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Thermochemistry: List Reactions Synthlet

The feasibility of a chemical reaction can be determined from the enthalpy, H, entropy, S, and the Gibbs' free energy, G.

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Sub select:

0K 200K 298K 500K 1000K 3000K 0°C 25°C 100°C 500°C 1000°C 2500°C    or    Kelvin

List of Thermochemical Reactions Ordered by Gibbs' Free Energy ΔG

Combustion of butane to carbon dioxide and steam     2       +       13 8       +         10 ΔrH⦵ = -5,314.0 kJmol-1 ΔrS⦵ = +0.311 kJK-1mol-1 ΔrG⦵ 298K = -5,406.6 kJmol-1 Keq 298K = >10100 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Combustion of acetone            +       4 3       +         3 ΔrH⦵ = -1,657.9 kJmol-1 ΔrS⦵ = +0.187 kJK-1mol-1 ΔrG⦵ 298K = -1,713.5 kJmol-1 Keq 298K = >10100 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Oxidation of ammonia to nitrogen and steam     4       +       3 2       +         6 ΔrH⦵ = -1,266.5 kJmol-1 ΔrS⦵ = +0.131 kJK-1mol-1 ΔrG⦵ 298K = -1,305.5 kJmol-1 Keq 298K = >10100 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Oxidation of ammonia to nitric oxide with hydrogen peroxide     2       +       5 2       +         8 ΔrH⦵ = -1,006.7 kJmol-1 ΔrS⦵ = +0.210 kJK-1mol-1 ΔrG⦵ 298K = -1,069.3 kJmol-1 Keq 298K = >10100 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Oxidation of ammonia to nitrogen with hydrogen peroxide     2       +       3       +         6 ΔrH⦵ = -991.1 kJmol-1 ΔrS⦵ = +0.060 kJK-1mol-1 ΔrG⦵ 298K = -1,008.8 kJmol-1 Keq 298K = >10100 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Oxidation of ammonia to nitric oxide     4       +       5 4       +         6 ΔrH⦵ = -905.5 kJmol-1 ΔrS⦵ = +0.181 kJK-1mol-1 ΔrG⦵ 298K = -959.3 kJmol-1 Keq 298K = >10100 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Combustion of methane to carbon dioxide and steam            +       2       +         2 ΔrH⦵ = -802.3 kJmol-1 ΔrS⦵ = -0.005 kJK-1mol-1 ΔrG⦵ 298K = -800.8 kJmol-1 Keq 298K = >10100 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 156,097Kelvin Select this reaction for further analysis

Radical coupling of methane radicals to ethane            +       ΔrH⦵ = -376.1 kJmol-1 ΔrS⦵ = -0.159 kJK-1mol-1 ΔrG⦵ 298K = -328.7 kJmol-1 Keq 298K = 4.18 x 10+57 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 2,368Kelvin Select this reaction for further analysis

Decomposition of ozone to oxygen     2 3 ΔrH⦵ = -285.4 kJmol-1 ΔrS⦵ = +0.138 kJK-1mol-1 ΔrG⦵ 298K = -326.4 kJmol-1 Keq 298K = 1.62 x 10+57 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Partial combustion of carbon to carbon monoxide     2       +       2 ΔrH⦵ = -221.1 kJmol-1 ΔrS⦵ = +0.179 kJK-1mol-1 ΔrG⦵ 298K = -274.3 kJmol-1 Keq 298K = 1.21 x 10+48 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Acetylene decomposing to its elements      2       +         ΔrH⦵ = -226.7 kJmol-1 ΔrS⦵ = -0.059 kJK-1mol-1 ΔrG⦵ 298K = -209.2 kJmol-1 Keq 298K = 4.69 x 10+36 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 3,857Kelvin Select this reaction for further analysis

Hydrogen radical plus oxygen gives hydrogen peroxide radical            +       ΔrH⦵ = -215.9 kJmol-1 ΔrS⦵ = -0.091 kJK-1mol-1 ΔrG⦵ 298K = -188.8 kJmol-1 Keq 298K = 1.24 x 10+33 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 2,376Kelvin Select this reaction for further analysis

Carbon monoxide + hydrogen gives methane + water equilibrium            +       3       +         ΔrH⦵ = -250.1 kJmol-1 ΔrS⦵ = -0.334 kJK-1mol-1 ΔrG⦵ 298K = -150.7 kJmol-1 Keq 298K = 2.61 x 10+26 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 750Kelvin Select this reaction for further analysis

The Contact process     2       +       2 ΔrH⦵ = -197.8 kJmol-1 ΔrS⦵ = -0.188 kJK-1mol-1 ΔrG⦵ 298K = -141.7 kJmol-1 Keq 298K = 6.98 x 10+24 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,052Kelvin Select this reaction for further analysis

Hydrogenation to ethylene to ethane            +       ΔrH⦵ = -136.9 kJmol-1 ΔrS⦵ = -0.121 kJK-1mol-1 ΔrG⦵ 298K = -101.0 kJmol-1 Keq 298K = 5.03 x 10+17 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,135Kelvin Select this reaction for further analysis

Hydrogenation of 1-butene            +       ΔrH⦵ = -126.0 kJmol-1 ΔrS⦵ = -0.126 kJK-1mol-1 ΔrG⦵ 298K = -88.4 kJmol-1 Keq 298K = 3.15 x 10+15 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 999Kelvin Select this reaction for further analysis

Acetaldehyde reacting with water to give acetic acid and ethanol     2       +             +         ΔrH⦵ = -91.8 kJmol-1 ΔrS⦵ = -0.070 kJK-1mol-1 ΔrG⦵ 298K = -71.0 kJmol-1 Keq 298K = 2.74 x 1012 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,314Kelvin Select this reaction for further analysis

Hydrolysis of carbon disulfide            +       2       +         2 ΔrH⦵ = -40.8 kJmol-1 ΔrS⦵ = +0.096 kJK-1mol-1 ΔrG⦵ 298K = -69.5 kJmol-1 Keq 298K = 1.54 x 1012 No equilibrium temperature: the reaction is feasible at all temperatures Select this reaction for further analysis

Formation of methane from its elements            +       2 ΔrH⦵ = -74.8 kJmol-1 ΔrS⦵ = -0.081 kJK-1mol-1 ΔrG⦵ 298K = -50.7 kJmol-1 Keq 298K = 7.76 x 108 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 925Kelvin Select this reaction for further analysis

Haber ammonia synthesis            +       3 2 ΔrH⦵ = -92.2 kJmol-1 ΔrS⦵ = -0.199 kJK-1mol-1 ΔrG⦵ 298K = -33.0 kJmol-1 Keq 298K = 6.07 x 105 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 464Kelvin Select this reaction for further analysis

Carbon monnoxide plus water gives hydrogen plus carbon dioxide equilibrium            +             +         ΔrH⦵ = +2.9 kJmol-1 ΔrS⦵ = +0.077 kJK-1mol-1 ΔrG⦵ 298K = -20.0 kJmol-1 Keq 298K = 3,270 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 37Kelvin Select this reaction for further analysis

Dimerisation of NO2 to N2O4            +       ΔrH⦵ = -58.4 kJmol-1 ΔrS⦵ = -0.176 kJK-1mol-1 ΔrG⦵ 298K = -6.0 kJmol-1 Keq 298K = 11.5 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 332Kelvin Select this reaction for further analysis

Hydrogen + iodine in equilibrium with hydrogen iodide            +       2 ΔrH⦵ = +53.0 kJmol-1 ΔrS⦵ = +0.166 kJK-1mol-1 ΔrG⦵ 298K = +3.4 kJmol-1 Keq 298K = 0.255 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 318Kelvin Select this reaction for further analysis

Water-steam equilibrium ΔrH⦵ = +44.0 kJmol-1 ΔrS⦵ = +0.119 kJK-1mol-1 ΔrG⦵ 298K = +8.6 kJmol-1 Keq 298K = 0.0314 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 370Kelvin Select this reaction for further analysis

Decomposing butane to its elements      4       +         5 ΔrH⦵ = +126.2 kJmol-1 ΔrS⦵ = +0.366 kJK-1mol-1 ΔrG⦵ 298K = +17.0 kJmol-1 Keq 298K = 1.03 x 10-3 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 345Kelvin Select this reaction for further analysis

Hydrogenation of benzene            +       3 ΔrH⦵ = -86.3 kJmol-1 ΔrS⦵ = -0.361 kJK-1mol-1 ΔrG⦵ 298K = +21.3 kJmol-1 Keq 298K = 1.85 x 10-4 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 239Kelvin Select this reaction for further analysis

Reduction of iron(III) oxide with hydrogen            +       3 2       +         3 ΔrH⦵ = +98.7 kJmol-1 ΔrS⦵ = +0.142 kJK-1mol-1 ΔrG⦵ 298K = +56.5 kJmol-1 Keq 298K = 1.23 x 10-10 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 697Kelvin Select this reaction for further analysis

Carbon plus water shift reaction            +             +         ΔrH⦵ = +131.3 kJmol-1 ΔrS⦵ = +0.134 kJK-1mol-1 ΔrG⦵ 298K = +91.4 kJmol-1 Keq 298K = 9.45 x 10-17 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 981Kelvin Select this reaction for further analysis

Carbon plus carbon dioxide gives carbon monoxide equilibrium            +       2 ΔrH⦵ = +172.5 kJmol-1 ΔrS⦵ = +0.176 kJK-1mol-1 ΔrG⦵ 298K = +120.0 kJmol-1 Keq 298K = 9.09 x 10-22 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 981Kelvin Select this reaction for further analysis

Decomposition of calcium carbonate to CaO and CO2            +         ΔrH⦵ = +178.3 kJmol-1 ΔrS⦵ = +0.161 kJK-1mol-1 ΔrG⦵ 298K = +130.4 kJmol-1 Keq 298K = 1.37 x 10-23 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,110Kelvin Select this reaction for further analysis

Cracking butane to ethylene and hydrogen      2       +         ΔrH⦵ = +230.7 kJmol-1 ΔrS⦵ = +0.260 kJK-1mol-1 ΔrG⦵ 298K = +153.3 kJmol-1 Keq 298K = 1.34 x 10-27 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 889Kelvin Select this reaction for further analysis

Oxidation of nitrogen to nitric oxide            +       2 ΔrH⦵ = +180.5 kJmol-1 ΔrS⦵ = +0.025 kJK-1mol-1 ΔrG⦵ 298K = +173.1 kJmol-1 Keq 298K = 4.53 x 10-31 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 7,287Kelvin Select this reaction for further analysis

Dimerising methane to acetylene and hydrogen     2       +         3 ΔrH⦵ = +376.4 kJmol-1 ΔrS⦵ = +0.220 kJK-1mol-1 ΔrG⦵ 298K = +310.7 kJmol-1 Keq 298K = 3.54 x 10-55 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,707Kelvin Select this reaction for further analysis

Dioxygen (O2) ozone (O3) equilibrium     3 2 ΔrH⦵ = +285.4 kJmol-1 ΔrS⦵ = -0.138 kJK-1mol-1 ΔrG⦵ 298K = +326.4 kJmol-1 Keq 298K = 6.16 x 10-58 No equilibrium temperature: the reaction is feasible at no temperature Select this reaction for further analysis

Partial oxidation of methane to acetylene, H2 and CO     6       +       2       +         2       +         10 ΔrH⦵ = +681.3 kJmol-1 ΔrS⦵ = +0.781 kJK-1mol-1 ΔrG⦵ 298K = +448.4 kJmol-1 Keq 298K = 2.51 x 10-79 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 872Kelvin Select this reaction for further analysis

Decomposing steam into its elements     2 2       +         ΔrH⦵ = +483.6 kJmol-1 ΔrS⦵ = +0.089 kJK-1mol-1 ΔrG⦵ 298K = +457.2 kJmol-1 Keq 298K = 7.38 x 10-81 ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 5,444Kelvin Select this reaction for further analysis

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Why Reactions Occur

Thermochemical Synthlet

© Mark R. Leach 1999 –

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