
 
 or one pound has absorbed 1174 B. T. U. 
 
 There is a correction to this, since we do not wish the 
 units existing in the steam, but only those added to it from 
 the fuel. We must then deduct that already existing in the 
 water at its entrance to the boiler. If the feed-water be 20 
 (68 F.) the formula becomes 
 
 652.25 20 = 632.25 calories, 
 or 1174 (68 32) = 1138 B. T. U. 
 
 159 
 
l6o CALORIFIC POWER OF FUELS 
 
 HEAT OF WASTE GASES. 
 
 The heat carried to the chimney by the waste gases is 
 from several sources : 
 
 -\. Sensible heat shown by the temperature. 
 
 2. Heat of vaporization of the hygroscopic water and the 
 water formed from the hydrogen of the coal. 
 
 3. Heat retained by the combustible gases or their heat of 
 combustion. 
 
 4. Heat represented by soot or black of the smoke. 
 
 I. SENSIBLE HEAT OF THE TEMPERATURE. 
 
 The calculation of the water equivalent of the heat carried 
 to the chimney as sensible heat requires the volume, tem- 
 perature, composition, and specific heat of the constituents. 
 
 The specific heats of the usual constituents of waste gases 
 are shown in Table VIII. The specific heats are supposed to 
 be under constant pressure, so as to avoid useless calculations. 
 The hydrocarbons or hydrogen will be omitted for the same 
 reason. Calling v, v' , v" , v'" the volumes in cubic metres 
 of the gases nitrogen, carbonic acid, carbonic oxide, and oxy- 
 gen, we find their respective weights, by multiplying these 
 volumes by the weight per cubic metre, 
 
 1.256^ 1.966s/ i. 2 5 IT/' I.430Z/" 
 
 ' co ~o~ 
 
 Multiplying these by the specific weights we obtain the value 
 in water, 
 
 C 1.2562; X 0.244+ i. 966^ X 0.217+ i.25iz/' X 0.245 + 
 1.430s/" X 0.217. 
 
 The equivalent in water c multiplied by the temperature 
 on leaving the boiler gives calories, 
 
 C = c X T. 
 
CALCULATION OF THE HEAT UNITS. l6l 
 
 A correction of the same kind as that applied to the tem- 
 perature of the feed-water must be applied. We do not 
 wish the total calories, only those taken up from the coal. 
 From the observed temperature T we must deduct the 
 original temperature / before entering the fire. So that 
 
 C=cX(T-f). 
 
 The general formula then becomes 
 C = [(1.256^)0.244 + (1.966^)0.217 + (i.25iz/')o.245 
 
 N CO, CO 
 
 1.43000-217] (T-t). 
 
 O 
 As an example, suppose the following composition : 
 
 Nitrogen 81.25 )_( Air in excess 23.04 (4.84 X 4.761) 
 
 Oxygen 4.84 ) ( Nitrogen 63. 05 (81.254.84 23.04) 
 
 Carbonic acid. . 13.08 13.08 
 
 Carbonic oxide. 0.83 0.83 
 
 100.00 100.00 
 
 and that the temperature (T t) is 130. Then 
 
 Nitrogen 1.256 X .8125 X 0.244 = 0.249 
 
 Carbonic acid. . .. 1.966 X .1308 X 0.217 = 0.055 
 Carbonic oxide. . . 1.25 I X .0083 X 0.245 = 0.002 
 Oxygen 1.430 X .0484 X 0.217 = 0.015 
 
 i.oooo 0.321 
 
 The value in water for I cubic metre is 0.321 kilogram, 
 which at 130 give 
 
 0.321 X 130 = 41.7 calories. 
 
 If the volume of the gases was 8.938 cubic metres per 
 kilogram of coal, the calories carried to the chimney would be 
 
 8.938 X 
 
 i oo 
 
 = 2 calories> 
 
162 
 
 CALORIFIC POWER OF FUELS. 
 
 The same result can be reached more quickly by taking 
 the ratio of the specific heats to the volume (Table VIII). 
 
 N 8125X0.306 = 0.249 
 
 CO, 1308 X 0.426 = 0.055 
 
 CO 0083 X 0.306 = 0.002 
 
 0484 X 0.310 = 0.015 
 
 i.oooo 0.321 
 
 0.321 X 130 X 8.938 = 372 calories. 
 
 This may be still further simplified in practical work with 
 the combustion under normal conditions. Base the calcula- 
 tion on the proportion of carbonic acid, using 0.306 as coeffi- 
 cient for the remaining gases. Then 
 
 C = (0.426^ + o.3o6^)(r /) 
 
 v CO a o. 1308 X 0.426 = 0.055 
 
 R N, CO, and 0.8692 X 0.306 = 0.266 
 
 \ _^_____ 
 
 0.321 
 
 By means of the coefficients in Table IX we can still 
 further shorten the calculation. By this table we get directly 
 
 0.321 X 130 X 8.938 = 372 calories. 
 
 The loss of heat due to temperature of the waste gases 
 varies according to the condition of the boiler, its surface for 
 radiation, the grate surface, and the air supply. With the 
 most advantageous cases, and moderate combustion, the gas 
 temperature at the exit does not exceed 150 (302 F.), and 
 the loss, 5 or 6 per cent of the total heat of combustion. 
 It may reach 10 per cent, and in some cases even more. 
 
 2. HEAT OF THE HYGROSCOPIC AND COMBUSTION WATER. 
 
 During combustion, coal furnishes a quantity of aqueous 
 vapor from its hygroscopic water and its hydrogen ; the latter 
 
CALCULATION OF THE HEAT UNITS. 163 
 
 is determined by multiplying the weight of hydrogen by 9. 
 This is added to the hygroscopic water, and the formula 
 
 (606.5 + 0.305*) /' 
 
 applied ; t being the temperature of the vapor in the gases 
 (equal to that of the gases), and t' being that of the external 
 air. Besides this, however, we must consider the specific 
 heat of the aqueous vapor, 0.475. Each kilogram still 
 absorbs 0.475 multiplied by the number of degrees of tem- 
 perature above 100, and the formula becomes 
 
 ^[(606.5 + 0.3050 - t' + 0.475^ - ioo)], 
 
 x being the quantity of water, in kilograms, furnished by the 
 coal. 
 
 Suppose a coal contains 1 5 grams per kilogram of hygro- 
 scopic water and 45 grams of hydrogen, as follows: 
 
 Hygroscopic water 15 
 
 Carbon 735 
 
 Hydrogen 45 
 
 Nitrogen and oxygen 50 
 
 Ash.. . , 160 
 
 1000 
 
 Hydrogen 45 produces 9 X 45 = 405 grams, to which 
 add the 15 grams of hygroscopic water, 405 -f- 15 = 420 
 grams. The heat necessary to vaporize this, increased by 
 that corresponding to the temperature of the gases passing up 
 the chimney, represents the heat lost. 
 
 If the flue temperature is 145 = t, and the external air 
 17.5 = /', we have 
 
 o.42o[(6o6.5 + 0.305 X 145) - J 7- 5 + 0.475(145 - ioo) 
 
 = 274.9(494.8 B T.U.). 
 
164 CALORIFIC POWER OF FUELS. 
 
 If the heat of combustion of the coal is 7000 calories, then 
 the loss is 
 
 274.0 
 
 - = 3.92 per cent. 
 7000 
 
 The loss due to these causes in an average coal (4-5 per 
 cent hydrogen and I to 2 per cent moisture) is usually from 2 
 to 4 per cent. 
 
 3. CALORIES OF THE COMBUSTIBLE GASES. 
 
 Carbonic oxide is always present in variable quantities, 
 often hydrocarbons and sometimes hydrogen. This refers to 
 ordinary fuel and the usual methods of burning. The quan- 
 tity of unburnt gases depends on the kind of fireplace used 
 and the system of charging. Thick charges of fuel always 
 increase the volume of unburnt gases; the smallest amount 
 being obtained from small, equivalent charges, fed frequently 
 and using 30 to 50 per cent more air than the theoretical 
 quantity. 
 
 To determine this loss we may commence with the volume 
 or the weight corresponding to I kilogram of coal burnt. 
 The calculation is given on pages 137 and 138. No account 
 need be made of the temperature, the calculation of loss due 
 this having been made on page 161 for all gases, and there- 
 fore for these gases. 
 
 The calorific coefficients of the unburnt gases, referred to 
 a cubic metre at o and 760 mm. pressure, are 
 
 Heat of Combustion. 
 Weight per cub. m. 
 
 in Kilograms. Per Kilo. Per Cubic Metre. 
 
 Hydrogen 0.089 345 3O9 1 
 
 Carbonic oxide 1.251 2435 3043 
 
 Methane (CH 4 ) 0.715 13343 10038 
 
 Carbon vapor 1.073 11328 12143 
 
CALCULATION OF THE HEAT UNITS. 165 
 
 The weight and heat of combustion of carbon vapor are 
 given, as most of the time we do not know the molecular 
 condensation of the hydrocarbons; usually the ultimate com- 
 position is all that is known. Hence the hydrogen and car- 
 bon must be given their heat values as though free. Fortu- 
 nately they occur in only small percentages, and the error 
 introduced by so doing is small. 
 
 Suppose a gas to analyze 
 
 Carbonic oxide i.o 
 
 Carbonic acid 13.0 
 
 Methane I .o 
 
 Oxygen 6.0 
 
 Nitrogen 79.0 
 
 100.0 
 
 Assuming that the air has been fed at the rate of 10 cubic 
 metres per kilogram (160.5 cubic feet per pound), and that 
 the coal has a heat value of 8000 calories (14400 B. T. U.), 
 we will have, for 10 cubic metres, 
 
 Carbonic oxide o. I cubic metres. 
 
 Carbonic acid 1.3 " 
 
 Methane o. I " 
 
 Oxygen 0.6 " 
 
 Nitrogen 7.9 " 
 
 10.0 
 Then 
 
 CH 4 , o.i cub. m. @ 0.715 = 0.0715 kilogram; 
 CO, o.i " " @ 1.251 =0.1251 
 
 and 0.0715 X 13343 = 933-7 calories; 
 
 0.1251 X 2435 = 305.0 
 
 Total 1238.7 
 
1 66 CALORIFIC POWER OF FUELS. 
 
 The loss, then, is 1238.7 in 8000, or 15.48 per cent. 
 
 If instead of knowing the proportion of the hydrocarbons 
 we know only that of carbon and hydrogen, the heat values 
 calculate separately. Then, instead of methane o. I, there 
 would be carbon 0.05, and hydrogen 0.2. Then the cal- 
 culation would be 
 
 0.2 X 0.089 = 0.0178; 0.0178x34500= 614.1 
 0.05x1.073=0.0536; 0.0536 X 8137 = 436.1 
 o.i X 1.251 = 0.1251 ; 0.1251 X 2435= 305.0 
 
 1355.2 calories 
 
 
 
 The difference, 1355.2 1238.7 = 116.5 calories, or 0.9 
 per cent of the calories lost, or 15.48 X .009 = 0.138 per cent 
 of the total calories of the coal, which is small compared with 
 other sources of error. 
 
 By employing Table VII we may dispense with reducing 
 the volumes to weights, thus : 
 
 Hydrogen o.2m 3 X 3091 = 618 
 
 Carbon vapor 0.05 x 8722 = 436 
 
 Carbonic oxide o. I X 3043 = 304 
 
 1358 
 
 The preceding is an exaggerated case; as usually, with 
 ordinary working, the loss is from 2 to 7 per cent, rarely 
 exceeding the latter. Either method of calculation may be 
 used, then, without risk of causing an error of importance. 
 
 4. CALORIES DUE TO THE SOOT. 
 
 The soot in smoke consists of carbon with a trace of 
 hydrogen. It can be calculated as all carbon without appre- 
 ciable error and with the coefficient 8137. Knowing the 
 volume of gases produced by I kilogram and its content in 
 black (page 154), calculate the number of calories. Under 
 
CALCULATION OF THE HEAT UNITS. 
 
 I6 7 
 
 the most favorable conditions for smoke production the loss 
 does not exceed I per cent, and is generally less than one 
 half that amount. 
 
 DISTRIBUTION OF CALORIES-LOSS. 
 
 The difference between heat units accounted for and 
 those possible is considered as resulting from radiation by 
 surfaces not available for producing steam. The following is 
 taken from Scheurer- Kestner's results with a three -tube 
 steam boiler followed by a reheater. The first column gives 
 results obtained with Ronchamp coal in 1868, the second 
 results with Nixon's Navigation Co.'s coal in 1881. 
 
 Ronchamp. Nixon. 
 
 Calories in the steam 58 to 67$ 74-5$ 
 
 " " " waste gases 3.8 to 7.7 5.42 
 
 " " " unburnt gases ... 2.4 to 9.7 traces 
 
 11 " " smoke 0.3 to 0.75 none 
 
 " " " aqueous vapor. . 2.0 to 3.7 2.81 
 
 " not accounted for 19.4 to 24.7 l 7-^7 
 
 On September 20, 1895, Engineering published the results 
 of some experiments made by Bryan Donkin with Nixon's 
 coal on twenty different types of boilers. The following 
 table contains some of them : 
 
 Calories. 
 
 XII. 
 
 VIII. 
 
 VI. 
 
 VII. 
 
 II. 
 
 XI. 
 
 III. 
 
 IV. 
 
 XX. 
 
 I. 
 
 In the steam 
 
 78 <; 
 
 78 T 
 
 7<1 d. 
 
 71 8 
 
 7O d. 
 
 69 8 
 
 67 6 
 
 66 2 
 
 65 8 
 
 6? 8 
 
 In the waste gases 
 In the combustible gases.. 
 Not accounted for 
 
 6-5 
 
 0.0 
 
 JC o 
 
 14.0 
 
 1.7 
 
 5 8 
 
 13.8 
 2.4 
 
 Q "\ 
 
 13-3 
 0.8 
 
 Id. O 
 
 I 3 .6 
 0.0 
 1 1 Q 
 
 18.0 
 
 1.2 
 
 JO Q 
 
 16.2 
 
 1.2 
 
 o 6 
 
 22.5 
 
 0.0 
 
 no 
 
 18.0 
 1.6 
 
 9.4 
 
 12.7 
 
 T Q 
 
 
 
 
 
 
 
 
 y.u 
 
 
 
 Aj.y 
 
 The calories in the steam varied from 63.8 to 78.5 per cent. 
 
 " " " " waste gases " " 6.5 to 22.5 " " 
 
 " " " combustible gases " " o.o to 12.7 " " 
 
 " " not accounted for " " 5.8 to 15.0 " " 
 
 For the method of properly tabulating the heat balance, 
 see section XXI of the Steam Boiler Code on page 193. 
 
168 CALORIFIC POWER OF FUELS. 
 
 FLAME AND FLAME TEMPERATURES. 
 
 Whenever the temperature is sufficiently high to raise a 
 portion of the carbon, hydrogen, or other gaseous com- 
 bustible to incandescence, flame is produced. The tempera- 
 ture at which this phenomenon occurs varies with the sub- 
 stance burnt. Usually it requires a red heat or higher, but 
 in some cases a much lower temperature suffices: bor-methyl 
 B(CH 3 ), is an example, the flame temperature of which is not 
 high enough to scorch the finger placed in it. It is not neces- 
 sary that the flame should have solid particles in it, as flame 
 is produced by hydrogen burning under pressure in oxygen ; 
 neither is incandescence alone sufficient, as the fire of pure 
 carbon, magnesium, or iron glows but does not flame. 
 Flame is hollow, the combustion occurring on the surface, 
 and this may be easily demonstrated, by drawing off some of 
 the interior unconsumed gases with a tube and burning them. 
 
 Bunsen's researches led to the conclusion that the tem- 
 perature of burning carbonic oxide rapidly rose to 3000 C., 
 and remained stationary till one third of it was consumed ; 
 the temperature then fell to 2500 C., at which more burnt; 
 and finally fell to about 1200 C., which temperature was 
 maintained till all the remainder was consumed. Actually 
 the last temperature is soon reached in practice. Berthelot 
 confirms this, but is in doubt whether the loss of temperature 
 is due to dissociation or to change in specific heat. Some 
 hold that part of this loss of heat is caused by its absorption, 
 due to the production of incandescence and its accompanying 
 flame phenomena. A gas raised to incandescence gradually 
 manifests each increment of heat till that point is reached, 
 and beyond this no increase is noticed, all such further 
 increase being consumed by the flame production. 
 
 The rate of propagation of flame varies with the pressure 
 and with the material burning. The most rapid rate with 
 coal gas is when it is mixed with 5 parts of air ; with marsh 
 
FLAME TEMPERATURES. 169 
 
 gas, 8| parts of air. It will be noticed that the proportion of 
 oxygen is sensibly less than that required for perfect com- 
 bustion. 
 
 The luminosity depends on the compression of the gases 
 or the air. Hydrogen burning in oxygen at ordinary pressure 
 gives a flame hardly visible at all ; with a pressure of 20 atmos- 
 pheres it becomes quite luminous. Arsenic in burning pro- 
 duces quite a luminous flame at ordinary air pressure ; but 
 hardly any in rarefied air. The same is true of carbonic 
 oxide and other gases. The luminosity seems to be in direct 
 proportion to the pressure. 
 
 Luminosity seems to be greater with those substances 
 which on burning produce dense vapors. Hydrogen and 
 chlorine produce a vapor twice as heavy as water and the 
 luminosity is much stronger than with the oxygen-hydrogen 
 flame. Carbon and sulphur also produce heavy vapors and 
 much light. Phosphorus burning in oxygen produces the 
 dense heavy phosphoric anhydride and this is accompanied 
 with an almost blinding light. 
 
 The length of the flame ordinarily depends on the quantity 
 of hydrogen, and consequently the hydrocarbons contained 
 in, or generated from, the body consumed. With fuels con- 
 taining high hydrocarbon percentages, flame of almost any 
 desired length can be produced. This is especially the case 
 with gases. 
 
 The theoretical temperature of combustion, and hence of 
 the flame, may be calculated by dividing the heat units pro- 
 duced by the specific heats of the products formed. Of course, 
 these theoretical temperatures are never reached in practice, 
 but they serve as aids in determining the value of fuels for 
 certain purposes. 
 
 A few typical examples of these calculations will be given. 
 
 I . Hydrogen. Hydrogen burnt in oxygen produces 
 29000 heat units (water considered as vapor); the specific 
 heat of the aqueous vapor produced is 0.475. The hydrogen 
 
CALORIFIC POWER OF FUELS. 
 
 uses 8 times its weight of oxygen and generates 9 times the 
 quantity of water. 
 Then 
 
 2 9 00 = 6727 C. 
 9 X 0.479 
 
 Bunsen and Sainte-Claire Deville showed that the highest 
 temperature actually obtained is 2500 C., which may be in- 
 creased to 2850 C. by a pressure 0f 10 atmospheres. 
 
 The presence of nitrogen modifies the result materially. 
 The quantity of oxygen required, obtained from air, would 
 introduce 26.78 parts of nitrogen, the specific heat of which 
 130.244. The equation would then be 
 
 9 X 0.479 + 26.78 X 0.244 " 
 
 Bunsen's maximum temperature actually reached was 
 1800 C. 
 
 2. Carbon. Carbon burnt to carbonic oxide consumes 
 1.33 parts of oxygen, forms 2.33 parts of carbonic oxide, and 
 if burnt in air, introduces 4.46 parts of nitrogen. The specific 
 heat of carbonic oxide is 0.245 an d of nitrogen 0.244, as 
 before. The heat units generated are 2435. 
 
 For combustion in oxygen the equation would be 
 
 2435 
 
 2.33 X 0.245 
 In air it would be 
 
 2435 
 
 = 1462 C. 
 
 2.33 X 0.245 +4-46 X 0.244 
 The latter temperature is about the same as that actually 
 observed, and shows that but little dissociation occurs. 
 Owing to the non-volatility of carbon no flame is produced, 
 only an incandescence. The flame we ordinarily see on in- 
 candescent carbon is from the burning of carbonic oxide. 
 Carbon burnt to carbon dioxide can be treated similarly ; also 
 carbonic oxide burnt to carbon dioxide. 
 
FLAME TEMPERATURES. IJl 
 
 3. Marsh Gas. This gas requires 4 times its weight of 
 oxygen, and produces 2.25 parts of aqueous vapor and 2.75 
 parts of carbonic acid. If air is used, 13.39 parts of nitrogen 
 are introduced. The heat of combustion is 13343 calories. 
 
 The equations are, then, 
 
 '3343 = 797 i'C., 
 
 2.25 X o.479 + 2 -75 X 0.217 
 for oxygen and 
 
 13343 
 
 2.25 X 0.479 + 2-75 X 0.217 + 13.39 X 0.244 
 for combustion in air. 
 
 Olefiant gas, acetylene, etc., can be calculated similarly. 
 With a mixed gas, i.e., one containing several gases, account 
 must be taken of each one separately. Producer gas will be 
 given as an example. 
 
 4. Producer Gas. The producer gas taken will be assumed 
 to have the following composition by volume : 
 
 Carbonic oxide 21.0 per cent. 
 
 Hydrogen 11.5 " " 
 
 Marsh gas 2.0 " " 
 
 Carbonic acid 6.0 " " 
 
 Nitrogen 59.5 " " 
 
 100.0 " 
 
 First obtain the weight of the constituents. (See the tables.) 
 0.21 X 1.2515 = 0.2628 
 o. 1 15 X 0.0896 = 0.0103 
 0.02 X 0.7155 = 0.0143 
 0.06 X 1.9666=0.1360 
 0.595 X 1.2561 =0.7474 
 
 C0 a H 3 N 
 
 CO 0.2628 produces ____ 0.413 .... 0.502 
 
 H 0.0103 " ........ 0.093 0.276 
 
 CH 4 0.0143 " ---- 0.039 0.032 0.192 
 
 CO, 0.1360 " .... 0.136 ---- 
 
 N 0.7474 ........ 0.747 
 
 0.588 0.125 
 
I? 2 CALORIFIC POWER OF FUELS. 
 
 Then as the heat of combustion is 747.66 by volume or 
 874.6 by weight, we have for combustion in oxygen, 
 
 _ *7S _ = 2350' C, 
 0.125 X 0.479 + 0.588 X 0.217+0.747 X 0.244 
 
 and for combustion in air, 
 
 0.125 X 0.479 + 0.588 X 0.217+ I-7I7 X 0.244 
 
 5. Petroleum Oil. The oil may be assumed to contain 
 
 Carbon .............. . ....... 85 per cent. 
 
 Hydrogen .................. 15 " " 
 
 100 
 
 C 0.85 produces ---- 3-H7 CO, and 7.588 N 
 
 H 0.15 " 1.35 H a O .... " " 4.017 " 
 
 i.35 H 2 O 1.117 CO 2 11.605 N 
 
 The heat of combustion maybe assumed at 10000 calories. 
 Then for combustion in oxygen, 
 
 = 7558C., 
 
 1.35 X 0.479+ 3.U7 X 0.217 
 and for combustion in air, 
 
 10000 
 1.35 X 0.479+3.117 X 0.217+ 11.605 X 0.244 
 
 = 2400 C. 
 
 Other oils or solid fuels may be calculated according to 
 this model. 
 
 At the end of the volume are given a few of those fuels 
 most commonly used with the theoretical oxygen and air 
 flame temperatures. 
 
CARBON VAPOR. 1 73 
 
 WEIGHT AND HEAT UNITS OF CARBON VAPOR. 
 
 Two volumes of carbonic oxide are produced from I volume 
 of oxygen, and hence from I volume of carbon. I cubic 
 metre of carbonic oxide weighs 1251 grams. I cubic metre 
 of oxygen weighs 1430 grams. I cubic metre of carbonic 
 oxide contains, then, one-half a cubic metre of oxygen weigh- 
 ing 7 J 5 grams, and one-half a cubic metre of carbon vapor 
 weighing 536 grams. Hence I cubic metre of carbon vapor 
 weighs 2 X 536 = 1072 grams, and I kilogram measures 
 I : 1072 = 0.9328 cubic metre. 
 Or 
 
 I cubic foot of carbonic oxide weighs 546.78 grains. 
 I " " " oxygen weighs ....... 624.85 " 
 
 One cubic foot CO then contains \ cubic foot of O and 
 cubic foot of C. 
 
 546.78 - 312.425 = 234.355, 
 and 
 
 2- X 234.355 = 468.71 grains, 
 
 weight of i cubic foot of carbon vapor. 
 
 One pound of carbon vapor measures 14.93 cubic feet. 
 
 If we wish the heat-units of carbon in vapor without the 
 heat of vaporization, multiply the weight of a cubic metre by 
 the heat of combustion of solid carbon. If from wood charcoal, 
 
 8137 X 1.072 = 8722(15699.6 B.T. U.). 
 If from diamond, 
 
 7859 X 1.072 = 8424(14963.2 B.T. U.). 
 
 If carbon vapor with its heat of vaporization be wanted, 
 take the heat of combustion of carbonic oxide which contains 
 carbon as vapor and compare it with the heat of combustion of 
 carbon, uniting with the same quantity of oxygen to form 
 
 UNIVERSITY 
 
174 CALORIFIC POWER OF FUELS. 
 
 carbonic oxide. In doing so it is supposed that carbon in 
 combining with two atoms of oxygen generates the same 
 quantity of heat with one as with the other, only in the first 
 case part of the heat is used in vaporizing the carbon. This 
 heat is found by subtracting the heat of combustion of the 
 solid carbon from that of the carbon supposed gaseous in 
 carbonic oxide. 
 
 One kilogram of carbon unites with 1.333 kilograms of 
 oxygen to form 2.333 kilograms of carbonic oxide. With 
 diamond there is generated 2405 calories. The 2.333 kilograms 
 of carbonic oxide in becoming carbonic acid generates 2.333 X 
 2435 = 5680 calories. Then I kilogram of carbon in passing 
 from carbonic oxide to carbonic acid generates 5680 calories. 
 We have seen, on the other hand, that I kilogram of diamond 
 carbon generates 2405 calories in becoming carbonic oxide. 
 The difference, then, 5680 2405 = 3275(5895 B. T. U.) cal- 
 ories, represents the heat of vaporization of diamond carbon. 
 With wood charcoal it becomes 5680 2489 = 3191(5743.8 
 B. T. U.). 
 
 The heat of combustion will be then 7859 -f- 3275 = 1 1 134 
 calories (20041 B. T. U.) for diamond, and 8137 -f- 3191 = 
 11328 calories (20390 B. T. U.) for wood charcoal. 
 
 % 
 
 EVAPORATIVE POWER OF FUEL. 
 
 The evaporative power of a fuel represents the number of 
 pounds of water at 212 F. that can be evaporated or con- 
 verted into steam by one pound of the fuel. Water at that 
 temperature is sufficiently heated to vaporize, but needs an 
 addition of force equivalent to that required for the vaporiza- 
 tion. This quantity varies for the pressure of the barometer 
 and the temperature of the water, but for the purposes of cal- 
 culation is considered to be taken at 30 inches of mercury and 
 212 F. Experiment has shown the equivalent to be 965.7 
 heatunits (B. T. U.). 
 
EVAPORATIVE POWER. 175 
 
 To find the theoretical evaporating power of a fuel, then, 
 divide the number of thermal units it generates on combus- 
 tion by 965.7. For instance, the heat of combustion of a 
 sample of Illinois coal was determined by Prof. Carpenter to 
 be 13200. Its evaporative power would be 
 
 13200 
 
 ^ = 13.67 pounds. 
 
 965.7 
 
 This means that under the proper conditions one pound 
 of the coal in question would evaporate 13.67 pounds already 
 heated to 212 F. 
 
 But this amount of duty is rarely realized. The boiler 
 may not be well built, the setting may be faulty, and there 
 are numerous other chemical or mechanical conditions which 
 modify the yield. With these no rule can be established ; 
 each individual case must be allowed for specially. With 
 , ashes and moisture, chemical constituents of the coal, the 
 case is different. A percentage allowance for these will usually 
 suffice. 
 
 For instance, in the above coal there was 5.12 per cent of 
 water and 15.2 per cent of ash. Then 
 
 100 (15.2 -|- 5.12) X 13.67 = 12.23 pounds. 
 
 If deemed necessary, a further correction can be made for 
 the water of the coal, which would reduce the evaporation by 
 its own amount. This correction would become 
 
 12.23 0.05 = 12. 18 pounds 
 
 as the quantity which should be evaporated with the coal as 
 analyzed. 
 
 The quantity of ash produces an effect on the evaporative 
 power aside from its proportional reduction in combustible. 
 This is due' to the fact that where a large percentage of ash 
 occurs, the particles of carbon of the fuel are not burnt com- 
 
CALORIFIC POWER OF FUELS. 
 
 pletely, owing to being enclosed in the ash and consequently 
 shut off from access of air. This is especially the case with 
 those ashes which are easily fuzed by the heat of the fire. 
 Ashes containing carbonates are much more easily fuzed than 
 those containing phosphates or sulphates. On this account a 
 chemical analysis of the ash is at times quite desirable. 
 
 Some difference in evaporation is noticed in using the dif- 
 ferent sizes of coal, more particularly with the fine sizes. 
 With the proper arrangements for burning fires a good yield 
 is obtained, but with the ordinary grates the yield is much 
 lower. 
 
APPENDIX, 
 
 REPORT OF THE COMMITTEE ON THE REVISION OF THE 
 SOCIETY CODE OF 1885, RELATIVE TO A STANDARD 
 METHOD OF CONDUCTING STEAM-BOILER TRIALS. 
 
 Presented to the New York meeting of the American Society of Mechani- 
 cal Engineers, December, 1897, and forming a part of the Transac- 
 tions, Volume XIX. 
 
 To THE AMERICAN SOCIETY OF MECHANICAL ENGINEERS. 
 
 Gentlemen : The undersigned Committee, to which was 
 submitted the revision of the Society Code of 1885, relative 
 to a standard method of conducting steam-boiler trials, 
 reports as follows : 
 
 The former Committee gave a full statement of the prin- 
 ciples which governed it in the preparation of the Code of 
 Rules at that time recommended. These principles covered 
 the ground in an admirable manner, so far as the practice of 
 boiler-testing had been perfected, and we are in unanimous 
 accord with the sentiments which the report of that Com- 
 mittee expressed. During the interval of twelve years which 
 has passed, methods and instruments have in some measure 
 changed. Improvements have been made in the instruments 
 for determining the moisture in steam. The throttling and 
 separating form of calorimeters have displaced the barrel and 
 other types of steam calorimeters referred to in the previous 
 report. Attention has been devoted to the determination of 
 the calorific value of coal, and a number of coal calorimeters 
 
 177 
 
1/8 APPENDIX. 
 
 have been brought out and successfully used for this purpose. 
 It has come to be a practice with many experts to include 
 in the table of results of boiler-tests the percentage of 
 " efficiency," or proportion of the calorific value of the coal 
 which is utilized by the boiler. Specifications and contracts 
 are in some cases drawn up, providing for certain percentages 
 of efficiency instead of a specified evaporation. The analysis 
 of flue-gases is receiving more attention than formerly, not 
 only in our educational institutions, but also in the regular 
 practice of engineers who make a specialty of boiler-testing. 
 
 Your Committee submits a revised Code, termed the Code 
 of 1897. It is substantially the same as the 1885 Code, with 
 such amendments as the experience of the last twelve years 
 has shown to be desirable. 
 
 It is beyond the province of the Committee to recom- 
 mend instruments of particular makers for obtaining the 
 quality of the steam, the calorific value of the fuel, or any 
 other data relating to the trial ; but following the practice of 
 the former Committee, individual members have submitted 
 their views (with the approval of the full membership) in an 
 " Appendix to the 1897 Code," signed by their initials. In 
 this appendix are included some of the articles from the 
 appendix to the former Code, which are thought to be of 
 especial value. 
 
 In the matter of instruments for determining the calorific 
 value of fuel, it seems desirable that the Committee should 
 make a recommendation which is as specific as present knowl- 
 edge and circumstances will warrant. It is agreed that some 
 form of calorimeter in which the coal is burned in an atmos- 
 phere of oxygen gas is to be preferred, and it is generally 
 held that the most perfect apparatus thus far brought out is 
 the Bomb Calorimeter, originally designed by Berthelot, and 
 modified by Mahler and Hempel. Several of these instru- 
 ments are in use in this country, principally in the laborato- 
 ries of engineering schools ; but the apparatus is complicated 
 
APPENDIX. 179 
 
 and expensive, and it is not probable that many engineers 
 will have the instrument as a part of their equipment for test- 
 ing boilers. It is recommended, therefore, that samples of 
 the coal used in testing boilers be sent for determinations of 
 their heating value to a testing laboratory provided with one 
 of these instruments, or with some instrument which shall be 
 proven to be equally good. 
 
 Besides the amendments to the Code of 1885, concerning 
 the determination of "efficiency " and the use of improved 
 steam calorimeters, directions are given for sampling the coal, 
 for determining the heat of combustion from the chemical 
 analysis of coal, and for working out a heat balance. Rules 
 are laid down for finding the quantity of moisture in coal and 
 for making allowance for it. The tabular form of presenting 
 the results of the test is somewhat changed from that of the 
 Code of 1885, and alterations in the text of that Code are 
 made wherever revision seems desirable. 
 
 The Committee approves the conclusions of the Com- 
 mittee of 1885 concerning the standard " unit of evapora- 
 tion " contained in the following extract from the introduction 
 to the Code of 1885: 
 
 44 It has gradually come to be the custom to reduce all 
 results to the common standard of weight of water evaporated 
 by the unit weight of fuel, the evaporation being considered 
 to have taken place at mean atmospheric pressure, and at the 
 temperature due that pressure, the feed-water being also 
 assumed to have been supplied at that temperature. This is, 
 in technical language, said to be the ' equivalent evaporation 
 from and at the boiling-point' (212 degrees Fahr.), and has 
 now become so generally incorporated into the science and 
 the practice of steam-engineering that your Committee would 
 simply express their approval of the adoption, and recom- 
 mend the permanent retention of this ' unit of evaporation,' 
 viz., one pound of water at 212 degrees Fahr. evaporated 
 into steam of the same temperature. This is equivalent to 
 
180 APPENDIX. 
 
 the utilization of 965.7 British thermal units per pound of 
 water so evaporated." 
 
 The unit of commercial boiler horse-power adopted by 
 the Committee of 1885 was the same as that used in the re- 
 ports of the boiler-tests made at the Centennial Exhibition 
 of 1876. The Committee of 1885 reported in favor of this 
 standard in language of which the following is an extract : 
 
 11 Your Committee, after due consideration, has deter- 
 mined to accept the Centennial standard, and to recommend 
 that in all standard trials the commercial horse-power be 
 taken as an evaporation of 30 pounds of water per hour 
 from a feed- water temperature of 100 degrees Fahr. into 
 steam at 70 pounds gauge-pressure, which shall be consid- 
 ered to be equal to 34^ units of evaporation ; that is, to 34^ 
 pounds of water evaporated from a feed-water temperature 
 of 212 degrees Fahr. into steam at the same temperature. 
 This standard is equal to 33,305 thermal units per hour." 
 
 The present Committee accepts the same standard, but 
 reverses the order of two clauses in the statement, and 
 slightly modifies them to read as follows: 
 
 In all standard trials the commercial horse-power shall 
 be taken as 34^ units of evaporation; that is, 34^ pounds 
 of water evaporated from a feed-water temperature of 212 
 degrees Fahr. into steam at the same temperature. This 
 standard is equivalent to 33,317 British thermal units per 
 hour. It is also practically equivalent to an evaporation of 
 30 pounds of water from a feed-water temperature of 100 
 degrees Fahr. into steam at 70 pounds gauge-pressure.* 
 
 * According to the tables in Porter's Treatise on the Richards Steam- 
 engine Indicator, an evaporation of 30 pounds of water from 100 degrees 
 Fahr. into steam at 70 pounds pressure is equal to an evaporation of 34.488 
 pounds from and at 212 degrees; and an evaporation of 34^ pounds from 
 and at 212 degrees Fahr. is equal to 30.010 pounds from 100 degrees Fahr. 
 into steam at 70 pounds pressure. 
 
 The "unit of evaporation" being equal to 965.7 thermal units, the 
 commercial horse-power = 34.5 X 965.7 = 33.317 thermal units. 
 
APPENDIX. l8l 
 
 The Committee also indorses the statement of the Com- 
 mittee of 1885 concerning the commercial rating of boilers, 
 changing somewhat its wording, so as to read as follows : 
 
 " It is the opinion of this Committee that a boiler rated 
 at any stated horse-power should develop that power when 
 using the best coal ordinarily sold in the market where the 
 boiler is located, fired by an ordinary fireman, with a draft at 
 the smoke-box not exceeding f inch of water column ; and, 
 further, that the boiler should develop at least one third 
 more than its rated power when operated with the best sys- 
 tem of firing and with the full draft available." 
 Respectfully submitted, 
 
 CHAS. E. EMERY,* 
 
 WM. KENT, 
 
 GEO. H. BARRUS, 
 
 CHAS. T. PORTER, 
 
 ROBERT H. THURSTON, y Committee. 
 
 ROBERT W. HUNT, 
 
 F. W. DEAN, 
 
 J. S. COON, 
 
 WM. B. POTTER, 
 
 RULES FOR CONDUCTING BOILER-TRIALS, 
 CODE OF 1897. 
 
 PRELIMINARIES TO A TRIAL. 
 
 I. Determine at the outset the specific object of the pro- 
 posed trial, whether it be to ascertain the capacity of the 
 
 * The motion for the appointment of this Committee was made by Mr. 
 Barrus in connection with the discussion of Mr. Dean's paper, No. DCL, 
 on " The Efficiency of Boilers," etc. The President of the Society desig- 
 nated Mr. Kent, the chairman of the Committee of 1884, to call the firsi 
 meeting of the new Committee. At that meeting, on motion of Mr. Kent, 
 Dr. Emery was selected as chairman, and he conducted the preliminary 
 correspondence. The report in the form originally printed was prepared 
 by a sub-committee consisting of Messrs. Emery, Porter, Barrus, and 
 Kent. 
 
1 82 APPENDIX. 
 
 boiler, its efficiency as a steam-generator, its efficiency and its 
 defects under usual working conditions, the economy of some 
 particular kind of fuel, or the effect of changes of design, 
 proportion, or operation ; and prepare for the trial accord- 
 ingly. 
 
 II. Examine the boiler ', both outside and inside; ascertain 
 the dimensions of grates^ heating-surfaces, and all important 
 parts; and make a full record, describing the same, and illus- 
 trating special features -by sketches. The area of heating 
 surface is to be computed from the outside diameter of all 
 tubes, whether water-tubes or fire-tubes. This rule corre- 
 sponds to the practice of many builders of different types of 
 boilers, and is intended to make the practice of rating heating- 
 surface uniform. All surfaces below the mean water-level 
 which have water on one side and products of combustion on 
 the other are to be considered as water-heating surface, and 
 all surfaces above the mean water-level which have steam on 
 one side and products of combustion on the other are to be 
 considered as superheating surface. 
 
 III. Notice the general condition of the boiler and its 
 equipment, and record such facts in relation thereto as bear 
 upon the objects in view. 
 
 If the object of the trial is to ascertain the maximum 
 economy or capacity of the boiler as a steam-generator, the 
 boiler and all its appurtenances should be put in first-class 
 condition. Clean the heating-surface inside and outside, 
 remove clinkers from the grates and from the sides of the fur- 
 nace. Remove all dust, soot, and ashes from the chambers, 
 smoke-connections, and flues. Close air-leaks in the masonry 
 and poorly fitted cleaning-doors. See that the damper will 
 open wide and close tight. Test for air-leaks by firing a few 
 shovels of smoky fuel and immediately closing the damper, 
 observing the escape of smoke through the crevices. 
 
 IV. Determine the character of the coal to be used. For 
 tests of the efficiency or capacity of the boiler the coal should, 
 
APPENDIX. 183 
 
 if possible, be of some kind which is commercially regarded 
 as a standard. For New England and that portion of the 
 country east of the Allegheny Mountains, good anthracite egg 
 coal, containing not over 10 per cent of ash, and semi- 
 bituminous Cumberland (Md.) and Pocahontas (Va.) coals are 
 thus regarded. West of the Allegheny Mountains, Poca- 
 hontas (Va.) and New River (W. Va.) semi-bituminous, and 
 Youghiogheny or Pittsburg bituminous coals are recognized 
 as standards.* There is no special grade of coal mined in 
 the Western States which is widely recognized as of superior 
 quality or considered as a standard coal for boiler-testing. 
 Big Muddy lump, an Illinois coal mined in Jackson County, 
 111., is suggested as being of sufficiently high grade to answer 
 the requirements in districts where it is more conveniently 
 obtainable than the other coals mentioned above. 
 
 V. Establish the correctness of all apparatus used in the 
 test for weighing and measuring. These are : 
 
 1. Scales for weighing coal, ashes, and water. 
 
 2. Tanks or water-meters for measuring water. Wafer- 
 meters, as a rule, should only be used as a check on other 
 measurements. For accurate work, the water should be 
 weighed or measured in a tank. 
 
 3. Thermometers and pyrometers for taking temperatures 
 of air, steam, feed- water, waste gases, etc. 
 
 4. Pressure-gauges, draft-gauges, etc. 
 
 The kind and location of the various pieces of testing 
 apparatus must be left to the judgment of the person con- 
 ducting the test, always keeping in mind the main object, 
 i.e., to obtain authentic data. 
 
 VI. See that the boiler and chimney are thoroughly heated 
 before the trial to their usual working temperature. If the 
 
 * These coals are selected because they are about the only coals which 
 contain the essentials of excellence of quality, adaptability to various kinds 
 of furnaces, grates, boilers, and methods of firing, and wide distribution 
 and general accessibility in the markets. 
 
1 84 APPENDIX. 
 
 boiler is new and of a form provided with a brick setting, it 
 should be in regular use at least a week before the trial, so as 
 to dry and heat the walls. If it has been laid off and become 
 cold, it should be worked before the trial until the walls are 
 well heated. 
 
 VII. The boiler and connections should be proved to be 
 free from leaks before beginning a test, and all water connec- 
 tions, including blow and extra feed-pipes, should be discon- 
 nected, stopped with blank flanges, or bled through special 
 openings beyond the valves, except the particular pipe through 
 which water is to be fed to the boiler during the trial. Dur- 
 ing the test the blow-off and feed-pipes should remain ex- 
 posed. 
 
 If an injector is used, it should receive steam directly 
 through a felted pipe from the boiler being tested.* 
 
 See that the steam-main is so arranged that water of con- 
 densation cannot run back into the boiler. 
 
 VIII. Starting and Stopping a Test. A test should last 
 at least ten .hours of continuous running. A longer test may 
 be made when it is desired to ascertain the effect of widely 
 varying conditions, or the performance of a boiler under the 
 working conditions of a prolonged run. The conditions of 
 the boiler and furnace in all respects should be, as nearly as 
 possible, the same at the end as at the beginning of the test. 
 The steam-pressure should be the same ; the water-level the 
 same ; the fire upon the grates should be the same in quan- 
 tity and condition; and the walls, flues, etc., should be of 
 the same temperature. Two methods of obtaining the de- 
 
 * In feeding a boiler undergoing test with an injector taking steam 
 from another boiler, or the main steam-pipe from several boilers, the 
 evaporative results may be modified by a difference in the quality of the 
 steam from such source compared with that supplied by the boiler being 
 tested, and in some cases the connection to the injector may act as a drip 
 for the main steam-pipe. If it is known that the steam from the main 
 pipe is of the same quality as that furnished by the boiler undergoing the 
 test, the steam may be taken from such main pipe. 
 
APPENDIX. 185 
 
 sired equality of conditions of the fire may be used, viz. : 
 those which were called in the Code of 1885 "the standard 
 method" and "the alternate method," the latter being em- 
 ployed where it is inconvenient to make use of the standard 
 method. 
 
 IX. Standard Method. Steam being raised to the work- 
 ing pressure, remove rapidly all the fire from the grate, close 
 the damper, clean the ash-pit, and as quickly as possible start 
 a new fire with weighed wood and coal, noting the time and 
 the water-level while the water is in a quiescent state, just 
 before lighting the fire. 
 
 At the end of the test remove the whole fire, which has 
 been burned low, clean the grates and ash-pit, and note the 
 water-level when the water is in a quiescent state, and record 
 the time of hauling the fire. The water-level should be as 
 nearly as possible the same as at the beginning of the test. 
 If it is not the same, a correction should be made by com- 
 putation, and not by operating the pump after the test is 
 completed. 
 
 X. Alternate Method. The boiler being thoroughly 
 heated by a preliminary run, the fires are to be burned low 
 and well cleaned. Note the amount of coal left on the grate 
 as nearly as it can be estimated ; note the pressure of steam 
 and the water-level, and note this time as the time of starting 
 the test. Fresh coal which has been weighed should now be 
 fired. The ash-pits should be thoroughly cleaned at once 
 after starting. Before the end of the test the fires should be 
 burned low, just as before the start, and the fires cleaned in 
 such a manner as to leave the bed of coal of the same depth, 
 and in the same condition, on the grates as at the start. The 
 water-level and steam-pressures should previously be brought 
 as nearly as possible to the same point as at the start, and 
 the time of ending of the test should be noted just before 
 fresh coal is fired. If the water-level is not the same as at 
 
1 86 APPENDIX. 
 
 the start, a correction should be made by computation, and 
 not by operating the pump after the test is completed. 
 
 XL Uniformity of Conditions. In all standard trials the 
 conditions should be maintained uniformly constant. Ar- 
 rangements should be made to dispose of the steam so that 
 the rate of evaporation may be kept the same from beginning 
 to end. This may be accomplished in a single boiler by 
 carrying the steam through a waste steam-pipe, the discharge 
 from which can be regulated as desired. In a battery of 
 boilers in which only one is tested the draught can be regu- 
 lated on the remaining boilers, leaving the test-boiler to work 
 under a constant rate of production. 
 
 Uniformity of conditions should prevail as to the pressure 
 of steam, the height of water, the rate of evaporation, the 
 thickness of fire, the times of firing and quantity of coal fired 
 at one time, and as to the intervals between the times of 
 cleaning the fires. 
 
 XII. Keeping the Records. Take note of every event 
 connected with the progress of the trial, however unimpor- 
 tant it may appear. Record the time of every occurrence 
 and the time of taking every weight and every observation. 
 
 The coal should be weighed and delivered to the fireman 
 in equal proportions, each sufficient for not more than one 
 hour's run, and a fresh portion should not be delivered until 
 the previous one has all been fired. The time required to- 
 consume each portion should be noted, the time being re- 
 corded at the instant of firing the last of each portion. It is 
 desirable that at the same time the amount of water fed into 
 the boiler should be accurately noted and recorded, including 
 the height of the water in the boiler, and the average pressure 
 of steam and temperature of feed during the time. By thus 
 recording the amount of water evaporated by successive por- 
 tions of coal, the test may be divided into several periods if 
 desired, and the degree of uniformity of combustion, evapo- 
 ration, and economy analyzed for each period. In addition 
 
APPENDIX. IS/ 
 
 to these records of the coal and the feed-water, half-hourly 
 observations should be made of the temperature of the feed- 
 water, of the flue gases, of the external air in the boiler-room, 
 of the temperature of the furnace when a furnace-pyrometer 
 is used, also of the pressure of steam, and of the readings of 
 the instruments for determining the moisture in the steam. 
 A log should be kept on properly prepared blanks containing 
 columns for record of the various observations. 
 
 When the " standard method" of starting and stopping 
 the test is used, the hourly rate of combustion and of evapo- 
 ration and the horse -power may be computed from the 
 records taken during the time when the fires are in active 
 condition. This time is somewhat less than the actual time 
 which elapses between the beginning and end of the run. 
 This method of computation is necessary, owing to the loss 
 of time due to kindling the fire at the beginning and burning 
 it out at the end. 
 
 XIII. Quality of Steam. The percentage of moisture in 
 the steam should be determined by the use of either a throt- 
 tling or a separating steam-calorimeter. The sampling-nozzle 
 should be placed in the vertical steam-pipe rising from the 
 boiler. It should be made of ^-inch pipe, and should extend 
 across the diameter of the steam-pipe to within half an inch 
 of the opposite side, being closed at the end and perforated 
 with not less than twenty -J-inch holes equally distributed 
 along and around its cylindrical surface, but none of these 
 holes should be nearer than j- inch to the inner side of the 
 steam -pipe. The calorimeter and the pipe leading to it 
 should be well covered with felting. Whenever the indica- 
 tions of the throttling or separating calorimeter show that the 
 percentage of moisture is irregular, or occasionally in excess 
 of three per cent, the results should be checked by a steam- 
 separator placed in the steam-pipe as close to the boiler as 
 convenient, with a calorimeter in the steam-pipe just beyond 
 the outlet from the separator. The drip from the separator 
 
1 88 APPENDIX. 
 
 should be caught and weighed, and the percentage of moist- 
 ure computed therefrom added to that shown by the calo- 
 rimeter. 
 
 Superheating should be determined by means of a ther- 
 mometer placed in a mercury-well or oil-well inserted in the 
 steam-pipe. 
 
 For calculations relating to quality of steam and correc- 
 tions for quality of steam. 
 
 XIV. Sampling the Coal and Determining its Moisture. 
 As each barrow-load or fresh portion of coal is taken from the 
 coal-pile, a representative shovelful is selected from it and 
 placed in a barrel or box in a cool place and kept until the 
 end of the trial. The samples are then mixed and broken 
 into pieces not exceeding one inch in diameter, and reduced 
 by the process of repeated quartering and crushing until a 
 final sample weighing about five pounds is obtained, and the 
 size of the larger pieces are such that they will pass through 
 a sieve with J-inch meshes. From this sample two one- 
 quart, air-tight glass preserving-jars, or other air-tight vessels 
 which will prevent the escape of moisture from the sample, 
 are to be promptly filled, and these samples are to be kept 
 for subsequent determinations of moisture and of heating 
 value, and for Chemical analyses. During the process of 
 quartering, when the sample has been reduced to about 100 
 pounds, a quarter to a half of it may be taken for an approxi- 
 mate determination of moisture. This may be made by 
 placing it in a shallow iron pan, not over three inches deep, 
 carefully weighing it, and setting the pan in the hottest place 
 that can be found on the brickwork of the boiler setting or 
 flues, keeping it there for at least twelve hours, and then 
 weighing it. The determination of moisture thus made is 
 believed to be approximately accurate for anthracite and 
 semi-bituminous coals, and also for Pittsburg or Youghio- 
 gheny coal; but it cannot be relied upon for coals mined 
 west of Pittsburg, or for other coals containing inherent 
 
APPENDIX. 189 
 
 moisture. For these latter coals it is important that a more 
 accurate method be adopted. The method recommended by 
 the Committee for all accurate tests, whatever the character 
 of the coal, is described as follows: 
 
 Take one of the samples contained in the glass jars, crush 
 the whole of it by running it through an ordinary coffee-mill 
 adjusted so as to produce somewhat coarse grains (less than 
 T V inch), thoroughly mix the crushed sample, select from it a 
 portion of from 10 to 50 grams, weigh it in a balance which 
 will easily show a variation as small as I part in 1000, and 
 dry it in an air or sand bath at a temperature between 240 
 and 280 degrees Fahr. for one hour. Weigh it and record 
 the loss, then heat and weigh it again repeatedly, at intervals 
 of an hour or less, until the minimum weight has been 
 reached and the weight begins to increase by oxidation of a 
 portion of the coal. The difference between the original and 
 the minimum weight is taken as the moisture. This moisture 
 should preferably be made on duplicate samples, and the 
 results should agree within 0.3 to 0.4 of one per cent, the 
 mean of the two determinations being taken as the correct 
 result. 
 
 If the coal contains an appreciable amount of surface 
 moisture, another portion of the 100 pounds sample should 
 be weighed and spread out in a thin layer on a clean sheet- 
 iron plate, and exposed for a period of twenty-four hours to 
 the atmosphere of the boiler-room, and by this means air- 
 dried. After being weighed again, the percentage which the 
 weight shrinks during this drying may be termed the percent- 
 age of surface moisture. 
 
 XV. Treatment of Ashes and Refuse. The ashes and 
 refuse are to be weighed in a dry state. For elaborate trials 
 a sample of the same should be procured for analysis. When 
 it is desired to know accurately the amount of coal consumed, 
 as distinguished from combustible, all lumps of unconsumed 
 
lOX) APPENDIX. 
 
 coal one-half inch or more in diameter are to be picked from 
 the refuse and deducted from the weight of coal fired. 
 
 XVI. Calorific Tests and Analysis of Coal. The quality 
 of the fuel should be determined either by heat test or by 
 analysis, or by both. 
 
 The rational method of determining the total heat of 
 combustion is to burn the sample of coal in an atmosphere of 
 oxygen-gas, the coal to be sampled as directed in Article XIV 
 of this Code. 
 
 The chemical analysis of the coal should be made only by 
 an expert chemist. The total heat of combustion computed 
 from the results of the ultimate analysis should be obtained 
 by the use of Dulong's formula (with constants modified by 
 recent determinations), viz., 
 
 / O 
 14600 C + 62000 ^ H g- 
 
 in which C, H, and O refer to the proportion of carbon, 
 hydrogen, and oxygen respectively, and determined by the 
 ultimate analysis.* 
 
 It is recommended that the analysis and the heat test be 
 each made by two independent laboratories, and the mean of 
 the two results, if there is any difference, be adopted as the 
 correct figures. 
 
 It is desirable that a proximate analysis should also be 
 made to determine the relative proportions of volatile matter 
 and fixed carbon in the coal. 
 
 XVII. Analysis of Flue -gases. The analysis of the flue- 
 gases is an especially valuable method of determining the 
 relative value of different methods of firing, or of different 
 kinds of furnaces. In making these analyses great care should 
 
 * Favre and Silbermann give 14544 B. T. U. per pound carbon; Berthe- 
 lot 14647 B. T. U. Favre and Silbermann give 62032 B. T. U. per pound 
 hydrogen; Thomson, 61816 B. T. U. 
 
APPENDIX. IQI 
 
 be taken to procure average samples, since the composition 
 is apt to vary at different points of the flue ; and where com- 
 plete determinations are desired, the analysis should be 
 intrusted to an expert chemist. For approximate determina- 
 tions the Orsat* or the Hempelf apparatus may be used by 
 the engineer. 
 
 XVIII. Smoke Observations. It is desirable to 'have a 
 uniform system of determining and recording the quantity of 
 smoke produced where bituminous coal is used. The system 
 commonly employed is to express the degree of smokiness 
 by means of percentages dependent upon the judgment of 
 the observer. The Committee does not place much value 
 upon a percentage method, because it depends so largely 
 upon the personal element, but if this method is used, it is 
 desirable that, so far as possible, a definition be given in ex- 
 plicit terms as to the basis and method employed in arriving 
 at the percentage. 
 
 XIX. Miscellaneous. In tests for purposes of scientific 
 research, in which the determination of all the variables en- 
 tering into the test is desired, certain observations should be 
 made which are in general unnecessary for ordinary tests. 
 These are the measurement of the air-supply, the determina- 
 tion of its contained moisture, the determination of the 
 amount of heat lost by radiation, of the amount of infiltra- 
 tion of air through the setting, and (by condensation of all 
 the steam made by the boiler) of the total heat imparted to 
 the water. 
 
 As these determinations are not likely to be undertaken 
 except by engineers of high scientific attainments, it is not 
 deemed advisable to give directions for making them. 
 
 XX. Calculations of Efficiency. Two methods of defining 
 
 * See R. S. Hale's paper on " Flue Gas Analysis," Transactions A. S. 
 M. ., vol. xvni. p. 901. 
 
 f See Hempel on " Gas Analysis." 
 
I Q2 APPENDIX. 
 
 and calculating the efficiency of a boiler are recommended. 
 They are : 
 
 Heat absorbed per Ib. combustible 
 
 1. Efficiency of the boiler = TJ -r - - 
 
 Heating value of I Ib. combustible 
 
 2. Efficiency of the boiler and grate 
 
 Heat absorbed per Ib. coal 
 Heating value of I Ib. coal 
 
 The first of these is sometimes called the efficiency based 
 on combustible, and the second the efficiency based on coal. 
 The first is recommended as a standard of comparison for all 
 tests, and this is the one which is understood to be referred to 
 when the word " efficiency " alone is used without qualifica- 
 tion. The second, however, should be included in a report 
 of a test, together with the first, whenever the object of the 
 test is to determine the efficiency of the boiler and furnace 
 together with the grate (or mechanical stoker), or to compare 
 different furnaces, grates, fuels, or methods of firing. 
 
 The heat absorbed per pound of combustible (or per pound 
 coal) is to be calculated by multiplying the equivalent evapo- 
 ration from and at 212 degrees per pound combustible (or 
 coal) by 965.7. 
 
 In calculating the efficiency where the coal contains an ap- 
 preciable amount of surface moisture, allowance is to be made 
 for the heat lost in evaporating this moisture by adding to the 
 heat absorbed by the boiler the heat of evaporation thus lost. 
 The percentage of surface moisture used in this calculation is 
 that which is found in the manner described in Article XIV 
 of Code. 
 
 XXI. The Heat-balance. An approximate "heat-bal- 
 ance," or statement of the distribution of the heating value of 
 the coal among the several items of heat utilized and heat 
 lost may be included in the report of a test when analyses of 
 the fuel and of the chimney gases have been made. It should 
 be reported in the following form : 
 
APPENDIX. 
 
 '93 
 
 HEAT BALANCE, OR DISTRIBUTION OF THE HEATING VALUE OF THE COM- 
 BUSTIBLE. 
 
 Total Heat Value of i Ib. of Combustible B. T. U. 
 
 B. T. U. Per Cent. 
 
 1. Heat absorbed by the boiler = evaporation from and at 
 
 212 degrees per pound of combustible X 965.7. 
 
 2. Loss due to moisture in coal = per cent of moisture re- 
 
 ferred to combustible -5- 100 X [(212 /) + 966 
 0.48(7^ 2i2)](* = temperature of air in the boiler 
 room, T = that of the flue gases). 
 
 3. Loss due to moisture formed by the burning of hydrogen 
 
 = per cent of hydrogen to combustible -i- 100 X 9 
 X [(212 - /) + 966 -f o.48(r - 212)]. 
 
 4.* Loss due to heat carried away in the dry chimney gases = 
 weight of gas per pound of combustible X 0.24 X 
 (T-t). 
 
 CO 
 5.f Loss due to incomplete combustion of carbon = .^-p 
 
 X 
 
 per cent C in combustible 
 
 .. 
 
 -\- CO 
 
 100 
 
 X 10150. 
 
 6. 
 
 Loss due to unconsumed hydrogen and hydrocarbons, to 
 heating the moisture in the air, to radiation, and 
 unaccounted for. 
 
 Totals 
 
 100.00 
 
 * The weight of gas per pound of carbon burned may be calculated from the gas analyses 
 as follows : 
 
 Dry gas per pound carbon 
 
 - ta which co <- 
 
 the percentages by volume of the several gases. As the sampling and analyses of the gases 
 in the present state of the art are liable to considerable errors, the result of this calculation is 
 usually only an approximate one. The heat-balance itself is also only approximate for this 
 reason, as well as for the fact that it is not possible to determine accurately the percentage 
 of unburned hydrogen or hydrocarbons in the flue gases. 
 
 The weight of dry gas per pound of combustible is found by multiplying the dry gas per 
 pound of carbon by the percentage of carbon in the combustible, and dividing by too. 
 
 t CO 2 and CO are respectively the percentage by volume of carbonic acid and carbonic 
 oxide in the flue gases. The quantity 10150 = No. heat-units generated by burning to car- 
 bonic acid one pound of carbon contained in carbonic oxide. 
 
 XXII. Report of the Trial. The data and results should 
 be reported in the manner given in the following table, omit- 
 ting lines where the tests have not been made as elaborately 
 as provided for in such table. Additional lines may be added 
 for data relating to the specific object of the test. The extra 
 lines should be classified under the headings provided in the 
 
194 APPENDIX. 
 
 table, and numbered, as per preceding line, with sub letters, 
 a, b, etc. 
 
 DATA AND RESULTS OF EVAPORATIVE TRIALS. 
 
 Made by of boiler at to 
 
 determine. 
 
 Principal conditions governing the trial 
 
 Kind of fuel .... 
 
 State of the weather 
 
 1. Date of trial 
 
 2. Duration of trial hours. 
 
 Dimensions and Proportions. 
 
 (A complete description of the boiler should be given on an annexed 
 sheet.) 
 
 3. Grate surface width length area sq. ft. 
 
 4. Water-heating surface 
 
 5 . Superheating surface 
 
 6. Ratio of water heating surface to grate surface 
 
 7. Ratio of minimum draft area to grate surface 
 
 Average Pressures. 
 
 8. Steam-pressure~by gauge Ibs. 
 
 9. Atmospheric pressure by barometer in. 
 
 10. Force of draft between damper and boiler 
 
 1 1 . Force of draft in furnace 
 
 12. Force of draft in ash-pit 
 
 Average Temperatures. 
 
 13. Of external air deg. 
 
 14. Of fire room 
 
 15. Of steam 
 
 16. Of feed water entering heater 
 
 17. Of feed water entering economizer 
 
 18. Of feed water entering boiler 
 
 19. Of escaping gases from boiler - 
 
 20. Of escaping gases from economizer 
 
APPENDIX. 
 
 '95 
 
 Fuel. 
 
 21. Size and condition 
 
 22. Weight of wood used in lighting fire Ibs. 
 
 23. Weight of coal as fired * 
 
 24. Percentage of moisture in coal \ percent. 
 
 25. Total weight of dry coal consumed (Art. XIV, Code) Ibs. 
 
 26. Total ash and refuse 
 
 27. Total combustible consumed 
 
 28. Percentage of ash and refuse in dry coal per cent. 
 
 Proximate Analysis of Coal. 
 
 Of Coal. Of Combustible. 
 
 29. Fixed carbon per cent. per cent. 
 
 30. Volatile matter 
 
 31. Moisture 
 
 32. Ash * 
 
 100 per cent. 100 per cent. 
 
 33. Sulphur, separately determined " " 
 
 Ultimate Analysis of Dry Coal. 
 (Art. XVI, Code.) 
 
 34. Carbon (C) per cent. 
 
 35. Hydrogen (H) 
 
 36. Oxygen (O) " 
 
 37. Nitrogen (N) 
 
 38. Sulphur (S) 
 
 100 per cent. 
 
 39. Moisture in sample of coal as received " 
 
 Analysis of Ash and Refuse. 
 
 40. Carbon per cent. 
 
 41. Earthy matter " 
 
 Fuel per Hour. 
 
 42. Dry coal consumed per hour Ibs. 
 
 43. Combustible consumed per hour " 
 
 44. Dry coal per square foot of grate surface per hour " 
 
 45. Combustible per square foot of water heating surface per 
 
 hour " 
 
 * Including equivalent of wood used in lighting the fire, not including unburnt coal with- 
 drawn from furnace at end of test. One pound of wood is taken to be equal to 0.4 pound of 
 coal. 
 
 t This is the total moisture in the coal as found by drying it artificially, as described in Art. 
 XIV of Code. 
 
ig6 
 
 APPENDIX. 
 
 Calorific Value of Fuel. 
 
 46. Calorific value by oxygen calorimeter, per pound of dry 
 
 coal B. T. U. 
 
 47. Calorific value by oxygen calorimeter, per pound of com- 
 
 bustible " " " 
 
 48. Calorific value by analysis, per Ib. of dry coal* " " " 
 
 49. Calorific value by analysis, per pound of combustible " " " 
 
 Quality of Steam. 
 
 50. Percentage of moisture in steam per cent. 
 
 51. Number of degrees of superheating deg. 
 
 52. Quality of steam (dry steam = unity) 
 
 53. Factor of correction for quality of steam (page 119) 
 
 Water. 
 
 54. Total weight of water fed to boiler , Ibs. 
 
 55. Water actually evaporated, corrected for quality of steam 
 
 56. Equivalent water evaporated into dry steam from and at 
 
 degrees 
 
 Water per Hour. 
 
 57. Water evaporated per hour, corrected for quality of steam " 
 
 58. Equivalent evaporation per hour from and at 212 degrees. " 
 
 59. Equivalent evaporation per hour from and at 212 degrees 
 
 per square foot of water-heating surface " 
 
 Horse-power. 
 
 60. Horse-power developed. (34^ Ibs. of water evaporated 
 
 per hour intodry steam from and at 212 degrees, equals 
 
 one horse-power)f H. P. 
 
 61. Builders' rated horse power " 
 
 62. Percentage of builders' rated horse-power developed per cent. 
 
 Economic Results. 
 
 63. Water apparently evaporated per Ib. of coal under actual 
 
 conditions. (Item 54 -5- Item 23) Ibs. 
 
 64. Equivalent evaporation from and at 212 degrees per Ib. of 
 
 coal (including moisture) 
 
 65. Equivalent evaporation from and at 212 degrees per Ib. of 
 
 dry coal 
 
 66. Equivalent evaporation from and at 212 degrees per Ib. of 
 
 combustible 
 
 * See formula for calorific value under Article XVI of Code. 
 
 t Held to be the equivalent of 30 Ibs. of water per hour evaporated from 100 degrees Fahr 
 into dry steam at 70 Ibs. gauge-pressure (See Introduction to Code.) 
 
APPENDIX. 197 
 
 Efficiency. 
 (See Art. XX, Code.) 
 
 67. Efficiency of the boiler ; heat absorbed by the boiler per Ib. 
 
 of combustible divided by the heat-value of one Ib. of 
 combustible.* per cent. 
 
 68. Efficiency of boiler, including the grate ; heat absorbed by 
 
 the boiler, per Ib. of dry coal fired, divided by the heat 
 value of one Ib. of dry coal.f 
 
 Cost of Evaporation. 
 
 69. Cost of coal per ton of 2240 Ibs. delivered in boiler-room... $ 
 
 70. Cost of fuel for evaporating 1000 Ibs. of water under ob- 
 
 served conditions $ 
 
 71. Cost of fuel used for evaporating 1,000 Ibs. of water from 
 
 and at 212 degrees $ 
 
 Smoke Observations. 
 
 72. Percentage of smoke as observed 
 
 73. Weight of soot per hour obtained from smoke-meter. 
 
 74. Volume of soot obtained from smoke-meter per hour 
 
 * In all cases where the word " combustible " is used, it means the coal without moisture 
 and ash, but including all other constituents. It is the same as what is called in Europe " coal 
 dry and free from ash." 
 
 t The heat value of the coal is to be determined either by an oxygen calorimeter or by cal- 
 culation from ultimate analysis. When both methods are used the mean value i to be taken. 
 
198 
 
 TABLE I. 
 
 TABLE I. HEAT OF COMBUSTION OF SUBSTANCES. 
 
 Calories. B. T. U. 
 
 Crystallized carbon toCO a .. 7859 14146 Berthelot 
 
 " " to CO... 2405 4329 " 
 
 Amorphous carbon to CO a . . 8137 14647 " 
 
 " " to CO. . . 2489 4480 " 
 
 Graphite to CO 2 7901 14222 " 
 
 Petroleum coke to CO a 8017 14503 Mahler 
 
 Gas coke to CO 2 8047 14485 F. & S. 
 
 Carbon vapor to CO a . . 8722 15700 \ Calculated. 
 
 I Page 173. 
 
 Coal (pure and dry) 7800 to 9000 14040 to 16200 Various 
 
 Lignite (pure and dry) 6000 to 7000 10800 to 12600 " 
 
 Beech charcoal 7140 12852 Schwackhofer 
 
 Soft charcoal 7071 12723 " 
 
 Cellulose 4200 7560 Berthelot 
 
 Soft resinous wood 5050 9090 Gottlieb 
 
 Hard wood, 4750 8550 
 
 Peat 5940 10692 Bainbridge 
 
 Cane sugar 3961 7130 Berthelot 
 
 Asphalt 9532 I7I59 Slosson & Colburn 
 
 Pitch 8400 15120 Anon. 
 
 Naphthalin 9690 16842 Berthelot 
 
 Paraffin nooo 19800 Mahler 
 
 Tallow 9500 17100 Stohmann 
 
 Sulphur 2500 4500 Berthelot 
 
 Petroleum 96001011000 172801019800 Various 
 
 Schist-oil 90001010000 16200 to'i 8000 " 
 
 Heavy coal gas oil. . . .*.. 8900 16020 Ste-Claire Deville 
 
 Cotton oil 9500 17100 Anon. 
 
 Rape oil 9489 17080 Stohmann 
 
 Olive oil 9473 17051 " 
 
 Sperm oil 10000 18000 Gibson 
 
 Hydrogen 345o 62100 Berthelot 
 
 Carbonic oxide 2435 4383 " 
 
 Marsh gas 13343 24017 " 
 
 Olefiant gas 12182 21898 " 
 
 Acetylene 12142 21856 " 
 
 Carbon vapor (diamond). .. 11134 20041 " 
 
 Coal gas 4440 to 7370 79901012266 Various 
 
 Petroleum gas 10800 19440 Anon. 
 
 Air producer gas 773 to 1370 1391 to 2466 Various 
 
 Watergas 235010 3032 423010 5458 
 
 Mixed gas 101510 1548 182710 2786 " 
 
TABLE II. 
 
 199 
 
 TABLE II. THERMOMETER REDUCTION TABLES. 
 
 C. 
 
 I 
 2 
 
 3 
 4 
 5 
 6 
 
 7 
 
 8 
 
 9 
 
 F. 
 
 1.8 
 
 3-6 
 
 5-4 
 
 7.2 
 
 9.0 
 
 10.8 
 
 12.6 
 
 14.4 
 
 16.2 
 
 A. CENTIGRADE TO FAHRENHEIT. 
 
 C. 
 
 10 
 
 20 
 
 30 
 40 
 50 
 
 60 
 70 
 80 
 90 
 
 F. 
 
 18 
 
 36 
 
 54 
 
 72 
 
 90 
 
 108 
 
 126 
 
 144 
 162 
 
 C. 
 
 100 
 
 200 
 300 
 4OO 
 5OO 
 600 
 700 
 800 
 900 
 
 F. 
 
 1 80 
 
 360 
 
 540 
 
 720 
 
 900 
 
 1080 
 
 1260 
 
 1440 
 
 1620 
 
 C. 
 
 F. 
 
 1000 
 
 1800 
 
 2000 
 
 3600 
 
 3000 
 
 5400 
 
 4000 
 
 7200 
 
 5000 
 
 9000 
 
 6000 
 
 10800 
 
 7000 
 
 12600 
 
 8000 
 
 14400 
 
 9000 
 
 16200 
 
 B. FAHRENHEIT TO CENTIGRADE. 
 
 C. 
 t 
 
 4 
 if 
 
 2f 
 2* 
 
 3t 
 
 3t 
 
 F. 
 
 10 
 
 20 
 30 
 40 
 50 
 60 
 70 
 80 
 9 
 
 C. 
 
 5f 
 
 22f 
 27* 
 
 33t 
 38* 
 44* 
 50 
 
 F. 
 100 
 200 
 300 
 400 
 500 
 600 
 700 
 800 
 900 
 
 C. 
 55f 
 
 222f 
 277* 
 
 333f 
 3 88f 
 
 444f 
 500 
 
 F. 
 
 1000 
 2000 
 3000 
 4000 
 5OOO 
 6OOO 
 7000 
 8000 
 9000 
 
 C. 
 
 555f 
 iui$ 
 i666f 
 
 2222f 
 
 2777* 
 
 33331 
 
 5000 
 
 Having given Centigrade degrees, obtain from Table A the 
 corresponding equivalents, and to their sum add 32. 
 
 Example: Find Fahrenheit degrees corresponding to 
 416 C. 
 
 720+ 18 + 10.8 + 32 = 780.8. 
 
 Having given Fahrenheit degrees, subtract 32 and find the 
 value in Table B corresponding to the remainder. 
 
 Example : Find Centigrade degrees corresponding to 
 
 -16-32= -48, - 4 8F. = - 
 
2OO 
 
 TABLES III, IV. 
 
 TABLE III. THEORETICAL FLAME TEMPERATURES. 
 
 
 In Oxygen. 
 
 In Air. 
 
 Centigrade. 
 
 Fahrenheit. 
 
 Centigrade. 
 
 Fahrenheit. 
 
 C to CO 
 
 4265 
 10000 
 
 7010 
 
 6727 
 7971 
 9659 
 
 11300 
 
 9350 
 
 2500 
 
 5400 
 
 7558 
 
 9444 
 5800 
 3000 
 3800 
 2300 
 
 7677 
 18000 
 12618 
 I2I08 
 14348 
 17286 
 20340 
 16830 
 4500 
 9720 
 13604 
 17000 
 10440 
 5400 
 6840 
 4140 
 
 1462 
 2718 
 3000 
 2674 
 2245 
 3000 
 3400 
 2790 
 1200 
 2700 
 2400 
 2730 
 2280 
 1200 
 1500 
 1060 
 
 2639 
 4892 
 5400 
 4813 
 4036 
 5400 
 6l2O 
 5022 
 2l6o 
 4860 
 4320 
 4914 
 4104 
 2l6o 
 2700 
 1908 
 
 C to CO 2 
 
 CO to CO 3 
 
 
 
 Olefiant gas C 2 H 4 
 
 
 Benzin CeHe 
 
 
 
 
 Naphthalin 
 
 Wood 
 
 
 Coal (bituminous) 
 
 Sulphur to H 2 SO 4 
 
 
 TABLE IV. WEIGHT AND VOLUME OF GASES. 
 
 Name. 
 
 Weight. 
 
 Volume. 
 
 Per Cubic 
 Metre in 
 Kilograms. 
 
 Per Cubic 
 Foot in 
 Pounds. 
 
 Per Kilogram 
 in Cubic 
 Metres. 
 
 Per Pound 
 in 
 Cubic Feet. 
 
 Air 
 
 .29318 
 .25616 
 .4298 
 0.08961 
 .9666 
 .2515 
 .0727 
 0.8047 
 2 . 8605 
 I.25I9 
 
 0.7155 
 I.igOO 
 
 3-3333 
 I.34I5 
 
 0.08073 
 0,07845 
 0.08926 
 0.00559 
 0.12344 
 0.07817 
 0.06696 
 0.05022 
 0.1787 
 0.07814 
 0.04466 
 0.07428 
 0.208 
 0.08565 
 
 0.773 
 0.796 
 0.699 
 11.160 
 0.508 
 0.800 
 0.932 
 1.242 
 
 0.349 
 0.799 
 
 1-397 
 0.840 
 0.303 
 0.746 
 
 12.385 
 12.763 
 I I . 203 
 178.83 
 8.147 
 12.800 
 14.930 
 19.912 
 5.596 
 12.797 
 22.391 
 13.456 
 4.808 
 11.950 
 
 
 
 
 
 
 Carbon vapor 
 
 
 
 
 Methane CH 4 
 
 Acetylene, C 2 H a 
 Benzine CeHe 
 
 
 
TABLE V. 
 
 20 1 
 
 6 
 
 5 
 
 u 
 
 
 .u 
 
 s^Dnpojj 
 
 oo n M ji 4 N 
 
 m w w 
 
 a 
 i 
 
 JU 
 
 
 
 jiy 
 
 f 1 1 1 1 1 
 
 I 
 
 '5 
 
 
 
 00 ^ M VO fO M 
 
 il 
 
 t5 S 
 
 2c3 
 
 0% 
 
 .Q 
 S 
 o 
 U 
 
 1 
 
 sionpojj 
 
 t& TO 8 ?. ^ 
 . S . ? T ? ? 
 
 1] 
 
 Ug 
 
 fl a 
 
 
 
 
 uaSXxQ 
 
 O >o fi O O oo 
 
 10 CT ON in oo tn 
 \o en o* oo o^ o> 
 
 M o o in c5 
 
 | 
 
 "o 
 
 > 
 
 
 
 aiqiisnq 
 ) Sri03SB) 
 
 in ?! ^ ^. *> 
 
 O O O M O 
 
 & 
 
 
 
 sjDnpojj 
 
 ^j n ci O "O *O 
 
 > 8 8 8 a 8cc 8 
 
 11 
 II 
 
 
 
 M.O 
 
 300000 o 
 
 E^ 
 
 cS 
 
 
 
 
 |0 U 8 DC + + 
 
 "o 
 
 
 .w 
 
 ,,n P o, d 
 
 j^ cJ vo rn n oo n 
 
 4, 
 
 1 
 
 B 
 
 uiy 
 
 o s g 5 1 I 
 
 5'i 
 
 mm 
 
 i 
 
 a 
 
 
 
 
 U' 
 
 ag 
 
 f 
 
 js 
 a 
 
 o 
 
 u 
 
 a 
 
 spnpojj 
 
 . t^ m M o O oo 
 
 .2 vo m n O 6 * 
 j^ rn ' M o> in -4- 
 
 1 
 
 
 
 
 o 
 
 i a R I i i 
 
 ja^ w M d oo -J- m 
 
 I 
 
 8 
 
 
 
 s^onpojj 
 
 II II II II II II II II 
 
 o" R o CT o^c, c . 
 
 O w U ffi UK UK 
 
 
 
 | 
 
 "3 
 
 1 
 
 
 
 U33XXQ 
 
 2 9 
 
 
 
 
 
 S 8 * " "8 
 
 
 
 Combustibles. 
 
 
 a c & S S 
 
 II llf 
 
 S 13 ' -S 
 u u u K S w 
 
2O2 
 
 TABLE VI. 
 
 COCO CO >H 
 
 jonpojj 
 
 saiqnsnq 
 
 Sg 
 
 il 
 
 11 
 5 ^ 
 
 jiy 
 
 sionpojj 
 
 siDnpojj 
 
 II 
 
 w ... 
 
 a >> q> o* o o t- 
 
 COO CO CO CO 
 
 M Tl- W M 
 
 oo rf co 
 
 ood .6-o". 
 
 CO 
 
 M M C, 
 
 E 
 
 Tf- N 
 
 U^ CJ 
 
 c O co 
 
 N CO 
 
 CO O^ 
 
 co m 
 
 CO M t-> 
 
 C?> Ooo co 
 vn r>. rt- r^ 
 
 M in 
 
 w co 
 
 O^ O 
 
 co 
 
 CO M M 
 
 ^s 
 
 CO c M O> in 
 
 45 
 
 CO M 
 
 co t^ 
 
 co in 
 
 "tvO CO O 
 Tf COCO CO 
 
 ^OCD^ 
 run: 
 
 I! II 
 
 O C 
 
 CO N 
 
 UUUK 
 
 
 W 
 
TABLE VII. 
 
 203 
 
 W 
 
 
 II 
 
 < < 
 w 
 ac 
 I 
 
 g 
 
 - 
 
 co Tf O coo co 
 
 a> <N o o -3- co 
 
 N O n *^> i^- O 
 
 O i^ o o Tt r^ 
 oo oo O O O Tf 
 to m M in co CO 
 
 M o r 
 4% M Cl H 
 
 u ; 
 *1 
 
 Bcor^MOr^* 
 CT> M M CO CO 
 M O *> tj- COO ' 
 
 N C*CQ M NO 
 
 M M o -^ "3-O 
 
 COOO I~^O^N COCOCO 
 
 8r^o oo co 
 M \r> o^ co 
 M Ococo co 
 
 co M 
 co ^- 
 coO 
 
 a^MMNCOTfOO 
 OC1MC4C4M C4 M 
 
 MOO O O MO comco 
 & COO u-> rj- O < CO <* 
 O O rj-wo -"I- O OM 
 
 Sco P d O 
 ^ ^j-co i 
 
 1OCOM M rt- 
 
 giiii 
 
 t^ u 
 
 O O O O O 
 
 uuuuuu 
 
 O O O O O 
 
 S K S gi dd jo 
 3 *^ J3 jcs W ***<*< 
 
 ^ w'S'S <u cti aj rt 
 
2O4 
 
 TABLE VIII. 
 
 ills Tg 
 
 1 1 1 1 
 
 I 
 
 S 
 
 5 
 
 I 
 
 
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 Sulphurous acid 
 
 Aqueous vapor . 
 
TABLES IX, X, XI. 2O$ 
 
 TABLE IX. TABLE OF SPECIFIC HEAT OF GASEOUS PROD- 
 UCTS OF COMBUSTION REFERRED TO THE PROPORTION 
 OF CARBONIC ACID. 
 
 Proportion of 
 Carbonic Acid. 
 
 Specific 
 Heat. 
 
 Proportion of 
 Carbonic Acid. 
 
 Specific 
 Heat. 
 
 5 per cent 
 6 " " 
 
 0.312 
 0.3H 
 
 1 1 per cent 
 
 12 " " 
 
 0.319 
 O.320 
 
 >j n (i 
 8 " 4< 
 
 0.315 
 0.316 
 
 13 " " 
 14 " " 
 
 0.321 
 0.322 
 
 9 " " .... 
 
 10 " " 
 
 0.317 
 0.318 
 
 15 " " 
 
 0.323 
 
 TABLE X. HEAT OF VAPORIZATION OF WATER AT o TO 
 
 230 C. 
 
 Temperature. Heat of 
 
 Centigrade. Fahrenheit. Vaporization. 
 
 o 32 606.5 
 
 IOO 212 537-0 
 
 230 456 676.6 
 
 Latent heat of vaporization, 966 (Regnault). 
 
 TABLE XL SPECIFIC HEAT OF WATER (REGNAULT). 
 Temperature. Specific Heat. Temperature. Specific Heat. 
 
 o i. oooo 110 1.0153 
 
 10 1.0005 120 I.OI77 
 
 20 1. 0012 130 I.02O4 
 
 30 I.OO2O 140 I.O232 
 
 40 1.0030 150 I.O262 
 
 50 1.0042 160 1.0294 
 
 60 1.0056 I7O 1.0328 
 
 70 1.0072 1 80 1.0364 
 
 80 I.OOgS 190 I.040I 
 
 90 1.0109 2O 1.0440 
 
 ioo 1.0130 
 
206 
 
 TABLES XII, XIII. 
 
 TABLE XII. VOLUME OF OXYGEN TO FORM WATER WITH THE 
 HYDROGEN OF COAL. 
 
 Per Cent of Hydrogen. 
 
 Oxygen in Litres per 
 Kilogram of Coal. 
 
 2 , 
 
 I 12 
 
 3 . 
 
 168 
 
 
 . . 223 
 
 4. 
 C.. 
 
 . 270 
 
 6 
 
 . 335 
 
 7.. 
 
 301 
 
 8 
 
 . 446 
 
 Q.. 
 
 , S02 
 
 Oxygen in Cubic Feet 
 per Pound of Coal. 
 
 .896 
 1.792 
 2.699 
 
 3.585 
 4.481 
 
 5-397 
 6.283 
 7.170 
 8.096 
 
 TABLE XIII. QUANTITY OF AIR REQUIRED FOR PERFECT 
 COMBUSTION OF FUELS. 
 
 Fuel. 
 
 Composition. 
 
 Air per 
 
 Carbon. 
 
 Hydrogen. 
 
 Oxygen. 
 
 Nitrogen. 
 
 Kilogram. 
 
 Pound. 
 
 Coke 
 
 ^98.0 
 
 95-4 
 87.0 
 85.0 
 84.0 
 77.0 
 90.0 
 71.0 
 58.0 
 50.0 
 85.0 
 68.7 
 58.0 
 34-0 
 
 I.O 
 
 0-5 
 2.2 
 5-0 
 
 5-0 
 6.0 
 5-o 
 
 2.O 
 
 5-0 
 
 6.0 
 6.0 
 14.0 
 22.5 
 23.7 
 5-9 
 5-0 
 
 
 
 cu. metres 
 10.09 
 9.01 
 
 8-93 
 8.68 
 8.79 
 7.67 
 8.53 
 7.02 
 
 5-75 
 4-57 
 10.76 
 14.20 
 
 14-51 
 3.16 
 
 .72 
 
 cu. feet 
 162.06 
 144.60 
 143.40 
 
 139.41 
 141.07 
 
 123.15 
 I33.9 
 112.43 
 92.36 
 73.36 
 172.86 
 227.93 
 233.06 
 50.70 
 11.56 
 
 Coal, anthracite 
 bituminous . . 
 
 1.8 
 4.0 
 6.0 
 8.0 
 15.0 
 
 0.5 
 
 
 
 cannel 
 smithy 
 
 
 
 
 
 19.0 
 30.0 
 42.0 
 I.O 
 I.O 
 
 1.4 
 
 43-o 
 
 21. 
 
 
 
 
 Wood dry 
 
 I.O 
 
 
 Natural gas. . . 
 
 6.2 
 
 3-8 
 3-4 
 69.0 
 
 
 
 Producer gas 
 
 
TABLES XIV, XV. 2O? 
 
 TABLE XIV. RELATION BY WEIGHT AND VOLUME OF THE 
 COMPONENTS OF AIR. 
 
 Air contains by volume : 
 
 Nitrogen 78.35 
 
 Oxygen 2O. 77 
 
 Aqueous vapor 0.84 
 
 Carbonic acid 0.04 
 
 100.00 
 
 Deducting the carbonic acid and aqueous vapor, we have : 
 Nitrogen. . ..By volume: 79.04 By weight : 76.83 
 
 Oxygen " " 20.96 " " 23.17 
 
 100.00 100.00 
 
 Ratio of nitrogen to oxygen : 
 
 N N 
 
 By volume, = 3.771. By weight, =3-32. 
 
 Ratio of air to oxygen : 
 
 Air A ir 
 
 By volume, = 4.771. By weight, = 4.315. 
 Ratio of air to nitrogen : 
 
 Air Air 
 
 By volume, = 1.265. By weight, = 1.302. 
 
 TABLE XV. IGNITION POINT OF GASES (Mayer and Munch)^ 
 
 Marsh gas, CH 667 C. 
 
 Ethane, C a H 6 616 
 
 Propane, C 3 H t 547 
 
 Acetylene, C 2 H a 580 
 
 Propylene, C 3 H a 504 
 
 * Berichte der deutscher Gesellschaft xxvi, 2421. 
 
FUEL TABLES. 
 
 These tables contain all the available information covering 
 the data required which have been published to date. They 
 contain analyses of the fuels, and the heat units as determined 
 by the authors, whose names are given. In some cases it has 
 been necessary to recalculate the results as published by the 
 experimenters to conform with the standard adopted. This 
 applies especially to the coals and solid fuels, the data for 
 which are given based on pure dry coal, i.e., on the combus- 
 tible present. If the actual test of the sample as given is 
 desired, it will be easy to make the necessary deductions. 
 Some of the cokes and some of the natural gases have been 
 calculated, the calculated results being within the limits of 
 
 experimental error in these cases. 
 
 209 
 
210 
 
 FUEL TABLES. 
 
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218 
 
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 d 6 
 
 |4 
 
 M M 
 
 6 
 
 uaSXxo 
 
 s ^ 
 
 ci to 
 
 vO rf 
 CO\O 
 \O vo 
 
 *> 
 
 > i 
 
 S 
 
 O 
 
 jnqd[ns 
 'u33cu}ix 
 'uaSAxo 
 
 
 
 1 
 
 uaSojpAn 
 
 co O 
 
 H- CJ 
 4 <* 
 
 5*- CO 
 
 o a 
 
 r> ^- 
 
 
 5 
 
 O O 
 
 ^T Tf 
 
 t9 
 
 ?D O COO vovovovovovoCO 
 
 ^g coo O Ococc OOt^ 
 
 H 
 
 CO CO 
 
 r^ r 
 
 ^'cooo t^cococococococo 
 
 c w 
 5 1 
 
 N M O O 
 
 vO 00 t-i 
 
 r^ vo o ""> Tf 
 O co O *> m 
 
 CO VOCO VOt^vOVOvOVOQ CO 
 COVOCOMONCOOOMrf 
 
 d 
 
 co r^- co co 
 
 O vO vo <f vo 
 
 CO CO CO CO CO 
 
 rt CO O vo O OO TJ- t^ W vo 
 eococococococococococo 
 
 i 
 
 W co r> N 
 
 M T(- r^ vn 
 
 VO to O VO Tf 
 
 Tj- N M M N 
 
 vo vo vo voco O O O O to O 
 t^ t^ N t~^ OO O co r->> vo co 
 
 & 
 
 10 <3- vo T 
 
 vovC t^O O 
 vo vo vo vo vo 
 
 co M rt-co M o) vo r^. TJ- coco 
 
 ^J-VOTJ-COVOTj-T^-Tj-TfVO^h 
 
 a 
 
 o 
 
 :::: 
 
 : : : ; w : 
 
 C . ' 
 
 5 - : ; 
 
 I 
 
 * 0) * 
 
 . ,-^,-v^ - bfl 
 
 % c! e . ** ; ; 
 r?||| ; : :| i : 
 
 iJ 
 
 15 
 I 
 
 i i >*, i . 
 a 
 
 L^, s 
 
 <j 
 I 
 
 : * s S 
 
 -E-sSi- -5- 
 
 il 
 
 ||i3 3 5 
 
 o -^ 
 c^ H 
 
 ^ ^oj^ug Srto 
 
 ^> aj^'^rt^ tx a ^ 
 
 J- c ^ J5- 2 : 3 J J3 
 
 <J <p3Mpqfq pquu 
 
COAL. 
 
 2I 9 
 
 Heat Units of 
 Combustible. 
 
 u 
 
 \f> Tt-o to M Tf coco o M r^ r>. M TI- u-> <^ co ^ M 
 M N N O tr>O r^ CO O to M co 0< O co O CO WvO 
 co Tf w M N TtM CON w ^^^TtN (N COCOM 
 
 MO O 
 Tfcnco 
 
 ON ^ CM r-* COCO ^ CO M N CO COO MCOU^ 
 
 Q M M r^r>cor^coO u->r^co O^O 'l-vn 
 co a>oo TT o M o ^t- r^ ooo a^co oo M o O co 
 ooo r^.t^oo t-t^r^r^r^i^ 
 
 qsy 
 
 to to O *o O to to O O O O O O tn 
 N co ^-co to O O f^ M co tno co M 
 O 
 
 t~^oo rj- <f to O M 
 co ^- in M d to M 
 
 anqdjns 
 
 co or s Ot^OO 
 O Ovnor^r^tn 
 
 TfO'^-coOrj-ooo 
 couirtoocot-.ovo 
 
 M M d d d NW" d4ddddddddddo'dddd 
 
 NO 
 
 
 
 jnqd[ng 
 
 r) incovnr>O coO mxnoo tncomOoo O O O Ocooo tr>OcoO 
 j!,O ^-^ N O^t^ 1 - 1 r-oco ^- d T}-a>M inxotoMO O toco 
 
 [>.Oco r>.co 
 
 oco i^oooo 
 
 O O cotnmOco N vDiocovnoo O O w tno O tncoaj too COM 
 too^OcoNOMVoOOMdOcooOt^MCONOtnO^tot^m 
 
 
 totntoO O OtoQ O OtoQvotoOOtoO OoO O O O*oto 
 t^r^rcoO O t^o^cotoo ^MOO ^M o PI w too r^tococo 
 rj- r^- r>. *i-cd Tt-'^cotoN coto\r>to r~co o co ^ ^cd to too O O 
 
 rfl^^^-^-tO^-Tj-rJ-Tt-Tt-tOtOlOTl-Tj-intO^-tOT^tOtOtOtOtO 
 
22O 
 
 TABLES. 
 
 Heat Units o 
 Combustible. 
 
 qsy 
 
 uwu 
 
 loO^S' 
 
 to 04 O"* CO 
 
 O oo M 
 
 4tA 4 
 
 . 
 
 dcJdoddd 
 
 r^ M M O 
 
 mo O O 
 
 O O 
 
221 
 
 Authority. 
 
 ll 
 
 JH 
 
 3 '. - - - - - 
 
 Q 
 
 G 
 
 c/5 " c/5 
 
 21 H' 
 
 O O O O M 
 O co O HI co O 
 co t to N in N 
 m mO m mo 
 
 U"> U") V) U"> VD IT) U") IO 
 
 CO O O O tOO N 
 t HI t ON CO O HI 
 
 O moo O in t O 
 in m m m m m in 
 
 CM PQ 
 
 
 
 
 sj i 
 
 CJ 
 
 80 o o o o 
 O O v> m Q 
 mo N tO O 
 
 CO CO O^CQ CO ON 
 
 8t O O O O O 
 O O co in o m co 
 co oo O t 10 in t t 
 
 cocooocococococo 
 
 O O O O O O O 
 O m O N coo t 
 coo co r^o m co 
 
 CO 00 CO OO CO CO CO 
 
 qsy 
 
 
 
 
 -M 
 
 
 
 
 
 
 0^8 
 
 t ON in ON t CO 
 
 co o O oo co r- 
 
 O CO t HI ON ON O 
 ON ON ON ONCO f-^ O 
 
 
 O O O M 
 
 000000 
 
 O O O O O O O 
 
 jnqdjns 
 
 t 
 O co COO tO 
 
 1^ OO N CO t m O> 
 
 m co m r^ r^ m M 
 
 O r^ t N in too 
 t^co O M t^oo o 
 
 
 O CO M M t HI 
 
 co M O *o N O CM 
 
 co o> tn in M N oo 
 
 
 
 
 
 
 
 w r-.'w t 
 
 ^t too o co M o 
 
 N O ""> l* ON CO M 
 
 o co r^ coco M t>. 
 
 CO ON HI HI s t t^ 
 
 
 tt tco t t 
 
 rj- O t CO COO t 
 
 O, CO t CO rf >0 CO 
 
 | 
 
 in 
 
 t N in O HI O 
 
 ON CO O O CO f HI 
 M O ON t N M l^ 
 
 in o ON m t^ in m 
 ON c* oo r^ o* t^ m 
 
 H 
 
 00 ONCO OO ONCO 
 
 N N t O co r- co 
 
 O^ ONCO ONCO CO s 
 
 to O HI N HI r^ 
 
 CO OO ON ONCO CO CO 
 
 1 t 
 
 O O COCO O 
 
 O HI l^ in O ON 
 
 O co r^ in co M i- 
 
 m ON m M ON O O 
 
 6 1 
 
 tO t** HI CO 
 
 t^ N CO O CO 
 
 m ON t co en O HI 
 
 1 
 
 CO CM vN vN t 
 
 N ON M HI CO t 
 
 CO N COO N f^ t 
 
 E 
 
 to r- CM o 
 co oo r^ co r^ 
 
 tMO N t >/> 
 
 CO OO OO OO CO CO 
 
 ONO O oo oo inO 
 
 
 : : 
 
 : : : : : : 
 
 
 c 
 _o 
 
 i 
 a 
 
 *u *.9 P 'S 
 
 JJ S 
 
 1 -*"3% ** 
 
 jjftjlj! 
 
 1 *::::: 
 
 o 
 
 0) 
 
 ^ <u ^ 
 
 I'll ' 
 
 
 
 
 
 u^l 
 
 B an t/t 
 
 
 l-l- - . I 
 11 "1 
 
 I s "ill" 
 
 s ^ a ' ' c 
 
222 
 
 FUEL TABLES. 
 
 
 
 ! 
 
 Q 
 j 
 1 
 
 Q 
 
 s 
 
 TD 
 
 Q P 
 S 
 
 3 
 
 < 
 
 S3 
 
 . v. d T 1 
 
 05* JScd 
 
 V, 
 
 I-J( 
 
 H 3." " " CS 
 
 0) . . 
 
 58 w c/5 " c/i 
 
 *3ji R 
 2r2 ^ 
 
 N CO O* CM 
 
 xn o co cr 
 xn xn xn xn 
 
 TtOOOCMOOO 
 co Tf M o r^-o co CN 
 
 OMOOO^OOO 
 CO ^- CM O coco CM O 
 
 c| 
 
 
 
 
 Si s 
 
 Si "g 
 
 E^ 13 
 
 CJ 
 
 ^vg^^ 
 O xn t-^ TJ- 
 
 CO CO CO CO 
 
 coxnOOOOOO 
 OOOO^OOC 
 
 co co a< o o CT>CO cc 
 
 coco o^ t^co co o^co r>. 
 cococococococoaoco 
 
 qsy 
 
 
 xn 
 
 q 
 iA 
 
 
 J3}12^ 
 
 
 xn 
 
 ^1- 
 
 CO 
 
 
 uaScuiiN 
 
 M QN ^ 
 
 6 o M 6 
 
 xn T^- 
 O CT 
 
 M 
 
 Sco O xn 
 CO CO CM 
 
 MO MM 
 
 jnqd[ns 
 
 ioS 
 
 CO M CO t^CO OO 
 
 3-SS-o8 S 
 
 'uaSXxo 
 
 n-cM-xn 
 
 M 
 
 Oxn^^cor-xn o 
 
 uaSXxQ 
 
 
 o 
 
 CO 
 
 ! 
 
 
 O^oo ^* t^* 
 
 vS^ 5-2 ct S 1 ^ 
 
 cTS O^M^^g' c^ 
 
 aaSojpXn 
 
 co co u> en 
 
 xn xn * Tt -t co xn Tf 
 
 xn x xn xr> ^ rt xn ^> 
 
 3 
 
 co mvo xn 
 
 S M^S'^^^O 
 
 'g S'^^^^g' ^ 
 
 o 
 H 
 
 O^CO CO O^ 
 
 c^icsaa^^^ 
 
 c^^^c^^gc? g 
 
 c Ji 
 
 rf O CM 
 co co O 
 
 vO co r^ O coco 
 
 a> xn a> o co CM 
 co r^ CT>CO w so 
 
 rt "o 
 
 CO rr rfr 
 
 CO O O * O N 
 
 r^ N xno O Tt 
 
 U > 
 
 M 
 
 M CM M 
 
 MM M 
 
 1 
 
 2c? g 
 
 t^- CM O 
 
 ^-^2^195 
 
 xn^l^co 
 
 
 
 00 TT 
 
 
 
 ^ 
 
 
 . ^ 
 
 j 
 
 "u 
 
 a 
 
 ^ 3. 
 ' > 
 
 ;iiUiJi 
 
 J3 j_, ""> 
 
 s 
 
 o 
 _} 
 
 s c - 
 
 4 c s 
 
 | :-i.:|J.s 
 
 J g * * tiO 
 
 
 
 2* ^p ^1"H^_r1 *J S 
 
 
 a 
 
 i 
 
 
 ^ l : 5l 
 
 13 , IMIII 
 
 "'-;j 
 
 
 I'll 
 
 o u S 
 
 ! || 
 
COAL. 
 
224 
 
 TABLES. 
 
 MJ3 
 
 'I 
 
 pq 
 
 1 
 
 ^ -g 
 
 tt en 
 
 co ^ M w 
 
 o co vn 
 
 o w '3- 
 r^coO 
 
 r^ mco co cc 
 
 O co rj- 
 ino i~^ 
 MHC> 
 COCOM 
 
 r^o F F* F-O co F* 
 
 r> T^- oj co o co O F* o co O 01 F* 
 coco O^cx w ^miH CON N ^r^ 
 r^ror^t^r^r^r^r^r^t^-r^r^t^ 
 
 qsy 
 
 jnqdjns 
 
 O Tf O COO vO 
 
 vnu-> vnco 
 
 Modddddddo'do'dd 
 
 CO !> M !>. ^ rf'OO M 
 "^ O^!^^? ^nCO d^O 
 
 \r>^O O ^ N Tfrfcoci ^COM N TJ- 
 
 Nwdddddddddddd 
 
 MQ>>HCOCOCOCO oi^-co O*nvnMxncoOco*ncoor^com 
 
 M t^ 
 
 CO CO CO 
 
 co O O 
 co O t^ 
 
 & 
 
 
 C/2 
 
 ?ir "i. 
 
 ^ " t> c/2 ti h .S'S 
 
 KH ^^^ *j 5^ ~ V V O 
 
 ', g bJD^ r^ 3" "a tio ~ O r-g "& t-i 
 
 a JaJSj M^SjS.s^S>;gS 
 
 5 HI -0^-5 SP'gs? 2 SP 
 
 ? ffil glslJIIIilcS^a 
 
COAL. 
 
 22$ 
 
 Q P 
 1 = 1 
 
 < 
 
 C/2PQ 
 
 ooJ 
 
 cnco 
 r^r^u^co M in 
 
 co vricovr>Ti-co 
 
 O O 
 i- 1 O M 
 
 TcOCT>co 
 co^Oi-< O 
 i-1 TJ-M MO 
 
 -iO NCO 
 r^uifjO 
 
 co O^ mo coOOOQOOOO't' voo co t^ 
 
 O or^Tj-O i '~>NwO"^OwNcoMoou">i~iao*4-u>t->.r~o^u">co 
 
 coco r^r^cococo r^oocococococococo r^co r^t^r^oocooo t^oo 
 
 qsy 
 
 anqdtng 
 
 ddodoMciowMod 
 
 \rt \f> 
 
 M ci 
 
 dddddddoM 
 
 mo^O O^O^OvO 
 co N CT> M 
 
 
 ONO O O to O O vnoo r^co co O 
 ^^^^^^ri-Ti-Tf^ntnir*^ 
 
 M r>-o^vOoo coeoo N 
 
 vO Tt- W ON W W M ^- 0> 
 
 1-to coo O eococoMco M tntHM CON QNM ^Tt--cot 
 
 OOCOOOCOCOCO I^COCOCOOOCO t^OOCOCOOOCOCO t^COCOCOCOCOCO 
 
 2 S 8 2"g 8 8 
 
 M <O C COO M CO 
 
 Omoooom 
 
 si 
 
 o 
 
 f tf i3^S 
 
 . . i3^ 
 
 
226 
 
 FUEL TABLES. 
 
 
 Heat Units of 
 Combustible. 
 
 t-^O M in M o co too O O 
 
 Tt <fr J^ *1- M W Oco in O O O CO co 
 
 o O "> co coco NOO-^Oc^oi 
 W O t^ r- -rt OOO u-i >H o en COO 
 OO UITCOO O^c< 
 
 -CO O 
 OcO 
 
 M xr> M O^QO t^ M 
 
 qsy 
 
 t>.T-cor^>r)eo wcooco O 
 
 *3-MMOr^c/*MNOv>OMTj-Oxn OO i^ M co O co 
 coOco O O r- <3- M N r^t^o mco d OO o c* r^men 
 
 pi c* TJ- cJ c5 mo O co ci r^o co o M M en rj- en 
 
 Mnqdinc; 
 
 co o xnco o O 
 
 o vncnoo t^cnO r^o^M M o-1 
 
 ^iH ^J-MCO OCOOOOCO OCO r->- to 
 
 Mxn^}-r>.ci MOO OO r^-T^oiooo M 
 NCOCOO OM xr>O OO t~^O M OO 
 
 MCOO odr^iAcnd 6 OM 
 
 co o O N co vno 
 r^i ooo in o O co 
 
 ^O 
 
 rt-co co co o co 
 
 O M r^ o O Tf t^ i^* t^ co O w"> t^ 1 co O r^ ^co r^ en M o ^ ^ M M 
 mooo inininininmOO ininininininmininminOOOO 
 
 
COAL. 
 
 227 
 
 OOONvOO^^- c^oo rf Tt 
 coo N -^-i-ixnw MVO >H ^N 
 d O^ co Oco O O 
 
 COMCOWC4COW 
 
 \r> TfCO u-> 
 
 OOOOOu->OOOO 
 ON v? r9 <P M r^ 00 M 
 
 ~ O CO W W 
 
 O 
 
 coo 
 
 t^ r^ t^ t^ 
 
 qsy 
 
 Ow^O 
 
 M M O 
 
 CO M XDOO M 
 
 OOOOOCO 
 O O 00 rj- O O 
 
 coco O rj-r>w 
 
 ua.So.niN 
 
 N COO C> CO COCO C>t^CO M COW 
 
 r^. r^-cd 6 w o r^-o ca ci 06 co M 
 
 OCO IDCOOOO M r> 
 
 O O M M r> M <>cd 6 
 N N N rt W w M 
 
 C> 1-1 
 o^o^ 
 
 
 
 cJ^2< ? 
 
 c c ic 13 s a? a,2 
 
 ^ U fe fl > 1/3 1; 
 
228 
 
 TABLES. 
 
 , 
 
 1 
 1 
 
 "8 
 
 
 
 
 O-------- 
 
 
 8* & 
 
 2 5 *1 
 
 ON ^vO d O O w ^* ^ 
 
 100 co 
 
 O\ M HH 
 
 N CO ^ 
 
 G to W 
 
 
 
 al 1 
 
 3 3 
 
 ir> O O *^>^O O^vO in oo 
 
 * O M 
 N COCO 
 
 
 vO (^O Ooocoomin 
 
 O N <3- 
 
 *t n >-> 
 
 
 coco wo co O co c* w 
 
 N CO U"> 
 
 .* 
 
 
 
 *** 
 
 
 
 *U9SO41If>J 
 
 
 
 uaSAxo 
 
 
 
 UaSoJpAfJ 
 
 
 
 1 
 
 V 
 
 
 1 1 
 
 JTINOOOCOIOOO 
 O I>OO ON OOO 
 
 O 
 CO 00 
 
 3 1 
 
 M M N CO CO CO 
 
 S 5* 2 
 
 1 
 
 mco O O O N xr> O O 
 
 SM^ 
 
 K 
 
 OOO co co O OO O O 
 
 00 O CO 
 
 O t^co 
 
 
 ......... 
 
 
 G 
 
 [lilN N 
 
 ; i 
 
 Name or Loc 
 
 ^i" rt 3 
 
 >S>Ut>H^c/2^ 
 
 2 ^ 
 
 5 -S 
 
 ? & 
 
 co o o r- co 
 moo N o O 
 O O COO CO 
 
 _ 
 
 H M CO O CO l-l 
 
 8O r^ O 
 co r. o 
 
 ^88^8 
 
 \o ci vo o cJ> 
 
 CO CM 
 
COAL. 
 
 229 
 
 
 
 Q 
 -d 
 
 *sL ~ - > rt - 
 
 ^ : - ^ 
 <u 
 
 '5? 
 
 ^ 
 
 1 
 
 sr 5 3 
 
 
 g ^ 
 
 < c/5 
 
 V 
 
 < 
 
 3 
 
 g 
 
 11 s 
 
 Tt in O CT Tf o oo m 
 
 Tt Tf CO O M O Tf M 
 
 M woooo r^-r^in 
 
 co co co Tt rt Ttco O 
 
 ^8^^ 
 
 m co O r^ 
 
 ^- 10 Tt 
 
 M t^ N O 
 
 Tf co m in 
 
 C " 
 
 
 
 
 i! | 
 
 CJ 
 
 r^ r** t^ co oo co Tt* in 
 
 JO O O 
 U") CO *H 
 oo 1^*00 
 
 CO m QN CO 
 CO M O O 
 
 00 O O t- 
 t^ t>CO CO 
 
 qsy 
 
 
 
 in t- N O 
 O r> TJ- in 
 
 ** 
 
 
 
 Tt m r>. co 
 TJ- in M 6 
 
 , nqd ,n S 
 
 ' 
 
 
 co r^co to 
 
 dodo 
 
 
 O * rto O O co m 
 
 QN O Tt O^ f"** O Tt OO 
 
 g" ^1 
 
 
 U3SOJ5IN 
 
 
 _ 2 o. 
 
 M d Tt in 
 
 
 M M in *tO N in O 
 
 COTtOOOOOMCO 
 
 i 
 
 in Ttoo M 
 
 .U3 XQ 
 
 "2 1 ?M 2 ^COCO 
 
 o 
 
 
 
 
 M J 
 
 
 
 COM^-M o^gO 
 
 co m O O 
 
 a 5*85 
 
 
 rt m in in in ^ Tt m 
 
 M Tt in Tt 
 
 in in m Tt 
 
 3 
 
 f^- N O O COCO Ol CT> 
 
 O m t^ co 
 
 M oo N in 
 in t^> N t^- 
 
 
 
 H 
 
 oooocowcoOOci 
 t^ f^ I^.CO 00 O>O O 
 
 O w W CO 
 
 M in o^O 
 
 r^o O co 
 
 1 1 
 U > 
 
 
 O m M 
 i^. r^ co 
 
 M 
 
 co m r^ m 
 IH in M co 
 
 Tt Tt cT ^ 
 
 I 
 
 
 Tt M CO 
 
 OCO O 
 
 
 
 
 
 
 a 
 .2 
 9 
 
 : || : 
 
 
 c 
 
 1 
 
 S -Q ' 
 
 
 
 Name or I 
 
 r l3 _Q _ rj rl C .! 
 
 Illllll 5 
 
 Groucheski .... 
 Miouki 
 Galoubosski 
 Rutschenkvo. . . 
 
 Magatoch, Saght 
 
 
 Nagassi, *' 
 Sutschan, " 
 Saghalien 
 
230 
 
 TABLES. 
 
 IS 
 
 ts o 
 ible. 
 
 H 
 C 
 
 qsy 
 
 SOOcoMCOOOtOcoc^OOO^tO^M 
 OONMNMN'^IHr^NO^NMMtOM 
 
 o r^ a o o ooo ci 
 
 MMMW MMMMMW 
 
 oo M co M M 
 
 rj-NWMt 
 O ^t C>O M 
 
 i-iOOvO\OMr}- 
 
 t>- O 
 
 6666 
 
 \r> \r>\O "^ 
 
 > " 
 
 13 
 S 
 
 8, 
 
 i" 
 
 1 
 
 . 
 
 1 
 
 
 O S 
 
LIGNITES. 
 
 231 
 
 g < 
 
 H u 
 
 2 
 
 S a 
 
 qsy 
 
 3 : cfl; 
 
 W 
 W 
 
 y 
 03c/5c/7 
 
 *i 
 
 -^ cJi 3 
 
 c/jPu << CQ 
 
 . 
 
 O f"J H W Q 1 * O*OO <* W M 
 
 m 10 O i 
 
 oo i 
 
 M f<l t^ CO t^* -^- 
 
 t^. cnvo ON *** N ts c>oo -^ Ix 
 M O (^ "^>O N fO N P) IOOO 
 
 c*> -4-00 10 ' co <*> cJ H ci 4> 
 
 ^vo t~ t^ r^oo M vo 
 
 M o 
 
 lOO IOWJU1O O W lO^-l 
 <J-u->l^'*-ONlOWVO fO CO 
 
 
 
 .,>-<>o<.. 
 
 Vvo o v5 tn ? o-^* o>\o OVCNMOOOO 
 
 \O vo vo txvo t^ t^vo c^vo t^vo vo lOvo 10 
 
 m o 10 in N rnoo o M 
 
 HNMMCSC4(MC4C4 
 
 w oo to rf. , . , , - ,, 
 
 t*. ttvo oo ?. S ex ft tN\o ts S. ^ ? In vo vo 
 
 - 4- 
 
 i- ^ 1 'III s * ;li 
 
 < I s a^ lii 
 
 '5 rf- i 
 
232 
 
 FUEL TABLES. 
 
 O 
 JB 
 
 3 
 
 
 4) 
 
 ^Q JU 
 
 '^ ^ 
 
 Berthelot and Petit. 
 
 
 
 r 
 
 ^ 
 
 
 
 
 a-x- a 
 
 CO O^ 
 
 vn oo 
 
 t^ vn co Qv O vn 
 
 *" O* vO O t7> O 
 
 CN m vo 
 
 f5- O 
 co O 
 
 M HI 
 
 vB 
 
 
 CO 
 
 S3UOIB3 
 
 O CO 
 
 IN O 
 CO Tf 
 
 vn t^ ^" co Qv co 
 
 M -^ r^ co co O 
 
 T^- vn co vn vn vn 
 
 O vo co 
 
 Qv vO* 0^ 
 vn rf vn 
 
 8 
 
 vn 
 
 2 
 
 33103 
 
 8 3- 
 
 00 * 
 N CO 
 
 IN 
 ^ O t^ 
 
 !> CO M 
 IN CO tO 
 
 
 
 
 *M 
 
 n 
 
 vd 
 
 C< 
 
 ^- *t vN 
 
 O CO M 
 
 IN 
 
 vd 
 
 
 
 qsy 
 
 IN 
 
 g e^ co 
 
 
 IN fi O 
 
 
 
 d 
 
 8 
 
 
 unqding 
 PUB uaJJXxQ 
 
 co a* 
 
 cT 6 
 
 CN CO 
 
 Tj- "fr CO IN CO CO 
 
 co co vn vo IN co 
 
 co vo vd vd 4 vd 
 
 tN CO IN CO CO CO 
 
 CO 
 
 CO 
 
 8 
 
 
 uaSojp^H 
 
 OO CO 
 
 00 CO 
 
 co vn 
 
 vn co ^ IN m o> 
 4 vn TJ- vd in in 
 
 in 
 in 
 
 8 
 
 
 uoqjir) 
 
 ^ J? 
 
 O^ CO 
 CO O 
 
 O W CO M M IN 
 
 4 c <> co i^. 
 
 
 
 M 
 CO 
 
 vn 
 
 8 
 
 vn 
 
 
 
 * W I 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 : 
 
 
 . 
 
 
 I 
 
 
 
 If : 
 
 
 . 
 
 
 
 .si "" 
 
 1 
 
 & Ir | j 
 
 
 
 
 
 
 Ismaning, Boh 
 < 
 
 - - - - 13 | 
 
 g S a 
 
 | ^ J3 
 
 ^ M M 
 
 iii 
 
 "8 M | 
 
 S I 1 
 
 C 
 
 1 
 
WOOD. 
 
 233 
 
 CO vO CO O 
 
 ti-H in ON 
 
 CO HI O 
 
 co ON co 
 
 8Tf vO 
 CO CO 
 
 i-i ^- M co mO moo 
 
 co co co 
 
 CO vO O CO CO 
 
 Tt rf vO CO CJ 
 
 O 
 
 in 
 
 rj- m r~^ 
 in in \o 
 
 8 8 
 
 qsy 
 
 m in d in N co co co r- 
 
 666666666 
 
 u3.8o.niN 
 
 I s ** ON O ^O m 0^ ^ 
 
 O O i-t O O O O 
 
 d d d 6 d d d 
 
 M t* t^ in s O co co ^ 
 
 O* *H *O w co co O !"** to r^ 
 
 co-^-'^-'^-cococodNd co 
 
 r^MvOONNOcoco 
 
 WMOWO'ONmrj- o 
 
 vO *O vO ^ m \O vO m in *n 
 
 wOcococoMCOcoin M 
 
 rt'^-'^-Tj-inininTfrf 4 
 
 : : '. :::::::* f 
 
 : : : * : I : : : I 5 : ^ 
 
 ' * ' O % 3 T3 ' -g 
 
 : : : ^ ' ' ^ ? 
 
 : - : i g ^3 H 2\ . II 
 :::;e:||^:*| V1 ^^ 
 
 :^::.:g^^^ ^ 
 
 5 1 1 5 ^ i j I i I a s 1 ; 5 s s 
 
 <eqWfeO^^OPHH w 
 
234 
 
 fUEL TABLES. 
 
 Heat Un 
 Combus 
 
 8 
 
 O 
 
 i 
 
 " 
 
 l" 8. 
 
 = 
 
 ..i- s 
 
 3 3- .2 
 
 r^M o Q^O O O o vn co PI ^-r^o^ 
 
 M'l^TtO M 'I'N cnMOQ MvO TfrvOC 
 Tj-rJ-^-fON WVOT^- COOO N '^^CO 
 
 r cn ^t 
 
 O^ w CO 
 ooOO 
 r>ooco 
 
 OO 
 
 MQO MWOOt^N 
 
 co )-i coco c<-> O O 
 O ON t^ M r** ^ 
 
 d d d d o" d d 
 
 W> W CO CO 
 
 d M d d 
 
 CO CO 
 
 r^ o M 
 
 d M d 
 
 d d 
 
 OcoM 
 - M O M 
 
 O M ino COO 
 
 \nMO COO 
 
 cococococococo r^ r^co cocococococooo 
 
 
 
 
OVEN COKES. 
 
 235 
 
 Heat Un 
 Combus 
 
 qsy 
 
 two 
 
 S: = = 
 
 gs 
 
 OO QO 
 
 xri w r^^-o>-< xnxnf^OO O ^ ^t" 
 r^c< xnr^O O^f^O xnvo O^oo xn co 
 
 M OO 
 
 N CO 
 
 66 
 
 M 
 
 t^OOxnO MxnQoo O^ 
 
 6666666666 
 
 - M HI 
 
 66666 
 
 MO 6 M 6 6 6 6 66 
 
 -J 
 
 H 
 
 ml 
 
 Ia l8 
 
 1 
 
 SQ So 
 
 *J 
 
 go 
 
 a* 
 
236 
 
 FUEL TABLES. 
 
 8 
 
 H 
 
 o 
 
 Authority. 
 
 13 
 
 
 
 
 
 
 
 3 
 
 
 
 
 
 
 s ^' 
 
 ceja H 
 
 M 
 
 CO 
 tn 
 
 CO 
 
 M 
 
 1 
 
 vO 
 
 1 
 
 1 3 1 1 
 
 'SS 
 
 
 
 
 
 
 
 ^^ 2 
 
 i 
 
 ffio 
 
 U 
 
 
 
 M 
 CO 
 
 CO 
 
 o 
 
 1 
 
 M 
 CO 
 
 M C* O O* 
 
 o o o o 
 
 CO CO CO CO 
 
 qsy 
 
 ? 
 
 CO 
 
 CO 
 
 CO 
 CO 
 
 M 
 
 o' 
 
 o 
 
 tn 
 
 CO 
 
 \O *-* Q\ O 
 
 O vO O tn 
 
 -M 
 
 
 
 CO 
 
 d 
 
 d 
 
 d 
 
 M I^ Tj" \O 
 
 w co tn co 
 
 d d d d 
 
 ^,n S 
 
 tn 
 
 vO 
 
 d 
 
 M 
 CO 
 
 d 
 
 CO 
 
 CO 
 
 8 
 
 M 
 
 co 
 
 d 
 
 ^- M M 
 
 d M d 
 
 uaSojjix 
 
 00 
 
 o 
 
 
 
 
 
 uaSXxQ 
 
 a 
 
 d 
 
 o 
 
 \r> 
 
 M 
 
 CO 
 
 CO 
 
 CO 
 
 
 ,, 30JP X H 
 
 d 
 
 CO 
 10 
 
 R 
 
 ! 
 
 o 
 
 
 3 
 
 \rt 
 
 
 
 04 
 
 -. 
 
 $ 
 
 tn co vC co 
 tn oo tn rj- 
 
 c, 
 
 H 
 
 8 
 
 oT 
 
 CO 
 
 CO 
 
 CO 
 CO 
 
 W M M CO 
 
 C *i 
 
 j I 
 
 
 
 
 
 
 
 | 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 Name or Location 
 
 Q 
 
 * 
 o 
 
 W 
 
 Average, Durham 
 
 I 
 
 1 
 
 (U 
 
 I 
 
 Brock well, Durham. . . 
 
 Whiteworth 
 South Braucepeth 
 
GAS COKES. 
 
 237 
 
 C/3 
 
 O 
 
 u 
 
 C/3 
 <J 
 
 O 
 
 G'Z 
 
 &s 
 
 si 
 
 qsy 
 
 pus 
 
 r^ N co a-o rt-vc M 
 
 ION H CO O 1^ W ""> 
 
 M o Ooo OOMi-i 
 
 Tj-TfcocoTj-^-^rTt-T3-'<;fr'T}-^' "^ rf 
 
 M O O O M 
 
 O^COCOOO M O 
 
 |_| Q\ M m CO O^O W 
 
 OO 
 
 N O^ 
 
 ONOO O oo r^vo o oo co M o 
 o5 co 'i- rf- co co ci pi cJ CON 
 
 oo OO 
 
 co co O 
 
 d d d 
 
 OO CO CO CO O>CO 
 
 i-i mO i^ 
 
 O>CO CT>CO 
 
 s .2-i<! ..S o| 
 
 1l-8 |J5 isu 
 8 ^4 d \r5 - 33 
 
 o|l SS^'a-s'S^. 
 
 r 
 
 5^ 
 
 
 
 leumcok 
 mian co 
 
238 
 
 TABLES. 
 
 >ILS 
 ERI 
 
 c> M 
 t^ &< 
 
 cno r^oOTfr^M cno to 
 coco r~ vooo NO ^VONI^ 
 Oco cooOwOOOOO 
 
 coo w co O^O r** o co O 
 M f* o^o co r^ s O O OO IH o\co co r^ rf ^j-oo o co ^- m TJ-O m r^ o 
 
 OOO^OOO^OWMMOOOOOOOOOt-'MMMMOMMOl 
 
 -too 
 
 C 
 
 66666 
 
 O co O 
 
 CO N O 
 
 co O O 
 
 666 
 
 t^OOoo 
 "^ ^-^ tf > 
 
 ooooooo 
 
 
 
 
 
 ...>,.. 
 
 ; * J j. * 1; ; ; ; 
 
 us *>->, 
 
 1^- S ^ S 5 ^rg :^ rc g 
 
 
 | 
 
 
 S -i'S 
 
 . 
 
 
0/Z.S'. 
 
 239 
 
 I- 1 
 
 < O 
 
 M r^ cooo MMM 
 PI ^01^0 ^txD 
 oo t^cooocxDoo CT> 
 
 mOcoOOOcQM 
 ^t M w rj-vO O O >-i 
 M tno -^-M N MO 
 
 Mtnm WOOOOOO 
 co Oco t^ m o O O O ** 
 
 00 V 
 
 T^OO o co M o O^O w> r^ O O co O O w ^ o co f*** o^ 
 
 OOOOCOCOOOCOCOCOCOOOCOCOOOCOCOOOOO 0000 00 00 
 
 O N W M M 10 rt-CO ^-O CO >n TfOO 00 00 OO 
 
 CO M OO r^-CO COM OOlOM 00 OOCOCOWN 
 
 odd odd o'd odd d ddddd 
 
 0) 
 
 I '. .S 
 ' ' : P^ 
 
 . 
 
 
 
 . 
 
 
 
240 
 
 TABLES. 
 
 
 
 jy JH 
 
 
 
 
 '> '> '> G 
 
 
 
 1 
 
 <u <u o 
 O Q Q & 
 <u D <u g C 
 
 
 
 ^ 
 
 G/|q" "|q"S|= = = 
 
 5 1 
 
 
 
 <35 S 
 
 o 
 
 
 h 
 
 oOMCOt-^NOOmON Ttco CT> n O>co 
 d O^O co in t^ co O O M M O f"** O O^ O 
 
 co O 
 r^oo 
 
 
 OQ 
 
 
 
 
 1 
 
 s 
 
 O O M Tt COO P O COCO tH COCO CO M O 1 
 
 ^- mco m N co M MO rj-co co M r^ ^-co 
 O s co O O CO O s M o O O^ co *^ ^1" ^" 
 O^ O^ O O^oo ^ O^co M O Oco CT*O^C>CT 
 
 M ' 
 
 
 
 
 
 
 
 U 
 
 
 
 
 3 
 J3 
 
 < 
 
 
 
 "3 
 Cfl 
 
 6 
 
 
 
 } 
 
 
 
 | 
 
 i 
 
 1 
 
 ? 
 
 
 rn C 
 
 
 
 
 
 H I 
 
 jg. 
 
 
 
 o 
 
 f 
 
 N O Tt ^t M r> 
 co co T}- c5 d 4 
 
 
 HH 
 
 O 
 
 M 
 
 
 U 
 
 
 
 
 H 
 
 c 
 
 
 
 O 
 
 jj 
 
 in co co O ** m in 
 
 
 
 a 
 
 M M M t^Tj- 
 
 
 
 33 
 
 
 
 
 d 
 
 ^ 
 
 
 
 I 
 
 co ^ r^ O co o 
 O O^ co cJ in 4 co 
 
 
 
 i 
 
 CO t>CO CO CO CO CO 
 
 
 
 w.* 
 
 * 
 
 
 
 O 
 
 M ^" ' . 
 
 
 
 * 
 
 O M 
 
 
 
 
 ii M i 
 
 
 
 
 
 g ''S : ? ^-A 
 
 ' 
 
 
 Name or Locat 
 
 .^ !< co 'a | 'i s ^? ^ , 
 
 ** rrt 4> _- rt *^ L* > *-*'r7H C/) , -N ^ 
 
 ^^ a S^^ o^^i o g - ^^ 
 
 i s i^ijiip ii 
 
 : 
 
 
 
 j j|||l||ll||r || 
 
 = 1 
 
 | 
 
 
 c 
 
 
 S c? 
 o s >^ 
 
 ; 
 
 
 
 00 
 
 cj 
 
 1- w O 
 
 CO CO M 
 
 C/^ co 
 in in 
 
 H 
 
 M -j- O 
 
 HI 
 
 1 
 .9 
 
 co ^- O 
 
 
 
 xn co 
 
 U 
 
 CO O^CO 
 
 
 s 
 
 f 7 ,S 
 
 N CO 
 
 
 3 
 
 ja 
 
 8 
 
 
 _a 
 
 CO 
 
 
 "3 
 
 
 
 t/3 
 
 
 
 C 
 g 
 
 
 
 
 
 
 d 
 
 
 g 
 
 CO 
 
 
 a 
 
 6 m M 
 
 
 bfi 
 
 CO r* 
 
 
 X 
 
 TJ-0* 
 
 
 O 
 
 M 
 
 
 c 
 
 k 
 
 g^o 
 
 
 a 
 
 co O O 1 * 
 
 
 X 
 
 
 
 1 
 
 co r^o 
 
 O M (T) 
 
 
 o 
 
 |A cnO 
 
 
 ^ 
 
 r^oo I*** 
 
 
 rd 
 
 5 
 
 
 "o 
 
 ci 
 
 
 "S 
 
 eg 
 
 
 X 
 
 of 
 
 
 
 
 bio 
 
 
 
 - 
 
 g 
 
 s 
 
 o : 
 
 o 
 
 C 
 
 ** 
 
 
 
 3 oj 
 
 U 
 
 h4 
 
 ^C/2 
 
 T3 
 
 O 
 
 qj aT^ 
 
 C p2i 
 
 i 
 
 3 ^ g 
 
 b/}g 
 
 1 
 
 *^ t/3 Q 
 
 25 ^ 
 
 z 
 
 C "^ *^ 
 
 
 
 lil 
 
 
 
 .- O to 
 
 
 
 PQ CQ < 
 
 
GASES. 
 
 H 
 
 .sg 
 
 - 
 
 S3 # S W W 
 
 fe co c/j 
 
 > 
 
 ( < 
 
 jooj 
 
 <t M oo r^ O O co OO O coo TJ- M M M N co o co O OO Ooo O 
 Oco M r^ "3" O to to oo to d o co r^ oo coo O d to cs co to to r^ i*^* 
 
 tooo O to O O tr> M 
 
 MMC4M W C1 i-H C4 
 
 6666 6666 
 
 dOWCOrJ- MMMWO N M t-O COCO W 
 
 M MM 
 
 6666 Modddd d ' OOMOM 
 
 ddo'd d ddddS M dd2 MCO 
 
 >O t"** O to O M o to O co "^ oo ^" o to oo QJ O O co O ^" 
 
 W C*< C^ M O M d CJ M d CO M O O CO to CJ OO O to OO ^~ 
 
 ddddo ddddcoMco dddH dcocoddo' 
 
 M 4-1 
 
 O O co y o a toco o coco M M 
 
 * TO Cy* -J"* 
 
 i^ ij M co 
 
 OOOO OOO co O O to ^ O O ^ 
 
 co^J-coe^ r>-o ci w COM cotooo f^O Oto^oo ci r^w' M" tod 
 
 M a M 01 
 
 a; oJ 
 O G 
 
242 
 
 FUEL TABLES. 
 
 H 
 
 Authority. 
 
 if:;;; l| 
 
 <L> CJra'U CS^PJ^ 
 
 E" 1 OPnE" 1 P^SoS 
 
 500^1 oiqnf) 
 
 O CM ,O in \r> co OO 
 
 t^ CO ONCO ON CM O ON 
 ONCO ON ON ON ONCO 00 
 
 Ooo 0^00 coco r-^. ir> xo o O O CM 
 
 M M 
 
 "aSSSk 
 
 M r~>. co CM coo M or 
 
 co O 0^ ^ x*"* co CM o O O r^*- o co Tj~ o* 
 
 w 
 
 8O 
 "? 
 
 8 OOO u~>oOOxn 
 OOxo coOOOM 
 
 M O^CO O CO COO CM CO 
 M Tj- CM CM CO CO 
 
 
 O O O O O O 
 M ON f^ rj- O* CM 
 
 OO QOOCMOOOcoOOO 
 ONCO OxovncoOOOocoxrico 
 
 I 
 
 M M rt- 
 CM MM 
 
 M I-H M CM <* M O 
 
 o 
 
 O 
 
 do d 
 
 80 O O 
 com 
 
 CO M M vn 
 
 M 
 
 
 c^^Rgs^ 2 
 
 Rco OOO 
 O O xr> co 
 
 ppyo.uoqjto 
 
 M M CM 
 
 M rf ^0 O O 
 
 " 
 
 
 
 
 oopooooc 
 
 tR888 8 &8 88 M S & 
 
 UBqiajM 
 
 5>E&&8 
 
 ) C*^ O** O^ 1 n to 1^* C^ O O O -t^ O CO Tf 1 QN 
 ^ t^ oo s co co co ^C IT) u~) to O^ 1 O* M 
 
 ,^p,H 
 
 
 8 
 
 CO 
 
 JO -ds 
 
 CM oo 
 O co 
 
 
 
 ooooo ooo N 
 
 O O ON CM O O l"^ 1 O 
 CM O M CM CO CO Tj-O OO 
 
 
 
 
 
 : : :| : : : 
 
 p'llIlljfUliH 
 
 
 
 _o 
 
 !'.'. o i : : 
 
 : | : : i i 
 
 Name or Loc 
 
 Bensham seam, Wallse 
 
 a < 
 
 Pipe from ' ' 
 Below Bensham, Hebb 
 < < < 
 
 Bensham, " 
 " Jarrow. 
 
 
 . 3 5 cu S <u 
 
 &:::= f| M 
 ** 9 of o^-* 
 
 ^ ^m ^ " " S ^ -a" 
 
COAL GAS. 
 
 243 
 
 O 
 
 8 
 
 s 
 
 -sl 
 
 oo 4JWQOU H 
 
 oo O 
 
 M ^ 
 
 M in N M O 
 
 in<3-w w N 
 
 O^mO^O vno 
 coO^ coo r> co 
 
 M CO N M 00 
 
 ^cd 6 co coo co 
 
 '3 w - '3 . , 
 ^ rt ^ - - - 
 
 ^a^i^i 
 HUH 
 
 M O N in M CO 
 
 r^ in M r^. O co 
 O m t** O I^O 
 
 co ^ O O co in 
 
 CO COO C^ O O 
 
 o NO co m co 
 
 O mo OOO 
 
 O in r^. M M 
 ^ ino O M r}- 
 O co T}- ej in M 
 
 r^co in q co M co co coo N N in r- 
 co ci o 6 co o' -<f cdr^cdo oo in 
 
 CO ^" CO ^T M CO CO W CO CO CO CO CO CO 
 
 o w co co 
 n co O O O 
 
 M CO CO 6 M 
 
 rt CO rj- CO r}- ^- 
 
 8N m O *<> 
 O M M t> T^- 
 
 ON CO CO CO* 
 CO N Tf CO -^- CO 
 
 O 
 MO 
 
 Ocooor~cod 
 
 O 
 ^- 
 
 X 
 
 c'S 
 
 ^ 
 
 g 
 mbo 
 
 E 
 
 Bry 
 any 
 ng 
 
 Birmingham, 
 Coke ovens, 
 Bonn, Germ 
 Brighton, E 
 Bristol, Eng 
 Chemnitz, G 
 
244 
 
 FUEL TABLES. 
 
 en p 55 S 
 
 jad 
 
 M O "fO M M 
 vr>i-i O^COOO- 
 
 <o o co oo t~*vo 
 
 tnco^rco 
 
 O^ 
 O 
 
 t^vO CO O^l^ 
 
 M o mcoO O r^ 
 
 t^cocooo -t 
 
 i-cO N 
 Tf co M *f t^ M 
 
 co u-> q o q co 
 
 O O O M N r~> OO M co <* Tt o vo oco O co co 
 
 ^ O O xr> M o M w M MNi-iwxnw'^-T^-MN r^ 
 
 M M' 6 6* 66666 6666666666 6 
 
 c* O O M o M t*> ^ O co r* xo M o t^- co -3* o coo ^~ M t^* M oo M 
 xncoo r^TftH xncJ \ncocor>-'^-o" cococoxno ^coin^rj-o' 6 
 
 M 
 
 MQOOOOOOM OcoOOOOMOONOO 
 
 O Q co Q m !> *> coco OM NOcoNOcoONO -^-co O O 
 xo O s ! O O^ M c< vo w o^ Tt~ i^* o ^ xo o w o co c^ *^ O c*i r> o^ w xo 
 
 MM M M M 
 
 JC ? 
 
 vS 
 
 CO CO TT Tf'cO CO CO CO TT Tt - 
 
 O O rfco o r^ o coo *f 
 
 O^t-^WMCONONM 
 
 o" co co &<& o' T}- co 6 o" i~^ O co vn o* 6 co vn 6 coco' o' co coo' M' co 
 xn^J-cocO'^-Tt- 1 ^-'5t'*cO'*-'^-to'3-rtxnxr)'^-xn'3-T^-co^txn'^-cOM 
 
 nJ S'Sv.^rt'rt cW-e'5 3 ^,^ 
 
 O 
 
 - 
 
AIR AND WATER GAS. 
 
 24$ 
 
 -2 
 
 jooj Di 
 
 co o M o w o N 
 en co <o w en <* cn 
 
 coOl^-M O O 
 
 o o o -f a* o 
 cocncnco * \r> 
 
 COM 
 coco 
 
 COC* 
 
 OTj-c\Mr^ O ^f 
 
 Naoo ^rco co HH 
 
 i^co O t^ O OO O O co>o r^O co co oo M w> xn 
 
 U^WCOCOCOU^CIvOCOCOCOClWWClMCO 'T U^ 
 
 >A xnvd O O O O co M 
 
 CO ^ 
 
 M 
 
 d 
 
 O 
 
 OMOr^ 
 
 OOMO 
 
 do 
 
 n \ft to 6 coo N 
 
 CO Tt M Tfr CO CO 
 
 cOvOO 
 WO^O 
 
 MCONNCOC'ICOCOCO CO CO 
 
 w 
 
 mo <^ O O N 
 
 o o M o mo o 
 eJ TJ- cJ 4 d o* o' 
 
 rj-owo 
 MvOOM 
 
 TfCO t^ O CO 
 
 MONO f^ OO^^-^O 
 
 M 9 "^"^T * ^ *? <> r; t l ^MC<COOCH ^ O 
 
 TJ-N do o cod OM-^-ddddM m co 
 
 NOW coco covOcoa^Oui M 
 r)comT^-^-co i ^-u-)Tt-ir>xn rj- 
 
 
 *M 
 
 
 
246 
 
 FUEL TABLES. 
 
 
 Authority. 
 
 Shepard, Bruckner 
 & Schimmel 
 < 
 
 F. B. Wheeler 
 E. E. Taylor, 1885 
 
 |! 
 
 a ^ <G g o ;5 ^ 
 
 n4 PQ ^'j ^W^'J !~ 
 
 Qfe fe fc EW^'jlJJ 
 
 
 
 "a^-a 
 
 O> CO O l~> 
 CO O CO (N 
 
 t^ t^. r>. co 
 
 a t HH-KIH 
 
 co 
 
 
 J3 W orqn3 
 
 CO CO CO N 
 
 O co r^o 
 
 'SSo' 3 ^SgSSKRSS 
 
 R 
 
 
 
 O t~>- O CO 
 
 N O N r O COO N N O O O M 
 
 CO 
 
 
 
 
 (O 
 
 CJ 
 
 o 2 
 . . T 
 
 8 
 
 M 
 
 
 
 
 N CO 
 
 O N CO O 
 
 CO ^ CO O 
 
 N in HH O O^O M ^-co O m O 
 
 CO 
 
 
 ua oaiiM 
 
 m m co N 
 
 ^rtO co COCOM^T ,vnO 
 
 in 
 
 (ft 
 
 3s 
 
 % 
 
 uaSXxQ 
 
 rj- Tt O 
 
 d do 
 
 ^d d'^ddddd " 
 
 CO 
 
 
 o 
 
 N O rj- m 
 
 Mcom N MMO\OoonO^OO 
 
 O 
 
 f-H * 
 
 8 
 
 -3- co r^ < ^- 
 
 N in M O O^oo O O m >H o co ^ 
 
 Tf 
 
 r's 
 
 
 <M ^ 
 
 
 *"" 
 
 ^ 1 
 
 ^ 
 
 N O 
 
 N O m O 
 OOO ^ OMOMOOr^covn 
 
 ^ 
 
 n^ 
 
 u 
 
 N M CO 
 
 CO Tf Tf N COCO in M N M N M 00 
 
 ^ 
 
 |a 
 
 
 OOO 
 
 m m 
 
 in 
 
 ^ & 
 
 
 CO O CO 
 
 ? 2" M"^M ?)fi >C>lM 
 
 in 
 
 h-H 
 < 
 
 sJ 
 
 J 
 
 co O 
 
 N CO 
 
 q 
 
 M 
 
 M 
 
 
 
 
 CO 
 
 CO CO M 
 
 MCO CO NOOCO M O^N 
 
 CO 
 
 
 
 t^ O 
 
 M N M 
 
 N ^ cT^C^^^C^N^ "> 
 
 * 
 
 
 
 in 
 
 O^ O co s 
 
 O O 
 mco^ t^ rJ-coOcor^t^c^inm 
 
 ^ 
 
 
 
 r^ Tt- MO 
 co co co m 
 
 r}-Ntn co co N^vncococo 
 
 * 
 
 
 Name or Location. 
 
 Lowe process, Jersey City, N. J. 
 " " Long Island City, 
 N. Y 
 Lowe process, Long Branch, 
 N. Y 
 Lowe process, Philadelphia, Pa. 
 " " " Ex- 
 
 pTt/3 O,.,^^^ aTfl< ^ 
 
 S^ K^UKSK^ ^jj ^Cv. p^ 
 
 O " ^ O " ' O >2 ^ oj ^ s* 
 
 J fc p^ p< x H^ K 
 
 3 
 
MIXED GAS. 
 
 247 
 
 o 
 
 ti 
 w 
 
 jooj 
 
 J913JM 
 
 oiuoq.no 
 
 ppy oiuoqjB3 
 
 auajAqig 
 
 uaSojpXfi 
 
 ff 
 
 cntoo moooo N c^ 
 O M rf M M T(-vO r}-oO M Ooo 
 
 
 in M 
 
 M O N O 
 
 M COO^M coo u->vnrJ-M 
 
 in in mo O mo O O O O ^ n xno 
 
 rf- O co N CT> co O ^" t^ 
 W W N M rt CS N 04 W 
 
 o ^ O ** moo 
 t^ t^oo O O^O vn 
 
 \neor^Mm i -iMOO^ 
 
 M M M <N 0! IN a 0) C4 
 
 O O N O *3"O O co 
 
 O 
 O 
 
 OOOr^O O O 
 
 n coco O r^ O O 
 
 o q ^t N q^co q m coowco coqcococoqwqq^ 
 " oo d o" 
 
 McS 
 
 - r^ 
 
 a 
 
 Q 
 
248 
 
 FUEL TABLES. 
 
 * 
 
 |r? 2 
 
 
 jooj oiqto 
 
 CO M O 
 
 c^NO 
 
 U"> M M M 
 
 pajjaanqdtns 
 
 IT to r 
 vO vO vO 
 
 co O O Tt- O o 
 
 coco coonOncONcooOOC>'<4-tHNOmM TJ-CO co O 
 
 covorco -N coxr>c> 
 
 WNNCICOCOWCONN 
 
 u 
 
 sjtreuiranm 
 
 
 
 ^3 
 PH 
 
 O 
 
INDEX. 
 
 AGITATOR, BERTHELOT'S, 27 
 Aguitton's exp'ments on coal gas, 95 
 Air, analysis (table), 207 
 
 necessary for combustion, 125; 
 
 (table), 206 
 necessary for combustion 
 
 (table), 201, 202 
 used in combustion, 139 
 Alexejew's calorimeter, 28 
 American Society of Mechanical 
 Engineers, boiler-test re- 
 port, 177 
 
 Analysis, Cinders, 115 
 , Coal, 113 
 
 , should show what, 114 
 , Coke, 82 
 , Gases, 133 
 , Lignite, 78 
 , Manchester gas, 93 
 , Peat, 80 
 , Proximate, 77 
 , Waste gases (table), 134, 135 
 , Wood, 84 
 
 Andrews' calorimeter, 47 
 Anemometer, Fan-wheel, 143 
 , Fletcher's, 144 
 
 , Volume of waste gases by, 143 
 Apparatus for steam-boiler testing 
 
 should be correct, 183 
 , Installation of, 13 
 , Hirn's, 145 
 , Orsat-Muencke, 134 
 Aqueous vapor, Heat of, 159 
 Ash, Analysis of, 115 
 , Lignite, 78 
 , Peat, 80 
 
 , Treatment of, 189 
 Aspirator, Oil, 132 
 Atomic calorie, 2 
 Atwater's calorimeter, 71 
 
 BARRUS'S CALORIMETER, 38 
 Berthelot's agitator, 27 
 bomb, 48 
 
 Bituminous schist * 79 
 
 Boghead coal, 79 
 
 Boiler-testing. See Steam-boiler 
 
 Testing 
 
 Bomb. See Calorimeter 
 Briquettes, how made, 51 
 British thermal units, 2 
 
 " to change to 
 
 calories, 3 
 
 Brix's experiments with charcoal, 84 
 Bueb-Dessau's experiments on coal 
 
 gas, 95 
 
 Bunsen's researches on flame, 168 
 Bunte's experiments on coal, 76 
 gas-coke determinations, 9 
 experiments on waste gases, 135 
 Burnat's smoke tests, 155 
 
 CALCULATION; 
 
 Air necessary for combustion, 125 
 
 Air supplied, 139 
 
 Calories of the boiler test, 159 
 
 Calories of carbon, 54 
 
 Carpenter's calorimeter, 34 
 
 Carbon, 54 
 
 Coal, 66 
 
 Coke, 68 
 
 Colza oil, 64 
 
 Favre and Silbermann's calorim- 
 eter, 26 
 
 Flame temperature, 169 
 
 Gases, 67, 94 
 
 Heat units of boiler trial, 159 
 
 Heat units by lead test, 10 
 
 Heat units from chemical com- 
 position, 7 
 
 Junker's calorimeter, 41 
 
 Mahler's calorimeter, 61 
 
 ; abridged, 70 
 
 Regnault and Pfaundler's, 18 
 
 Vapor of carbon, 173 
 
 Volume of waste gases, 143 
 
 Water value of calorimeters, 14, 
 63 
 
 249 
 
250 
 
 INDEX. 
 
 Calculation ; Weight of waste gases, 
 
 141 
 
 Calories, atomic or molecular, 2 
 Kilo-, 3 
 Pound-, 2 
 To change to B. T. U., 3. See 
 
 Heat Units 
 Calorific power, 2 
 
 Ratio of, to fixed carbon, 78 
 Calorimeter, Alexejew, 28 
 Analytical, 74 
 Andrews, 47 
 Atwater, 71 
 Barrus, 38 
 Berthelot, 48 
 
 corrections, 53 
 
 examples, 54 
 
 operation, 53 
 Carpenter's, 31 
 
 calculation, 34 
 Constant pressure, 20 
 Constant volume, 45 
 Constant pressure and volume, 
 
 ratio of, 45 
 Correction for F. and S., 16 
 
 Berthelot. 53 
 
 cooling, 18, 60 
 
 Junker's, 42 
 
 Regnault and Pfaundler's, 18 
 Cost of, 27 
 Dulong, 20 
 
 Evaluation in water. See Calo- 
 rimeter, Water value 
 Favre and Silbermann, 21 
 
 Calculation, 26 
 
 in complete combustion with, 
 
 23, 25 
 
 Fischer, 29 
 Hartley, 40 
 Junker, 40 
 
 calculation, 41 
 
 errors, 42 
 Kroeker, 73 
 Mahler, 57 
 
 and Berthelot compared, 70 
 
 calculation, 61 
 , abridged, 70 
 
 enamel chips off, 58 (foot-note) 
 
 examples, 64 
 
 for gases, 62 
 
 operation, 59 
 Protection for, 13 
 Rumford, 20 
 Schwackhofer, 35 
 
 waste gases, 37 
 Thompson, L., 43 
 Thompson, W., 37 
 
 Calorimeter, Thomsen, 30 
 Throttling, 117 
 Walther-Hempel, 74 
 Water value 
 
 , Berthelot's calorimeter, 14 
 by combustion, 14 
 by mixing, 15 
 
 Favre and Silbermann's cal- 
 orimeter, 14 
 
 Fischer's calorimeter, 30 
 Lord and Haas' calorimeter, 14 
 Mahler's calorimeter, 14, 63 
 Witz, 47 
 Calorimeters, 12 
 Calorimetric endiometer, 47 
 Candle power and heat of combus- 
 tion compared, 96 
 Cannel coal, 79 
 Carbon, calculation of calories, 54 
 
 calories by various authors, 12 
 in cinders, 115 
 " smoke, 154 
 
 " " ; analysis of, 154, 191 
 oxygen necessary for, 125 
 vapor, weight, and calories, 173 
 Carpenter's calorimeter, 31 
 Carbonic acid, Automatic determi- 
 nation of, 147, 148, 150 
 in producer gases. See Gas 
 
 Producer 
 in waste gases, 81, 84, 91, 134, 
 
 137, 155 
 , proper proportion irt waste 
 
 gases, 135 
 Carbonic oxide, Flame temperature 
 
 of, 170 
 
 in producer gas, 99 
 in waste gases, 84, 91, 101, 134, 
 
 137 (table 135), 164 
 Cellulose, calories of, 85 
 Charbon roux, 83 
 Charcoal, peat, 80 
 wood, 83 
 
 ; Brix's tests, 84 
 , half-burnt, 83 
 ; Sauvage's tests, 83 
 ; Scheurer-K.'s results, 84 
 , Waste gases of, 84 
 Cinder, Analysis of, 115 
 Coal, Actual evaporation of, 76 
 , Air necessary, 126 
 , " supplied, 139 
 Analysis, 113; (tables), 209-230 
 
 should show, 114 
 Bunte's experiments, 76 
 Calories of, 66 
 Difference in samples of, 113 
 
INDEX. 
 
 251 
 
 Coal, Gruner's table, 77 
 
 Heat of combustion (table), 198, 
 
 209 
 
 Johnson's tests, 75 
 Moisture in, 112, 114, 188 
 Morin and Tresca's tests, 75 
 Pure, 75 
 
 Ratio of calories and fixed car- 
 bon, 77 
 
 Ratio of hyd'gen and carbon, 78 
 Sampling, 112 
 Size for combustion, 24 
 Uniformity in same bed, 112 
 Weight of, in 
 Coal gas. See Gas, Coal 
 Coke analyses (table), 209 
 Calories of, 68 
 Composition of, 82 
 Heat of combustion (table), 230 
 Kinds of, 81 
 Use of, 82 
 
 Colza oil, Calories of, 64 
 Combustion. Air necessary, 125 
 Air supplied, 139 
 Heat of. See Heat of Combus- 
 tion 
 
 incomplete in F. and S. calorim- 
 eter, 23 
 
 Constant pressure, 20, 45 
 " volume, 45 
 " " relation of, to 
 
 constant pressure, 45 
 Cooling, Newton's law, 60 
 
 Regnault-Pfaundler's law, 18 
 Corrections for Berthelot calorim- 
 eter, 53 
 
 Cooling, 18, 60 
 Junker calorimeter, 42 
 
 DASYMETER, 146 
 
 Differential gauge, Segur's, 145 
 
 Dissociation, effect of, upon tem- 
 perature, 168 
 
 Dulong's calorimeter, 20 
 
 Dulong's formula, 7 
 
 , Agreement of, with test, 9 
 
 , Mahler's limit to, 10 (foot-note) 
 
 heat unit, 21 
 
 ECONOMETER, 148 
 Efficiency of steam-boilers, 191 
 Electric igniter, Heat of, 70 
 Evaluation in water. See Water 
 
 Value 
 Evaporative effect of coal, 76 
 
 , Factor for, 174 
 
 power of fuel, 174 
 
 Evaporative power of charcoal, 84 
 " gas, 93 
 " lignite, 79 
 " peat, 80 
 " wood, 86 
 
 Evaporative power petroleum, 90 
 of natural gas, 107 
 unit, 180 
 
 Examples, Berthelot's cal'meter, 54 
 Carpenter's calorimeter, 34 
 Favre and S. 26 
 
 Mahler's " 64 
 
 FAN-WHEEL ANEMOMETER, 143 
 Favre and S.'s calorimeter, 21 
 Fischer's calorimeter, 29 
 Flame, 168 
 
 Bunsen's researches, 168 
 length, 169 
 
 not due to incandescence, 168 
 not due to solid particles, 168 
 Propagation of, 168 
 temperature, Calculation of, 169 
 
 , Loss due to dissociation, 168 
 acetylene, 170 
 bor-methyl, 168 
 carbon and carbonic oxide, 170 
 hydrogen, 169 
 
 marsh and olefiant gases, 171 
 oils, 172 
 petroleum, 172 
 
 producer and other gases, 171 
 solid fuels, 172 
 table, 200 
 
 Fletcher's anemometer, 144 
 Flue-gas. See Waste Gases 
 Formula, Balling's, 8 
 Burnat's, 143 
 Dulong's, 7 
 German Engineers', 8 
 Hirn's, 146 
 Jacobus's, 143 
 Mahler's, 9 
 Quality of steam, 119 
 Regnault, for vaporization, 4 
 Regnault and Pfaundler's, 18 
 Schwackhofer's, 8 
 Superheated steam, 123 
 Throttling calorimeter, 122 
 Vaporization of water, 4 
 Waste gases, weight, 141, 143 
 Welter's, 10 
 Fuel, Air required for, 125; table, 
 
 206 
 
 Air supplied to, 139 
 Calorific power under steam- 
 boiler, 109 
 
INDEX. 
 
 Fuel, Evaporative power, 174 
 
 Gaseous, 92 
 
 Weight of, in 
 Fuels, i 
 
 , Division of, I 
 
 Tables, 209 
 
 GAS, COAL 
 
 Aguitton's experiments, 95 
 Bueb-Dessau's experiments, 95 
 Heat of combustion (table), 243 
 Mahler's experiments, 96 
 Variation in, 95 
 Gas-composimeter, 150 
 Gas, gasogene ; heat theory, 97 
 Loss of calories, 98 
 Value, 97 
 Varieties, 98 
 Gas-holder, Oil, 132 
 Gas, Natural. See Natural Gas 
 Gas, Producer ; Heat theory of, 99 
 Heat of combustion (table)245,246 
 Mahler's experiments, 101 
 Gas sampler, A. S. M. E., 131 
 
 Scheurer-Kestner's, 128 
 Gas, water. See Water Gas 
 Gaseous fuels, 92 
 
 Heat of combustion of (tables), 245 
 Gases, Analysis, 133 
 as fuel, 92 
 
 Calculation of calories, 67 
 Comparative value, 107 
 Heat of combustion from anal- 
 ysis, 93 
 Heat units, 164; table, 203 
 
 " " example, 165 
 Ignition point (table), 207 
 Weight and volume (table), 200 
 Specific heat (table), 204 
 Gases, waste. See Waste Gases 
 
 Specific heat of (table), 205 
 Gottlieb's wood tests, 86 
 Gruener's coal table, 77 
 
 HARTLEY'S CALORIMETER, 40 
 Heat, balance in boiler trials, 193 
 Loss of, in producer gas, 104 
 of aqueous vapor, 159 
 combination, 94 
 combustible gases, 164 
 combustion, 3 
 
 and candle power, 96 
 ; Calculated vs. det'mined, 9 
 Cause of disagreement, 10 
 Determination of, 3, 4 
 From chem. composition, 7 
 , Litharge or lead test, 10 
 
 Heat, Methods of determining, 7 
 of carbon, 12, 54 
 carbon vapor, 173 
 coal, 66 
 coke, 68 
 colza oil, 64 
 constant pressure, 20 
 constant pressure and vol- 
 ume, 45 
 
 fuels (tables), 209 
 gas, 67 
 
 gases, calculation, 68, 93 
 gases, difference in, 94 
 gases, modified by con- 
 densation, 94 
 gases (table), 203, 241 et 
 
 scq. 
 
 hydrogen, 97 
 marsh gas, 97 
 natural gas, 106; table, 241 
 oils (table), 238 
 olefiant gas, 97 
 petroleum, 90 
 various subst. (table), 198 
 electric igniter, 70 
 hygroscopic water, 162 
 sensible of the temperature, 160 
 soot, 166 
 vaporization of water, 4; table, 
 
 205 
 
 water of combustion, 162 
 Specific ; gases (table), 204 
 waste gases (table), 205 
 water (table), 205 
 Heat units, Dulong's, 21 
 
 from chemical composition, 7 
 lead reduction test, 10 
 Ratio of, to fixed carbon, 77 
 of steam-boiler tests, Cal'tion, 159 
 of steam-boiler tests Distribu- 
 tion, 167 
 Heat value, 2 
 
 of fuels (tables), 209 
 Heating by charcoal, 84 
 coke, 82 
 gas, 92 
 lignite, 78 
 oil, 89, 90 
 peat, 80 
 wood, 84 
 Hirn's waste-gas apparatus, 145 
 
 formula, 146 
 
 Horse-power, Commercial, 180 
 Hydrocarbons, Unconsumed, 25 
 Hydrogen, Calories of, 4 
 in cinders, 115 
 , Oxygen necessary for, 125 
 
INDEX. 
 
 253 
 
 IGNITER, ELECTRIC 
 
 Heat of, 70 
 
 Ignition point of gases (table), 207 
 Incandescence not flame, 168 
 Indiana natural gas analyses, 105 
 Installation of apparatus, 13 
 
 JACOBUS'S FORMULA, 143 
 Johnson's coal tests, 75 
 Junker's calorimeter, 40 
 
 KENT ON WASTE GASES, 141 
 Kent's ratio of hydrogen and carbon 
 
 in coal, 78 
 
 revision of Johnson's tests, 75 
 Kilo-calorie, 3 
 Kroeker calorimeter and correction 
 
 for water, 73 
 
 LEAD OR LITHARGE TEST, 10 
 is unreliable, n 
 
 Lignite, 78 
 
 , Heat of combustion (table), 231 
 
 Lord and Haas on Ohio and Penn- 
 sylvania coal, 9 
 
 Luminosity, 168 
 
 depends on pressure, 169 
 not due to solid particles, 168 
 
 MAHLER'S CALORIMETER, 57 
 determinations of gas, 101 
 experiments on coal gas, 96 
 formula, 9 
 
 Manchester gas, Analysis of, 93 
 
 Mixed gas, 101 
 
 , Calories of (table), 245 
 
 Moisture in coal, 112, 114 
 
 Moisture in steam, 119, 187 
 
 Molecular calorie, 2 
 
 Morin and Tresca on coal, 75 
 
 Morin and Tresca's wood tests, 86 
 
 NAPHTHALIN.CALORIES OF, 4 6 
 Natural gas and analysis of, 105 
 Calories of, 106; (table), 241 
 Value of, 106 
 Variation in, 105 
 Nitrogen, ratio of, to oxygen 
 
 (table), 207 
 
 Nixon's coal ; calories of, deter- 
 mined, 66 
 
 OHIO NATURAL GAS, 105 
 Oil aspirator or gas-holder, 132 
 Oils, Heat of combustion (table), 238 
 Orsat-Muencke'apparatus, 134 
 
 Oven cokes, Heat of combustion 
 
 (table), 234 
 
 Oxygen, Compressed, is dry, 52 
 in cylinders, 59 
 necessary for combustion, 125 
 
 (table), 
 
 2OI, 2O2 
 
 , Ratio of, to nitrogen in air 
 
 (table), 207 
 required to form water with coal, 
 
 140 ; (table), 206 
 To prepare, 24 
 
 PASTILLES, HOW MADE, 51 
 Peat, 80 
 
 ; Calories of (table), 232 
 Petroleum, 88 
 
 at Chicago, Canada, Moscow, 89 
 
 , Calorific power of, 90 
 
 heating tests, 90 
 
 , Calories of (tables), 238 
 
 , Steam used in atomizing, 91 
 Pittsburg natural gas, 105 
 Pneumatic pyrometer, 152 
 Pound-calorie, 2 
 
 Producer gas, 98. See Gas, Producer 
 Products of combustion of 
 
 Alexejew's calorimeter, 28 
 
 charcoal, 84 
 
 Favre and Silbermann's calorim- 
 eter, 26 
 
 oil, 91 
 
 Schwackhofer's calorimeter, 37. 
 
 See Waste Gases. 
 Pyrometer, Pneumatic, 152 
 
 REGNAULT'S FORMULA, 4 
 Regnault and Pfaundler's law, 18 
 Ringelmann's smoke scale, 158 
 Ronchamp coal, Smoke of, 156 
 
 " " Waste gases of, 134 
 Rothkohle, 83 
 Rumford's calorimeter, 20 
 
 SAMPLER, GAS, 128, 131 
 Sampling, Coal, 112 
 Sauvage's exp'ments on charcoal, 83 
 Scheurer-Kestner's experiments on 
 charcoal, 84 
 
 gas sampler, 128 
 
 smoke analysis, 155 
 
 and Meunier-Dollfus on coal, 75 
 Schist, Bituminous, 79 
 Schwackhofer's calorimeter, 35 
 Segur's differential gauge, 145 
 Sensitiveness of thermometers, 6 
 Shale oil, 88 
 
254 
 
 INDEX. 
 
 Smoke, Bunte's observations, 157 
 Burnat's experiments, 155 
 Carbon in, 154 
 Ringelmann's scale, 158 
 Scheurer-Kestner's analysis, 155 
 Tatlock's tests, 155 
 Soda-lime for absorbing moisture, 23 
 Soot, Heat units of, 166 
 Specific heat. See Heat, Specific 
 
 " of water not consid- 
 ered, 3 
 
 Steam, Moisture in, 117, 119, 187 
 , Quality of, 119, 187 
 , Superheated, 123 
 , Temperature of, 116 
 used in atomizing petroleum, 91 
 Steam-boilers, petroleum-fired, 89 
 
 , Lignite-fired, 79 
 Steam-boiler testing 
 
 apparatus to be correct, 183 
 Ashes and residues, 189 
 Analysis of cinders, 115 
 
 " coal, 113 
 
 " " waste gases, 133, 
 190 
 Boiler and chimney to be 
 
 heated. 183 
 
 Calculation of air necessary, 125 
 " " supplied, 139 
 " heat units, 159 
 " waste gases, 136, 
 141, 146 
 
 Carbon in smoke, 154 
 Coal used, 182 
 
 Corrections of apparatus, 183 
 determine what, 109 
 Distribution of Calories, 167 
 
 " heat, 109 
 Duration of test, 115 
 Early tests, 109 
 Efficiency, 191 
 
 Examination of boiler, etc., 182 
 Heat balance, 192 
 Heat tests and coal anal., 190 
 Johnson's tests, 109 
 Keeping records, 186 
 Moisture in steam, 117 
 Need of knowledge of cal- 
 ories in, 109 
 Preliminaries of, 181 
 Quality of steam, 119, 187 
 Report of A. S. M. E. com- 
 mittee, 177 
 Report of trial, 193 
 Sampling the coal, 112 
 Scheurer-Kestner's tests, no 
 Starting and stopping, 184 
 
 Steam-boiler testing, Temperature 
 
 of steam, 116 
 
 Temperature of waste gases, 151 
 Volume of air necessary, 125 
 ' " supplied, 139 
 " waste gases, 127 
 Waste gas samples and an- 
 alysis, 133, 190 
 Water evaporated, 116 
 Weight of fuel, in 
 
 " waste gases, 141 
 What is necesary, no 
 Sulphur, oxygen necessary for, 126 
 
 TABLE ; AIR COMPONENTS, 207 
 
 Air for combustion, 201, 202 
 
 for perfect combustion, 206 
 
 Ash analyses, 115 
 
 Candle power and heat of com- 
 bustion, 96 
 
 Coal (Gruner's), 77 
 
 Coke analyses, 82 
 
 Distribution of calories, 167 
 
 Flame temperatures, 200 
 
 Fuels, 209 
 
 Heat balance, 193 
 
 Heat of combustion, 198 
 
 of fuels, 209 
 " gases, 202 
 " lignites, 231 
 " peat, 232 
 wood, 86, 233 
 
 vapor 
 
 n of water, 205 
 
 Ignition point of gases, 207 
 Natural gas, 105, 106, 241, 242 
 Oxygen for combustion, 201, 202 
 Oxygen to form water, 206 
 Regnaultand Pfaundler's law, 18 
 Ronchamp coal waste gases, 134 
 Smoke analyses, 157 
 Specific heat of gases, 204 
 
 ' waste gases, 205 
 " " water, 205 
 Thermometer reduction, 199 
 Waste gas analyses, 134, 135 
 Water value calculation, 15 
 Weight and volume of gases, 200 
 Wood, 86 
 
 Tatlock's smoke tests, 155 
 
 Temperature, Heat of sensible, 160 
 of waste gases, 151 
 
 Thermal units, 2 
 
 Thermometer, 4 
 
 , Correction, mercury column, 6 
 , Favre and Silbermann's, 6 
 , Metastatic, 6 
 , reduction table, 199 
 
INDEX. 
 
 255 
 
 Thermometer, Sensibility of, 6 
 Thomsen's calorimeter, 30 
 Thompson's, L., calorimeter, 43 
 Thompson's, W.. 37 
 
 Throttling calorimeter, 117 
 
 UNIT OF EVAPORATION, 179 
 Units of heat, 3 
 
 VAPORIZATION OF WATER, 4 
 
 Vaporization of water (table), 205 
 Variation in coal gas, 95 
 
 " natural gas, 105 
 
 WALTHER-HEMPEL 
 Calorimeter, 74 
 Waste gas analysis, 190 
 Waste gases, Automatic apparatus 
 
 for, 147 
 
 , Bunte's results, 135 
 from charcoal, 84 
 " petroleum, 91 
 " Ronchamp coal, 134 
 , Heat of, 160 
 , Hirn's apparatus, 145 
 
 " formula, 146 
 , Schwackhofer's calorimeter, 37 
 
 Waste gases (table), 134, 135 
 , Temperature of, 151 
 Volume of, 127 
 Water evaporated, 116 
 
 , Heat of combination, 162 
 
 , Heat of vaporization of, 4; 
 
 table, 205 
 
 , Hygroscopic, heat of, 162 
 in Lignite, 78 
 in peat, 80 
 
 , Kroeker's correction for, 73 
 , Specific heat (table), 205 
 , Specific heat of, not considered, 3 
 -value of cal'meters, 14, 15, 30, 63 
 Water gas, 101 
 
 , Heat of combustion of (table), 
 
 245 et seq. 
 Theory, 102 
 Loss of heat, 104 
 Weight of carbon vapor, 173 
 fuel, in 
 waste gases, 141 
 Witz calorimeter, 47 
 Wood, Condition for burning, 87 
 Gottlieb's tests, 86 
 Calories (table), 86, 233 
 Hydrate of carbon, 84 
 Morin and Tresca's tests, 86 
 Wood charcoal. See Charcoal Wood. 
 
70 32 4 
 
 UNIVERSITY OF CALIFORNIA LIBRARY 
 
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