the coking properties of coal at elevated pressures. - Argonne ...
the coking properties of coal at elevated pressures. - Argonne ... the coking properties of coal at elevated pressures. - Argonne ...
than in steam. Figure 9 shows data obtained for a char-5% K CO Qhe same sample as that used in Figure 3) on gasification in 1 atm. C02 between 600 a8d 980 C. In this case, during four successive thermal cycles the kinetic data were remarkably constant, with only a slight decrease in rates between the first and second cycles. The apparent activation energy for this series of experiments was 49.3 Kcal/mole. Similar data for a char sample to which 5 % K co had been added before the 700°C charring step are shown in Figure 10. Again, following a {mad reduction in gasification rates between the first and second cycles, the reactivity ota further cycling was reproducible, with an apparent activation energy of 53.8 Kcal/mole. Comparison with Figure 9 indicates that the catalytic effect of the K CO was similar regardless of whether the salt was added before or after charring. Similar Jatalor a CH3COOK-doped char sample are shown in Figure 11. In this case also, following a slight reduction in reactivity between cycles I and 2, subsequent kinetic data were quite reproducible. Comparison with Figure 5 shows the marked difference in behavior of this doped char sample in the two gaseous environments. Gasification data in C02 for char doped with 5% Li CO Na CO and K CO (added prior to charring) are shown in Figure 12. In this envi?onrr?&t dierd was nb si2nificant difference in activity between the three salts when compared on a weight % basis. The effect of increasing concentration of K CO (added prior to charring) on the C02 gasification kinetics is illustrated in Figure 13. ReagtivAy generally increased with K CO concentration, at least up to the 20% level, however, the effect on apparent activation eneqgy 3 was small. Reaction between Alkali Carbonates and Carbon When K CO is heated with carbon in an inert atmosphere, a solid state reaction takes place between2 60d and 9OO0C, depending on the particle size and extent of physical contact between the two phases. The products of this r tion are CO and potassium vapor which sublimes into the cooler parts of the apparatusfB Figure 14 shows thermograms (weight changes vs. temperature) for K2CO3_char and K2C03-graphite mixtures on heating in dry helium in the thermobalance at an increasing temperature of 10°C/min. In the case of graphite, loss in weight became marked above 800°C and the reaction was essentially completed at 1000°C. The char had a much larger surface area than the graphite and reaction with the salt began at about 600OC. This solid state reaction, which takes place in the gasification range, is believed to play tyoiwortant role in the gasification of carbon with C02 as discussed in the next section. or steam in the presence of the K2C0 ' 3 DISCUSSION The reactivities of coal chars are obviously strongly influenced by a number of factors such as charring temperature and thermal history, pore size distribution and the presence of ubiquitous mineral impurities. However, the catalytic behavior of additives such as the alkali metal carbonates is similar for char and graphite and the same mechanisms probably operate in both cases. The main effect of the salt catalysts (Figures 1,2,12,13) in both gasification reactions is to increase the pre-exponential factor of the rate equation. Changes in the apparent activation energy are small from catalyst to catalyst and on increasing the salt concentration. The most likely explanation of this effect is that the salt reacts with the char substrate to produce active sites on the surface where gasification can proceed. Increasing the amount of salt present increases the effective concentration of these active sites up to the point at which the surface becomes saturated. A plausible mechanism which has been proposed previo~sly(~~,~~~~~) to account for the catalytic effects of Na2C03 and K2C0 in these reactions is shown in Table 11. A common first 3
step, reaction (I) is suggested for both reactions, with the subsequent steps being different for C02 and H20 as the gaseous oxidant. C - C02 REACTION C - H20 REACTION M2C03 + 2C = 2M + 3CO 2M + co2 = M20 + co M20 + C02 = M2C03 c + co2 = 2co M2C03 + 2C = 2M + 3CO 2M + 2H20 = 2MOH + H2 2MOH + CO = M2C03 + H2 C + H 20 = CO + H2 Table n: Carbon Gasification Catalyzed by Na2C03 or K2C03 Although reaction (I) possesses a positive free energy change at temperatures in the 600- 1000°C range, at low partial pressures of CO the reaction can proceed rapidly, as shown by the TGA data in Figure IS. Figure IS shows the equilibrium stability regions of K C03 and K(P, for reaction (l), calculated from free energy data, as functions of temperaturg and the partial pressures (in atmospheres) of K(g) and CO. The sloping lines at each temperature separate the region of stability of %C03 (upper left) from that of K(g) (lower right). An overall gasification rate of 5 x IO- min- (about the maximu3attained in this study at 9OO0C) would give an ambient partial pressure of CO of about 10 atm. above the gasifying char sample. At this value of Pco, and with a similar value of PK, Figure 15 indicates that reaction (1) would be thermodynamically possible for all temperatures above about 800°C. At a temperature of 6OO0C the measured gasification rate, and the ambient value of P are about two orders of magnitude ess than at 9OO0C and Figure 15 shows that reaction (IF?: again possible for P ?l Pco = IO- atm. The steady state values of P reaction will in fact be much less than $ = because of the occurrence of reactions (2) and [f& DiFect evidence that reaction (3) does oc%? has recently been obtained by Wood et al., using high temperature Knudsen cell mass spectrometry. On heating K C03 and carbon together at temperatures of 500°C and above, the evolution of K vapor and 20 could be measured. Thus, reaction (I), which is inhibited by increasing amounts of CO in the gas phase, is probably the rate determining step in the case of the gasification reactions catalyzed by Na2C0 and K CO . Reactions (2) and (3) and also (4) and (5) have large negative free energy values a? gasifi&tiofi temperatures and are thus favored thermodynamically, although little is known about their kinetics. A somewhat different pathway probably operates in the case of the reactions catalyzed by Li CO as Li 0 is more stable than the oxides of Na and K, also Li CO is more easily hy&olyzed 3 to Aydroxide than the carbonates of Na and K. A possible sequegce Jf reactions that might be involved in the catalysis process in the case of Li CO is shown in Table Ill below. Evidence for the occurrence of these individual reactions is &ill,%owever, indirect and future efforts will be directed to exploring the catalytic process by the aid of isotopic tracers and in determining the relative rates of the elementary steps involved in the catalyzed gasification process. 79 (2) (3) (1) (4) (5)
- Page 28 and 29: 1. . 2. 3. 4. 5. 6. 7. 8. 9. REFERE
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- Page 36 and 37: These phenomena iiiay be described
- Page 38 and 39: Walker, P. L., Rusinko, F., and Aus
- Page 40 and 41: -""I- *I,".. I Dlrf".,on Co.1flcl.n
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- Page 44 and 45: Changes in Char Chemistry The infra
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- Page 50 and 51: COAL PYROLYSIS AT HIGH TEMPERATURES
- Page 52 and 53: actions, decreasing the secondary c
- Page 54 and 55: 01 40 60 TI MEISeC) 80 100 120 140
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- Page 62 and 63: si sio Fraction of solid species i
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- Page 68 and 69: to condense excess steam, the press
- Page 70 and 71: conversion-time data.* The integrat
- Page 72 and 73: catalyzed and uncatalyzed runs were
- Page 74 and 75: CATALYTIC EFFECTS OF ALKALI METAL S
- Page 76 and 77: %me thermogravimetric measurements
- Page 80 and 81: C - C02 REACTION C - H20 REACTION L
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- Page 105 and 106: TABLE 3 -----______________________
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- Page 109 and 110: I. INTRODUCTION DIRECT METHANATION
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- Page 113 and 114: Preparing process flow diagrams and
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- Page 117 and 118: (JMS-OlBM-2). The mass spectra were
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than in steam. Figure 9 shows d<strong>at</strong>a obtained for a char-5% K CO Qhe same sample as th<strong>at</strong><br />
used in Figure 3) on gasific<strong>at</strong>ion in 1 <strong>at</strong>m. C02 between 600 a8d 980 C. In this case, during<br />
four successive <strong>the</strong>rmal cycles <strong>the</strong> kinetic d<strong>at</strong>a were remarkably constant, with only a slight<br />
decrease in r<strong>at</strong>es between <strong>the</strong> first and second cycles. The apparent activ<strong>at</strong>ion energy for this<br />
series <strong>of</strong> experiments was 49.3 Kcal/mole. Similar d<strong>at</strong>a for a char sample to which 5 % K co<br />
had been added before <strong>the</strong> 700°C charring step are shown in Figure 10. Again, following a {mad<br />
reduction in gasific<strong>at</strong>ion r<strong>at</strong>es between <strong>the</strong> first and second cycles, <strong>the</strong> reactivity ota fur<strong>the</strong>r<br />
cycling was reproducible, with an apparent activ<strong>at</strong>ion energy <strong>of</strong> 53.8 Kcal/mole. Comparison<br />
with Figure 9 indic<strong>at</strong>es th<strong>at</strong> <strong>the</strong> c<strong>at</strong>alytic effect <strong>of</strong> <strong>the</strong> K CO was similar regardless <strong>of</strong><br />
whe<strong>the</strong>r <strong>the</strong> salt was added before or after charring. Similar J<strong>at</strong>alor a CH3COOK-doped char<br />
sample are shown in Figure 11. In this case also, following a slight reduction in reactivity<br />
between cycles I and 2, subsequent kinetic d<strong>at</strong>a were quite reproducible. Comparison with<br />
Figure 5 shows <strong>the</strong> marked difference in behavior <strong>of</strong> this doped char sample in <strong>the</strong> two gaseous<br />
environments.<br />
Gasific<strong>at</strong>ion d<strong>at</strong>a in C02 for char doped with 5% Li CO Na CO and K CO (added<br />
prior to charring) are shown in Figure 12. In this envi?onrr?&t dierd was nb si2nificant<br />
difference in activity between <strong>the</strong> three salts when compared on a weight % basis. The effect<br />
<strong>of</strong> increasing concentr<strong>at</strong>ion <strong>of</strong> K CO (added prior to charring) on <strong>the</strong> C02 gasific<strong>at</strong>ion kinetics<br />
is illustr<strong>at</strong>ed in Figure 13. ReagtivAy generally increased with K CO concentr<strong>at</strong>ion, <strong>at</strong> least<br />
up to <strong>the</strong> 20% level, however, <strong>the</strong> effect on apparent activ<strong>at</strong>ion eneqgy<br />
3<br />
was small.<br />
Reaction between Alkali Carbon<strong>at</strong>es and Carbon<br />
When K CO is he<strong>at</strong>ed with carbon in an inert <strong>at</strong>mosphere, a solid st<strong>at</strong>e reaction takes<br />
place between2 60d and 9OO0C, depending on <strong>the</strong> particle size and extent <strong>of</strong> physical contact<br />
between <strong>the</strong> two phases. The products <strong>of</strong> this r tion are CO and potassium vapor which<br />
sublimes into <strong>the</strong> cooler parts <strong>of</strong> <strong>the</strong> appar<strong>at</strong>usfB Figure 14 shows <strong>the</strong>rmograms (weight<br />
changes vs. temper<strong>at</strong>ure) for K2CO3_char and K2C03-graphite mixtures on he<strong>at</strong>ing in dry<br />
helium in <strong>the</strong> <strong>the</strong>rmobalance <strong>at</strong> an increasing temper<strong>at</strong>ure <strong>of</strong> 10°C/min. In <strong>the</strong> case <strong>of</strong><br />
graphite, loss in weight became marked above 800°C and <strong>the</strong> reaction was essentially<br />
completed <strong>at</strong> 1000°C. The char had a much larger surface area than <strong>the</strong> graphite and reaction<br />
with <strong>the</strong> salt began <strong>at</strong> about 600OC. This solid st<strong>at</strong>e reaction, which takes place in <strong>the</strong><br />
gasific<strong>at</strong>ion range, is believed to play tyoiwortant role in <strong>the</strong> gasific<strong>at</strong>ion <strong>of</strong> carbon with C02<br />
as discussed in <strong>the</strong> next section.<br />
or steam in <strong>the</strong> presence <strong>of</strong> <strong>the</strong> K2C0 '<br />
3<br />
DISCUSSION<br />
The reactivities <strong>of</strong> <strong>coal</strong> chars are obviously strongly influenced by a number <strong>of</strong> factors<br />
such as charring temper<strong>at</strong>ure and <strong>the</strong>rmal history, pore size distribution and <strong>the</strong> presence <strong>of</strong><br />
ubiquitous mineral impurities. However, <strong>the</strong> c<strong>at</strong>alytic behavior <strong>of</strong> additives such as <strong>the</strong> alkali<br />
metal carbon<strong>at</strong>es is similar for char and graphite and <strong>the</strong> same mechanisms probably oper<strong>at</strong>e in<br />
both cases.<br />
The main effect <strong>of</strong> <strong>the</strong> salt c<strong>at</strong>alysts (Figures 1,2,12,13) in both gasific<strong>at</strong>ion reactions is<br />
to increase <strong>the</strong> pre-exponential factor <strong>of</strong> <strong>the</strong> r<strong>at</strong>e equ<strong>at</strong>ion. Changes in <strong>the</strong> apparent activ<strong>at</strong>ion<br />
energy are small from c<strong>at</strong>alyst to c<strong>at</strong>alyst and on increasing <strong>the</strong> salt concentr<strong>at</strong>ion. The most<br />
likely explan<strong>at</strong>ion <strong>of</strong> this effect is th<strong>at</strong> <strong>the</strong> salt reacts with <strong>the</strong> char substr<strong>at</strong>e to produce active<br />
sites on <strong>the</strong> surface where gasific<strong>at</strong>ion can proceed. Increasing <strong>the</strong> amount <strong>of</strong> salt present<br />
increases <strong>the</strong> effective concentr<strong>at</strong>ion <strong>of</strong> <strong>the</strong>se active sites up to <strong>the</strong> point <strong>at</strong> which <strong>the</strong> surface<br />
becomes s<strong>at</strong>ur<strong>at</strong>ed.<br />
A plausible mechanism which has been proposed previo~sly(~~,~~~~~)<br />
to account for <strong>the</strong><br />
c<strong>at</strong>alytic effects <strong>of</strong> Na2C03 and K2C0 in <strong>the</strong>se reactions is shown in Table 11. A common first<br />
3