THE EFFECT OF OXYGEN AND CARBON DIOXIDE ON THE CARBONIZATION OF COAL BY FLOYD BEATTY HOBART B. S. University of Illinois, 1920 THESIS Submitted in Partial Fulfillment of the Requirements for the Degree of MASTER OF SCIENCE IN CHEMISTRY IN THE GRADUATE SCHOOL , OF THE UNIVERSITY OF ILLINOIS 1921 V2>2.\ UNIVERSITY OF ILLINOIS THE GRADUATE SCHOOL July. 29 , 1 92L I HEREBY RECOMMEND THAT THE THESIS PREPARED UNDER MY SUPERVISION BY Floyd. Bea_tty Hobart.. __ ENTITLED The Effect o f O xyge n a nd C arbon Dioxide on the Carbonization of Coal . BE ACCEPTED AS FULFILLING THIS PART OF THE REQUIREMENTS FOR Recommendation concurred in* Committee on Final Examination* ^Required for doctor’s degree but not for master’s Digitized by the Internet Archive in 2015 https://archive.org/details/effectofoxygencaOOhoba This investiation v/as undertaken at the suggestion of Dr. T. E. Layng. He has given valuable advice, help and instruction on all occasions during the investigation and I am deeply indebted to him, not only for his as- sistance in this particular problem, but also, for the deeper appreciation of research that he has inspired, and I wish to sincerely thank him. I wish, also, to thank Prof. 3. Vi". Parr for the interest he has shown towards this investigation. Table of Contents pages I. Introduction. 1. nature of the Problem 1 2. Historical 1 3. Outline of the Present Investigation.... 8 II. Experimental. 1. Apparatus 9 2. Temperature Control and lie a sure me nt 12 3. Operation of Apparatus 13 4. Determination of Products and Analysis.. 14 5. Types of Coal Used 15 III. Results. 1. The Effect of Carbon Dioxide... 16 2. The Effect of Oxygen 18 IV. Discussion and Conclusions 32 V. Summary 36 VI. Bibliography 37 ' 1 . THE EFFECT CF OXYGEN AND CARBON LIOXILE ON THE CARBONIZATION OF COAL. I. Introduction. 1. Nature of the Problem: This problem is one of a series of closely related problems which are being studied in this laboratory, with a purpose of learning mor6 about the carbonization of coal. Luring previous work it was observed that the gases, obtained from the carboniza- tion of non-coking and poorly coking coals, held large percentages of carbon dioxide. It was thought at the time that this carbon dioxide was responsible, in part at least, for the non-coking of these coals. Accordingly this problem was undertaken as a means of learning whether or not carbon dioxide is responsible for the non-coking of certain coals. After some investigation it was learned that it would be advantageous to study along with the ef- fect of carbon dioxide, the effect of oxygen; as it appeared that the carbon dioxide, formed during carbonization, was a result of oxygen present in the coal. 2. Historical: There is nothing in the literature concerning the effect of carbon dioxide on the coking constituents of coal. Anderson and 1 Roberts, during tests on a large number of coals to determine the cause of coking in some of them and not in others, "heated these coals (from the Clyde Basin) to a temperature of 500° C. for three hours in an atmosphere of dry carbon dioxide, instead of gaining ' 2 . in weight as they did when heated in air to between 100“’ and 150' C., they lost in weight. The non-coking coals lost the most and the coking coals the least, that is to say, the humus bodies were even at this temperature beginning to decompose. The same experiment showed that after this treatment the percentage of coke was in- creased (probably fixed carbon is meant, as only three of the coals coked), and that in the feebly-coking coals the power of coking was entirely destroyed, but only impaired in the true coking coals! The authors conclude, n that in all the coals resinoid bodies ex- ist, which can be saponified by caustic potash, and which alone are accountable for the coking of semi-coking coals. In addition to these, in the true coking coals there is a constituent not so easily, if at all, acted on by alkalies, oxidisable in air, but not volatile at 300° C." They find also "that the true coking coals melt in an atmosphere of carbon dioxide at 317 C.", and this they take to be the melting point of the constituent referred to. It is evident that Anderson and Roberts saw nothing in the behavior of coals, when in an atmosphere of carbon dioxide, to cause them to believe that carbon dioxide had a deleterious effect upon their coking constituents. 2 According to Anderson, the first one to investigate the ef- fect of heating coal in air, or in oxygen, was Prof. Richter, who, in 1870, found that coal heated in air absorbed oxygen, and that on further heating the percentage of fixed residue was increased extraordinarily. He also knew that some of the ?as coals resisted the absorption of oxygen for some tine. Anderson investigated the effect of oxygen on Scotch coals with the idea of determining the nature of the coking constituent. He proved the validity of « , ’ 3. Richter's work, and that the effect of oxygen was a destruction of the coking properties, especially in the weakly-coking coals. fhe effect of oxygen, that is in the original combination of the coal and that which has been absorbed by weathering, has pro- bably been noted by every authority who has studied the carboniza- tion of coal since Richter's publication of 1870, and was no doubt noted by some even before this time. The earlier investigation along this line was undertaken with the idea of learning more a- bout spontaneous combustion and v/eathering, and their causes. On- ly recently has the study been carried on to a great extent with the effect on coking as the important object. 3 White claims, that the coking qualities of coal depend upon the presence of certain gelatinous algae, that those coals which contain the greatest quantity of micro-algae shov; hydrogen and oxygen in almost the same proportion as exists in bitumen, that is, they have the highest hydrogen and lowest oxygen content. He therefore concludes that coals high in volatile matter and whose analysis show sufficiently high bituminization will coke by the ordinary, or bee-hive process, and that the degree of bituminiza- tion in these coals is indicated by the relative excess of hydro- gen as compared with the diminished oxygen in dry coal, expressed by the ratio of hydrogen over oxygen(E:0). White examined and compared the results from a large number of American coals, and an examination of his results shows that be- low the highest of the semi-bituminous coals, which are approaching the anthracite stage, those coals with a H:Q ratio, or percentage, of 59 or more, but with one or two exceptions, make coke by the ordinary commercial process. Nearly all of those below 59 and a- * • • Um I 4 bove 55, so far as tested, make a coke, and among those with a ra- tio of between 55 and 50 a large percentage make coke. A few of the coals, tested, with a slightly lower, ratio also make coke, but those cokes made from coals with a H:0 ratio of less than 55 are usually very poor and apt to be dark and brittle. The best cokes are made from coals in which the H:0 ratios are 60 or more. Other factors need to be considered, the most important being the fixed carbon content. White’s results point to the fact that coals of less than 79 per cent, fixed carbon, on the pure coal ba- sis, will give a true index of their coking qualities on applica- tion of the H:0 ratio. In coals of greater than 79 per cent, fixed carbon it is gen- erally possible to produce a coke if the qunatity of carbon in the volatile matter is relatively large. Also, most coals in which the H:0 ratio is high, but which refuse to coke, are distin- guishable by their clearly defined calorific deficiency with re- ference to the carbon : oxygen f ash ratio. White further states that, "the changes of coal on exposure or weathering are indicated in the analysis by reduced H:0 ratios; by reduced available hydro- gen; and in many cases by reduced volatile carbon ratios. Weath- ering can in most cases be detected by the change in the oxygen- hydrogen relations and by the marked calorific deficiencies.” Considerable data relating to the absorption of oxygen by zi coal is available. Anderson; in 1898 found that at temperatures below 160° C. atmospheric oxidation of Scottish coals progressed rapidly during the first 12 to 24 hours, but afterwards fell off considerably. Nevertheless the coal increased slowly in weight for a long time, the period varying for different coals. . ... ' v 5 Bone mentions that, "the Doncaster workers had been puzzled to find that 'in the oxidation of coal at low temperatures oxygen disappears but scarcely any carbon dioxide is formed 1 , but this fact was surely well known before to chemists (S.W.Parr in parti- cular), and need cause no surprise to any one familiar with the phenomena of surface combustion generally." G Bone has experimented on the absorption of oxygen at temper- atures between 45 and 120* 0. on a Durham coking coal and a Barns- ley hard steam coal. He found that at temperatures below 80 Q G. the absorption was in each case rather slow, even under increased pressure. In the nieghborhood of 80^ G. the reaction became de- cidedly quicker and at above 100° C. it was marked by a regular and simultaneous production of the two oxides of carbon, and steam, these evidently resulting from the decomposition of some unstable body, or bodies, primarily formed by the absorption of the oxygen. These tests were made by circulating dry oxygen continuously over the previously dried coal. Bon6 gives quantitative results of the tests made on both coals at 107 to 109° C. which are, in part, as follows; Durham Coking Coal. Temperature 100' 200 * 300 6 400 * 500 0 P absorbed 34.40 57.90 84.00 9 7.40 110.00 COp evolved 4.27 6.94 9.30 11.32 GO evolved 1.92 2.78 3.63 4.27 . • ♦ 6 . Barnsley Hard Stean: Coal. Temperature 100" 200 ' 300 * 400° o 500 Op absorbed 57.50 81.20 96.00 108.30 110.10 COg evolved 7.60 12.00 14.40 15.90 CO evolved 5.90 5.30 5.76 5.76 Note. The volumes of gas are in c.c. per gram of coal. Bone says that , "the whole process is one of 'surface combustion 1 which, the writer's researches have shown, is subject to special conditions which do not apply in homogenous gaseous combustion. It is abundantly evident that the oxygen is first of all ’’absorbed" by the coal substance, possibly in some 'activated' form , then incorporated in some way (it may only be loosely, or, on the other hand, it may be, as S.W.Parr suggested, in some defi- nite form), and as the temperature rises, it finally is expelled in gaseous products (HgO and oxides of carbon). And between its initial absorption and its final expulsion a whole series of com- plex phenomena may be involved, which have hitherto received lit- tle attention." 7 Porter and Ralston have recently done considerable research on the effect of oxygen and air on coal. They used a Pittsburgh, a West Virginia and an Illinois coal and also a Wyoming lignite. They determined the total amount of oxygen absorbed by these coals at various temperatures and pressures and the amount of exothermic heat (roughly) from this absorption. They also passed air over the Illinois and Wyoming coals at different temperatures and de- termined the weight of carbon dioxide, carbon monoxide and water formed and the change in weight of the coal, but did not determine the amount of oxygen that was actually used during the tests. , - 7 . Porter and Ralstons' s conclusions are in part as follows: "The effect of weathering or of perliminary moderate heating on the coking quality of coal is explained as an effect of oxidation whereby the fusible organic constituents of the coal are decomposed or altered. The alteration does not occur in a nonoxidizing at- mosphere. It is known that weathering of coal causes an increase of ”eombined"water ; that is, of water that is not in the normal free stat6 and that has at any given temperature a vapor pressure lower than the normal. This water remains in the coal after "air drying." Its increase by weathering is due to oxidation and to the formation thereby of a complex easily decomposed by heat to form water." Katz® has shown that coal will absorb any gas until an equil- ibrium with that gas is reached, the volume required depending upon the gas used. He concludes from his work that, "In so far as investigated, the absorption of gases by Pittsburgh coal is close- ly analogous to the absorption of gases by charcoal." The study of oxidation or weathering of coal is not a new to- pic. The first investigations were carried on in an attempt to learn something of deterioration and spontaneous combustion of coal and wer6 of little value otherwise. At the present time the same motives favor investigation, the desired result being greater efficiency from the storage and use of coal for power production. The effect of oxygen on the coking qualities of coal has usually been noted, but in many cases given but slight consideration. White seems to have associated the oxygen content of coal with its coking qualities more closely than any one previously, and his H:0 ratio is quite applicable as a means of determining . ' 8 . the coking qualities of most coals. Bone, and Porter, and Ralston, give considerable quantitative data on the absorption of oxygen oy coal, but their results may be slightly erroneous due to partial combustion, since th6y passed a continuous stream of oxygen over heated coal. Bone advances the idea that the oxygen may be held in an "ac- tivated form” whil6 Katz suggests that coal behaves similiarly to charcoal towards gases. Thus both hint at the plausibility of the oxygen being held to the coal mechanically as a molecular conden- sation or in an adsorbed condition. Porter and Ralston explain the effect of oxidation of coal as destroying the coking constituent by altering or decomposing the fusable organic compounds in the coal. 9 Parr and Olin sum up the situation rather well in the fol- lowing: "It has been proved that oxygen absorption goes on rapid- ly when fresh coal is exposed to the atmosphere. It has been shown further that this absorption weakens or destroys altogether any coking properties that the original coal may have. In other words a high H:0 ratio marks the absence of fusibility and cemen- tation. The organic compounds of the coal which furnish the ce- menting material for the cok6 are apparently attacked by oxygen. They yield, on oxidation, humic acids of varying composition which decompose into powdery residues.” Outline of the Present Investigation: The initial portion of the investigation consisted in a study of the effect of carbon dioxide on the coking qualities of various coals. The coal used was either saturated with carbon dioxide and . . . 9 . carbonized, or it was carbonized in a current of carbon dioxide. In either case the carbon dioxide used v/as measured and the total gas evolved, also measured and analyzed, and the gain or loss in carbon dioxide noted. In studying the effect of oxygen on the coking properties, the coal v/as in each case saturated with the oxygen before the carbonization began. This made it necessary to determine the tem- perature best suited for the saturation, and the time necessary for complete saturation. The data from these preliminary oxida- 6 tion tests conforms very well with that of done and fairly well 7 with that of Porter and Ralston. Blank or straight carbonization tests were made on each of the coals and the products determined. These were followed by tests in which the coal v/as previously sat- urated v/ith oxygen and again, the products were determined. The resultant gas was analyzed, in both cases, and the difference in its constituents , due to the added oxygen, noted. II. Experimental. Apparatus : The complete apparatus is shown in Figure 1. For measuring and storing the gas that v/as added to the coal two sets of aspir- ator bottles and a 200 c.c. gas burette v/ere used. These bottles (A & B) were of four and two liter capacity and were always filled to the same level at atmospheric pressure. The burette (G) was used to measure volumes less than the capacity of the smaller bot- tle. The bottles and burette were connected so that either of the three could be filled or emptied as desired, and they were u- sed, not only for measuring the gas passing into the retort, but / . . 10 . also for that evolved by the coal. The wash bottles (D & E) con- tained sulfuric acid for drying the used gas and also to show the rate of flow of the gas as it was being used. The gas passed in- to the bottom of the retort (F), under a slight pressure measured by the manometer (G). The retort used was made of pyrex tubing 50 mm. in diameter and 45 cm. long. At the lower end a 10 mm. tube was sealed on and a second 10 mm. tube or side arm was sealed on at about 10 cm. from the top of the retort. The retort was placed in the furnace (T) in a vertical position with the upper 15 to 20 cm. exposed. The top of the retort was closed with a one hole rubber stopper carrying a pyrex thermocouple tube (P). Heat was held away from the stopper by two aluminum discs (Q) placed on the thermocouple tube. The retort was in reality a modified distilling flask with a side arm long enough to act as a condenser. Over the end of the side arm v/as placed a 50 c. c. distilling flask (H) in which the tar and water were collected. The evolved gas passed out through the side arm of the small distilling flask into a small bulb filled with glass wool, used to remove the tar fog. The man- ometer (G) measured the pressure of the evolved gas. The U tube (K) contained dilute sulfuric acid for th6 removal of ammonia from the gas. Hext in the train was a CaCls tub6 (L) for removing the last traces of water. The gas next passed into a KOE bulb (!I) (used for determining C0 o in organic combustions, but here filled with a weakly acid solution of CdSC> 4 ) w bich re- moved the hydrogen sulfide. Prom here the gas passed directly in- to the 12 liter aspirator bottle (IT) where it was stored until ready to be measured in the previously mentioned bottles (A & B). . * 12 . Temperature Control and Measurement: The furnace used for heating the retort and charge of coal was built in this laboratory. It consisted of a Chromel heating element, h6ld on an Alundum core of about 14 by 4 inches, and in- sulated with Sil-O-Cel. The outside container was an ordinary can of approximately 16 inches in diameter and depth. The heat- ing element was connected in series with an external resistance, by means of which the temperature of the furnace could be held at any desired point up to 800 * C. , or could be brought from room temperature to 600° C. at an uniform rate and in about two hours a. if desired. In all of these tests 600 to 625° C. were the maxi- mum temperatures used. Temperature readings of the furnace and of the center of the charge were taken each 15 minutes. Ordinary thermometers we re used for temperatures up to 250 or 300° C., one being suspended in the furnace between its wall and the retort and the other being hung in the pyrex tube (?) which passed through the stopper and down to the center of the charge of coal. For temperatures above 300°C. two Chromel -Alum© 1 thermocouples (0), made of number 16 wire, were used. These were connected as shown in Figure l,.to a Weston Direct Current Millivoltmeter (3). They were standar- dized against the freezing points of Bureau of Standards Aluminum and Tin. The couples we re exact duplicates and the same curve was used for both. The temperatures could be read from the curve to within two degrees and the couples were accurate to the same de- gree. ITo external resistance was needed. , . , . . . . 13. Operation of Apparatus: The bottom of the pyrex retort was covered with glass wool; 100 grams of coal, usually ground to 60 mesh, wer6 poured in and the stopper and thermocouple tube inserted. The retort and con- tents were weighed and placed in the furnace. The small flask was placed over the side arm and the various connections made. All pieces of the train for collecting the products were weighed before being placed in position. Thus on a second weighing, after the 1 6 st was completed, the weights of the products we re available., In nearly all of the tests using carbon dioxide, the gas was passed continuously through the retort. This was easily accom- plished since it was possible to fill either aspirator bottle while the other was being emptied. In all the tests using oxygen, the coal was saturated before the carbonisation began. The tempera- ture at which the coal was saturated was varied as desired in the different tests. In some cases, after the desired amount of oxy- gen had been added, the retort was swept out with nitrogen before the carbonization began, while in others this was thought unneces- sary and neglected. A number of tests were made in which no gas was added to or passed through the coal. These were termed blank tests and were made in order that the effect of the added gas could be more dis- tinctly noted. The apparatus did not need to be altered for these tests. In order to easily control the flow of gas, both into the re- tort and from it, the auxiliary aspirator bottles (A, B & II) were suspended by means of cords and pulleys (not shown in Figure 1.). In this manner the bottles could be held at any desired height and , . . . . 14 the pressure in the retort easily controled. The time of preliminary treatment of the coal with oxygen or carbon dioxide varied and did not require close attention. The time of carbonization also varied but was usually about three hours . Determination of Products and Analysis: The most important products from the carbonization tests W 6 re the coke residues and the evolved gases. The amount of residue, in the retort, was determined by weighing the coal used and the retort and contents before and after the t 6 st. The coke was then taken from the retort and stored in small glass jars. The gas collected in either or any of the bottles A, B, or K, and was measured by means of the bottles A and B, and the burette G. The volume of gas was in each case corrected to 60° P. and 30 inches of mercury. The evolved gas was analyzed in a Modified Orsat Ap- 10 paratus, designed and built in this laboratory. The constituents were determined as follows: COg by absorption in KOK, Og in al- kaline pyrogallol, GgH A in bromine water, and CgHg in fuming Hp,S0^. Hp and CO were burned in a copper oxide furnace at 300^ G. ; the Hg determined by contraction and the CO by absorption of the resultant CO 2 in KOH.CH 4 and CgHg were burned in oxygen over mer- cury in a glass bulb and the two gases diferentiated according to Earnshaw , s' 1 method. ilg was taken as the difference between the total of the above mentioned constituents and the original volume. The original volume taken was always 100 C.C. and thus the values obtained were in percentage by volume. ■ 15 The water and tar, collected in the flask (H) wer6 v/eighed together, centrifuged, and the volumes determined. Thus the weights of each were obtainable . II o attempt was made to analyze the tar. The apparatus as designed would also permit the determination of the ammonia and hydrogen sulfide formed, but as these had no direct bearing on the problem and since their determination re- quired considerable time, none were made on the ammonia and only a few were made on the hydrogen sulfide. In most of the tests these products were not collected. Probably very little ammonia was formed at the temperatures attained and the amount of hydro- gen sulfide depended upon the coal carbonized. Hydrogen sulfide was observed to be first liberated at 275 to 300° G. In the tests where the hydrogen sulfide was not removed as cadmium sulfide, it remained in the gas and was determined as carbon dioxide. Thus, although the carbon dioxide values for the gases analyzed were high, they were uniformly so and the ultimate results were unef- fected. Types of Coal Used: Two types of coal we re used for these tests, one was an Eas- tern Bituminous Goal of the High Volatile type, from the Consoli- dated Goal Company of Fairmount, West Virginia, and the other type consisted of several coals from the Illinois field. These were from Saline, Perry, Franklin, and Moultrie Counties. The Saline and Perry County coals were mainly used, the former being a good coking and the latter a weakly coking coal. The analysis of these two and the West Virginia coal are as follows: . . . . 16 . Proximate Nest Saline Perry Virginia County County Moisture 1.34 4.27 5.30 Volatile Matter 35.76 35.93 35.91 Fixed Carbon 56.92 53.17 49.85 Ash 5.98 6.63 8.96 Ultimate Carbon 78.43 71.88 68.00 Hydrogen 5.06 4.83 4.94 Oxygen 6.91 8.32 10.00 Nitrogen 1.50 1.03 1.66 Sulfur 0.78 3.04 1.14 Ash 5.98 6.63 8.96 Moisture 1.34 4.27 5.30 III . I\6 Suit S The Effect of Carbon Dioxide: The results from the tests where carbon dioxide was used dur- ing the carboniz ation were all of a negative character. Those given in Table 1 . show that carbon dioxide has apparently no effect on the coking constituents of Illinois or Eastern Bituminous coal. The first tests with carbon dioxide were made on the West Vir- ginia coal and when the results were found to be negative it was decided that the younger coals of Illinois might be more easily effected. Accordingly, tests were next made on a Saline County coal. Here again negative results were obtained. The results of these tests are shown in Table 1. as tests 3, 4 and 5. In these . ' 17 and other tests (data not shown) the conditions were varied so as to attack and destroy th6 coking constituent in the coal. In test number 5 the coal w as held at its decomposition point for four hours and carbon dioxide passed continuously through the retort, but nevertheless, a residue of coke was obtained. In test number 6 the residue was a powder. The coal used in this test, from Franklin County, had been in the laboratory for some time and was in a more or less weathered condition. A second test, number 7, was made on fresh Franklin County coal and a good coke obtained. This proved that the results of test number 6 were due to the weathered condition of the coal and not to the carbon dioxide , In all these tests the carbon dioxide was passed through the retort in a continuous stream during the period of decomposition. It was laser learned that if the coal, in a powdered condition, was heated slightly above 100 C. and evacuated it could be made to "adsorb" gases in a similiar manner as activated charcoal. There- fore test number 23 was made on a weakly coking coal from Perry County, in which the coal was heated to about 180 P C., evacuated, and carbon dioxide admitted. The coal was then allowed to stand in this carbon dioxide atmosphere for several hours to insure com- plete saturation. It was hoped that the "adsorbed" carbon dioxide would be combined sufficiently with the coal to have a deleterious effect upon the coking constituents. However nearly all of this added carbon dioxide was delivered with the gas that came from the coal below 400 *0. and the resultant coke was even better than that obtained from one of the blank tests (Humber 18.) on this sam6 coal . , . . , - 18 All of this data SG6ras to prove, then, that carbon dioxide does not have a deleterious effect upon the coking coals. And the carbon dioxide that is obtained in the gas from coking tests on non-coking coals must b6 a product of decomposition and not in itself responsible for the non-coking of the coal. However this carbon dioxide, coming as it does from the reaction of oxygen with carbon, may be an index of the state of oxidation, or better, the weathered condition of the original coal. And in this ?/ay the study of the effects of the two gases is connected. The Effect of Oxygen: The addition of oxygen continuously during a coking test is not advisable since combustion would take place when a temperature of about 300° C. was reached. Therefore in the study of the ef- fect of oxygen on the carbonization of coal, the coal was satura- ted with the oxygen before the carbonization was attempted. In order to determine at which temperature oxygen would be most readi- ly adsorbed, a series of tests were made on Saline County coal, to determine quantitatively the volume taken at different temperature q, and the time of apparent saturation. Temperatures from 30 to 330*0, were used and it was found that the coal took more oxygen in a short time at a temperature slightly above 100 * C. The results of these tests are shown in Figure II. The method employed was to heat the coal to the desired temperature, evacuate as low as possi- ble, and admit the oxygen from a graduated container. The oxygen did not pass through the retort in which the coal was held but merely replaced the vacuum, more oxygen being free to enter as needed. As has been mentioned. Bone, and Porter, and Ralston, have . o o o o O O Q 1-3 fel p-a P p =3 p tei o o o o C5 05 ff) O p H* << p « p p o O c TT Tf 1 y* CO > • • • 3 i H ^ z z Q o CD Q 3 3 O CO CO • • (0 • • fed CO o pp p hrl CO p 05 P P fcd co CO P -3 CO ^0 <3 l_i tO cn h ro o S3 • • ^ • P • -O O i P cn o p • tri P a CO O ro cn 05 p cn o o O P o iv P -3 O < i — i P CO cn cn o o cn cn cn O o o cn o p ro o to P P p o • • fed o o O CO cn P o p fed o co cn cd co -o cn p 05 o • p bd • 00 • o • ro -a to cn o p p H- O CO ^ cn cn <3 ro 05 cn oc o o o V P -50 p y P fed o o o o o o o o o o o o p O CO 05 O p p < o • U p o X a co p cn i — 1 cn HHM p o p u 05 cn P POOP p P cn o ♦ p w • -3 ♦ cn • CD H O cn o P P H- • on 05 ro cn -3 05 O ro o o o V <2 O p y o o o o o o o o o o o o p to to cn o p p C o • hrj y a p 05 O 3 ro O 05 co 05 cn cd cn ro p •x; • V • P • ib* • ro 05 cn p p M P O - . 6600 Tater 12 " Time o £ Garb oni sa 1 on 3:30 Type of Residue: PowderGd, no evidence \ of softening or cakin'- • Gas Data: Fractions * ' I II III Total c.c. % c.c. % c #c « % c.c. Total Gas 1740 3036 4840 5616 Temperature 426" * m> * 620 s co g 45.2 740 11,3 346 7.1 344 14.8 1430 °2 7.4 129 0.4 12 0.3 15 1.6 156 G g H 4 4.1 71 4.5 134 0,5 24 2,4. 229 ^6% 1.3 23 1.0 30 0.3 15 0.8 68 Hg 2.7 47 13.8 420 33.5 1620 21.7 2087 CO 4.1 71 2.2 67 10.4 540 7.4 670 CH 4 4.7 82 31.4 952 36.6 1757 28.9 2791 CgH 6 20,0 384 24*6 746 6.6 319 14.7 1413 ilg 13.3 230 11.0 334 4.8 232 0.3 756 Remarks : 1666 c.c. added Og not accounted for by analysis = 1.96 gable IV 25 BATA FROi* TS T 3 OS 3A *11? JUIITI goat Ho. 21 Weight Coal 100 gms, !o&‘ .1 Oxyren /Idod Ilono Residue 70 ” Time of addition mum Tar 10 ” Carbon! sat i on Tern. 620' C. Water 10 " fine of Carbonization 3: If hr a. *.f Residue: Coke, hard and dense. Gao Data: Fractions I II III Total * c.c. % c.c. C e 0 . ?-• c.c. Total Gas 1550 3024 6,50 10624 Temperature 425* 5 0* 620 ° CO* 10.0 244 0.6 262 *• 0 .6 399 8.9 955 °2 0.7 11 0.3 9 0 .4 24 0.4 44 c 2 H l 4.2 65 4.0 122 0 .6 36 2.1 283 C r ,H 6 0.4 6 1.0 55 0 .4 24 ir.- co CD e o Hg 6*0 93 14.3 436 iW . *' c> 8 2 U 25.8 2749 C0„ 1.0 16 0.0 24 3.3 199 2.3 239 CH 4 c»h| 17.5 271 42.2 1287 37 .0 2246 35.6 3798 21.1 327 21 • 3 649 8 .2 496 13.8 1472 Hfi 30.1 467 6.7 p ; A 6 *8 418 10.2 183 Remarks : Retort swept with Tip at start . Do iG in retort 568 c.c. * 45 m * * * Teat Ho. 22 Weight Coal 100 * Total OXw iron added 2525 c *3, lie si due 71 " Time of addition 13:00 his Tar 9 " Carbonisation Temp 620* C. ! Water 10 w Time o f Garb ni z a tion 3 i 45 hr a Type of Re si duo: Powdered , no evidence of softening S’ T} O o & o O&s Data: Fractions 1 II III Total i c.c. % c.c. % c.c. c.c. Total Gas 2150 3100 6160 11420 Temperature 500" 680 d 680 " GOg 37.2 800 10.1 313 8.0 493 14.1 1606 °2 11.2 241 0*6 18 0.5 31 2.5 290 c. b h 5.0 107 3.2 99 0.3 18 2*0 224 g 6 H 5 0.4 9 1.9 59 0.5 31 0.9 99 Ho 3.4 73 14.5 450 32,2 8830 84.1 2753 CO ' 9.8 . 10 3.5 108 7. ) 453 6.6 750 C*3$ 13.6 294 44.2 1360 36,6 82255 34.3 3917 13*4 288 18.0 558 6.0 370 10.6 1216 *2 6.0 129 4.0 124 4.9 302 4.9 555 Re? arks: 1330 c.o. of added Og unacc 3 unted for by analysis, * 1.61 ;• table V*. 26, DATA FROM TJS3T0 05 V.T:oT V X :l INIA C fa . Test No. 24 Y. 7 elght Coal 100 gms • Total Oxy ren added Hone Residue 76 ” Time of addition — Tar 15 ” Cart) oni a at ion T ; enp 605 * C. flator 4 " Tine of Carbon! b: vt i on 3 :16 hr a. Type of Residue : Coke, sli jhtly por us, avide noe of swelling* Oao Data: Fractions .. I II . Ill Total fo C.C. % c.c . » < : . <1 c.c. Total Gas 1606 3820 5600 10605 Temperature 415* 496" 6 ° 005° COp 15.8 216 6.1 196 *3.9 218 6.5 680 o* 5*8 56 025 16 1*0 56 1.2 128 %H4 5599 99 6,1 196 0.5 28 3.0 323 C.H. 2.4 40 1.6 51 0.6 34 1.3 125 *4 4.5 76 9.9 318 33.5 1875 25.6 8269 CO 0.6 10 0.0 26 3.9 218 2.4 254 oh* 11.2 189 44.2 1420 46.2 2586 40.0 4195 26.3 4«'k> 21.8 ®02 6.4 3359 14.4 1513 »8 29.5 417 9.0 290 4.0 224 9.7 1011 Remarks : Air in retort at start - 120 c.e. 0£ and 45C > c.c. Ho. * m * #e * * 4f * \ Test Ho, 26 Weight Coal 100 3Q8 . Total Oxygen added 5395 c.c. Residue 72 u Time of addition 100: 0 hrs. Tar 12 " Carbonisation T or ip. 616° C Water 6 M Tiro of Carbonization 3:6 0 hrs. Type of Residue : Powdered, no evidence of softenin of coking. Gas Data : Fractions I II III j* Tot 1 % c.c. c.c • c.c. jtv c.c. Total (las 1730 3140 6260 11030 Temperature 416° 6 >0 d 615 * 615° 43.5 2.1 5.5 1.3 2.3 14.9 10.8 3.? 5.9 4 36 95 22 40 £58 18? 151 9.4 1.0 6.2 1.5 9.1 6.3 45.4 16.1 4*0 286 30 189 46 277 191 1 00 .439 122 5.3 0.3 0.3 0,6 50.0 6.0 44.5 6.6 6,5 332 19 19 38 1880 376 2786 407 407 IS. 2 0.8 2.8 1.0 20*0 7.5 39.6 9.5 5.7 3468 85 303 106 2197 825 4362 1 47 631 Remarks: 1000 c.c. added Op in evolved gas. Undetermined 437603. 27 The volumes of oxygen, carbon dioxide, hydrogen and carbon monoxide are plotted in Figures IV, V and VI against the tempera- tures of fractional collection. Each graph represents the tests on one coal. Thus the differences in the constituents evolved by each coal under different conditions are shown. The oxygen added to the coal is shown to be given off, in part, as carbon dioxide and carbon monoxide, the former predominating at the lower temper- atures and the latter increasing as the temperature rises. This must be due in part to the reduction of carbon dioxide to the mon- oxide at high temperatures, by carbon. The oxygen added does not seem to effect the volume of hydrogen evolved nor does it effect the volume of oxygen, except in the first fraction of gas taken. However it is impossible to account for all of the oxygen added by an analysis of th6 evolved gas. In all probability the oxygen lost is in part retained in the residue, and would at higher tem- peratures b6 evolved as carbon monoxide, and is in part held in the tar. There is also the probability that the water of decompo- sition, from the tests in which oxygen was added, is in greater proportion than in the blank tests but it was impossible to detar - mine this accurately in these tests. However the formation of water of decomposition should decrease the volume of hydrogen in the gas and as the curves do not show this to be true it would seem that the probability, of a greater amount of water of decom- position, is erroneous. Figure III shows a comparison of the adsorption of carbon dioxide, oxygen and nitrogen by Saline County coal at ordinary temperatures. Time is the only variable, since the pressure and temperature remained constant during the test. . , . -S--> . vu/urne m cuo/c Leor/merers Volume in Cubic Centimeters otion temperatures Centimeters i \ Carbpn Carbon Monoxide grams carbonization . W200 2000 - * 35 . vestigation and also from other sources. It is not the intention of the writer to disprove other existing theories on carbonization nor to propose these as proven facts, but as theoretical consi- derations worthy of further study and investigation, and as such it is hoped that they will prove to be of value. 36 • V. Summary. Carbon dioxide adsorbed by coal or passed through the retort during the carboni zation process has no effect upon the coking qualities of coal. A coking coal if saturated with sufficient oxygen will refuse to coke. The H:0 ration is an excellent index of the coking prop erties of a weathered or oxidized coal as well as of a fresh coal. The oxygen adsorbed by coal is delivered during the carbonization, mostly as oxides of carbon. That portion unaccounted for must necessarily remain in the tar and the residue . Finely ground coal possesses an avidity for gases, and especially oxygen, very similiar to that of activated char- coal . Adsorbed oxygen destroys the coking properties of coal by apparently reacting with the phenol soluble portion during the carbonization, and changing it, into compounds of such high melting point that they decompose before this point is reached, or into compounds of indefinite physical properties. Carbon dioxide is a product of the decomposition of the oxiginated phenol extract and the probable carbon-oxygen complex (sub-oxides of carbon or fixed oxygen). . 1 37 Bibliography. 1. Anderson and Roberts, J. S. C. I. (1898) p 1013 (abstracted in Lewes text (1914) P 212) 2. Anderson and Roberts, J. 3. C. I. (1898) p 1005 3. Bureau of Mines Bulletin 29. by David White. (1911) (The Effect of Oxygen in Goal) 4. Y/. A. Bone, text, "Goal and its Scientific Uses" p 152 5. W. A. Bone, text, " ” " " " p 157 6. W. A. Bone, text, ” M " " ’* p 158-62 7. Tech. Paper 65. Bur. Min. Porter and Ralston. (1914) (A Study of the Oxidation of Goal) 8. Tech. Paper 170. Bur. Mines, by S.H.Katz. (1917) (The Diffusion of Oxygen Through Stored Goal) 9. U of I Bulletin 60, by 3. W. Parr and H.L.Olin. (1912) (The Coking of Coal at Low Temperatures) 10. S.W.Parr, text. The Chemical Examination of ’Water, Fuel, Flue Gases and Lubricants. (1921) 11. J. of the Franklin Inst. 154 , pp. 161-76. (1898) 12. U of I Bulletin 76, by S.W.Parr and H.F. Hadley. (1914) ( Th.6 Analysis of Goal with Phenol as a Solvent) 13. Thesis by 0. A. Cherry for B. 3. degree U of I (1920) (The Effect of Oxygen on the Coking of Coal) 14. J.Am.Chem.Soc . _42, Ho. 7. pp. 1393 July 1920. (Studies in the Adsorption of Charcoal)