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Using data from Table A-25, calculate the equilibrium constant expressed as log10K, for the water-gas shift reaction CO + H₂O(g) ⇒ CO₂ + H₂

Using data from Table A-25, calculate the equilibrium constant expressed as log10K, for the water-gas shift reaction CO + H₂O(g) ⇒ CO₂ + H₂

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Using data from Table A-25, calculate the equilibrium constant expressed as log₁0K, for the water-gas shift reaction CO + H₂O (g) ↔ CO₂ + H₂ at 298 K and then at 1000K. Also, determine the equilibrium constant at 298 K and then at 1000K using Table A-27. Table A-25: T(K) 298 1000 log10K
Transcribed Image Text:Using data from Table A-25, calculate the equilibrium constant expressed as log₁0K, for the water-gas shift reaction CO + H₂O (g) ↔ CO₂ + H₂ at 298 K and then at 1000K. Also, determine the equilibrium constant at 298 K and then at 1000K using Table A-27. Table A-25: T(K) 298 1000 log10K
TABLE A-25 Thermochemical Properties of Selected Substances at 298K and 1 atm Substance Carbon Hydrogen Nitrogen Oxygen Carbon monoxide Carbon dioxide Water Water Hydrogen peroxide Ammonia Oxygen Hydrogen Nitrogen Hydroxyl Methane Acetylene Ethylene Ethane Propylene Propane Butane Pentane Octane Octane Benzene Methanol Methanol Ethanol Ethanol Formula C(s) H₂(g) N₂(g) O₂(g) CO(g) CO₂(g) H₂O(g) H₂O(l) H₂O₂(g) NH,(g) O(g) H(g) N(g) OH(g) CH₂(g) C₂H₂(g) C₂H₂(g) C₂Hs(g) C3Hs(g) C₂H₂(g) C₂H₂(g) C3H₁2(g) CgH18(g) C8H18(1) CH(g) CH₂OH(g) CH₂OH(1) C₂H₂OH(g) C₂H₂OH(1) Molar Mass, M (kg/kmol) 12.01 2.016 28.01 32.00 28.01 44.01 18.02 18.02 34.02 17.03 16.00 1.008 14.01 17.01 16.04 26.04 28.05 30.07 42.08 44.09 58.12 72.15 114.22 114.22 78.11 32.04 32.04 46.07 46.07 Enthalpy of Formation, h (kJ/kmol) 0 0 0 0 -110,530 -393,520 -241,820 -285,830 -136,310 -46,190 249,170 218,000 472,680 39,460 -74,850 226,730 52,280 -84,680 20,410 -103,850 -126,150 -146,440 -208,450 -249,910 82,930 -200,890 -238,810 -235,310 -277,690 Gibbs Function of Formation, gi (kJ/kmol) 0000 0 -137,150 -394,380 -228,590 -237,180 -105,600 -16,590 231,770 203,290 455,510 34,280 -50,790 209,170 68,120 -32,890 62,720 -23,490 -15,710 -8,200 17,320 6,610 129,660 -162,140 -166,290 -168,570 -174,890 Absolute Entropy, sº (kJ/kmol. K) 5.74 130.57 191.50 205.03 197.54 213.69 188.72 69.95 232.63 192.33 160.95 114.61 153.19 183.75 186.16 200.85 219.83 229.49 266.94 269.91 310.03 348.40 463.67 360.79 269.20 239.70 126.80 282.59 160.70 Heating Values Higher, Lower, HHV LHV (kJ/kg) (kJ/kg) 32,770 141,780 55,510 49,910 50,300 51,870 48,920 50,350 49,500 49,010 48,260 47,900 42,270 23,850 22,670 30,590 29,670 32,770 119,950 ||||||||||||| 50,020 48,220 47,160 47,480 45,780 46,360 45,720 45,350 44,790 44,430 40,580 21,110 19,920 27,720 26,800
Transcribed Image Text:TABLE A-25 Thermochemical Properties of Selected Substances at 298K and 1 atm Substance Carbon Hydrogen Nitrogen Oxygen Carbon monoxide Carbon dioxide Water Water Hydrogen peroxide Ammonia Oxygen Hydrogen Nitrogen Hydroxyl Methane Acetylene Ethylene Ethane Propylene Propane Butane Pentane Octane Octane Benzene Methanol Methanol Ethanol Ethanol Formula C(s) H₂(g) N₂(g) O₂(g) CO(g) CO₂(g) H₂O(g) H₂O(l) H₂O₂(g) NH,(g) O(g) H(g) N(g) OH(g) CH₂(g) C₂H₂(g) C₂H₂(g) C₂Hs(g) C3Hs(g) C₂H₂(g) C₂H₂(g) C3H₁2(g) CgH18(g) C8H18(1) CH(g) CH₂OH(g) CH₂OH(1) C₂H₂OH(g) C₂H₂OH(1) Molar Mass, M (kg/kmol) 12.01 2.016 28.01 32.00 28.01 44.01 18.02 18.02 34.02 17.03 16.00 1.008 14.01 17.01 16.04 26.04 28.05 30.07 42.08 44.09 58.12 72.15 114.22 114.22 78.11 32.04 32.04 46.07 46.07 Enthalpy of Formation, h (kJ/kmol) 0 0 0 0 -110,530 -393,520 -241,820 -285,830 -136,310 -46,190 249,170 218,000 472,680 39,460 -74,850 226,730 52,280 -84,680 20,410 -103,850 -126,150 -146,440 -208,450 -249,910 82,930 -200,890 -238,810 -235,310 -277,690 Gibbs Function of Formation, gi (kJ/kmol) 0000 0 -137,150 -394,380 -228,590 -237,180 -105,600 -16,590 231,770 203,290 455,510 34,280 -50,790 209,170 68,120 -32,890 62,720 -23,490 -15,710 -8,200 17,320 6,610 129,660 -162,140 -166,290 -168,570 -174,890 Absolute Entropy, sº (kJ/kmol. K) 5.74 130.57 191.50 205.03 197.54 213.69 188.72 69.95 232.63 192.33 160.95 114.61 153.19 183.75 186.16 200.85 219.83 229.49 266.94 269.91 310.03 348.40 463.67 360.79 269.20 239.70 126.80 282.59 160.70 Heating Values Higher, Lower, HHV LHV (kJ/kg) (kJ/kg) 32,770 141,780 55,510 49,910 50,300 51,870 48,920 50,350 49,500 49,010 48,260 47,900 42,270 23,850 22,670 30,590 29,670 32,770 119,950 ||||||||||||| 50,020 48,220 47,160 47,480 45,780 46,360 45,720 45,350 44,790 44,430 40,580 21,110 19,920 27,720 26,800
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