List of Thermochemical Reactions Ordered by Gibbs' Free Energy ΔG 
Combustion of butane to carbon dioxide and steam

Δ_{r}H = 5,314.0 kJmol^{1}
Δ_{r}S = +0.311 kJK^{1}mol^{1}
Δ_{r}G 298K = 5,406.6 kJmol^{1}
K_{eq} 298K = >10^{100}
No equilibrium temperature: the reaction is feasible at all temperatures
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Δ_{r}H = 1,657.9 kJmol^{1}
Δ_{r}S = +0.187 kJK^{1}mol^{1}
Δ_{r}G 298K = 1,713.5 kJmol^{1}
K_{eq} 298K = >10^{100}
No equilibrium temperature: the reaction is feasible at all temperatures
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Oxidation of ammonia to nitrogen and steam

Δ_{r}H = 1,266.5 kJmol^{1}
Δ_{r}S = +0.131 kJK^{1}mol^{1}
Δ_{r}G 298K = 1,305.5 kJmol^{1}
K_{eq} 298K = >10^{100}
No equilibrium temperature: the reaction is feasible at all temperatures
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Oxidation of ammonia to nitric oxide with hydrogen peroxide

Δ_{r}H = 1,006.7 kJmol^{1}
Δ_{r}S = +0.210 kJK^{1}mol^{1}
Δ_{r}G 298K = 1,069.3 kJmol^{1}
K_{eq} 298K = >10^{100}
No equilibrium temperature: the reaction is feasible at all temperatures
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Oxidation of ammonia to nitrogen with hydrogen peroxide

Δ_{r}H = 991.1 kJmol^{1}
Δ_{r}S = +0.060 kJK^{1}mol^{1}
Δ_{r}G 298K = 1,008.8 kJmol^{1}
K_{eq} 298K = >10^{100}
No equilibrium temperature: the reaction is feasible at all temperatures
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Oxidation of ammonia to nitric oxide

Δ_{r}H = 905.5 kJmol^{1}
Δ_{r}S = +0.181 kJK^{1}mol^{1}
Δ_{r}G 298K = 959.3 kJmol^{1}
K_{eq} 298K = >10^{100}
No equilibrium temperature: the reaction is feasible at all temperatures
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Combustion of methane to carbon dioxide and steam

Δ_{r}H = 802.3 kJmol^{1}
Δ_{r}S = 0.005 kJK^{1}mol^{1}
Δ_{r}G 298K = 800.8 kJmol^{1}
K_{eq} 298K = >10^{100}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 156,097Kelvin
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Radical coupling of methane radicals to ethane

Δ_{r}H = 376.1 kJmol^{1}
Δ_{r}S = 0.159 kJK^{1}mol^{1}
Δ_{r}G 298K = 328.7 kJmol^{1}
K_{eq} 298K = 4.18 x 10^{+57}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 2,368Kelvin
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Decomposition of ozone to oxygen

Δ_{r}H = 285.4 kJmol^{1}
Δ_{r}S = +0.138 kJK^{1}mol^{1}
Δ_{r}G 298K = 326.4 kJmol^{1}
K_{eq} 298K = 1.62 x 10^{+57}
No equilibrium temperature: the reaction is feasible at all temperatures
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Partial combustion of carbon to carbon monoxide

Δ_{r}H = 221.1 kJmol^{1}
Δ_{r}S = +0.179 kJK^{1}mol^{1}
Δ_{r}G 298K = 274.3 kJmol^{1}
K_{eq} 298K = 1.21 x 10^{+48}
No equilibrium temperature: the reaction is feasible at all temperatures
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Acetylene decomposing to its elements

Δ_{r}H = 226.7 kJmol^{1}
Δ_{r}S = 0.059 kJK^{1}mol^{1}
Δ_{r}G 298K = 209.2 kJmol^{1}
K_{eq} 298K = 4.69 x 10^{+36}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 3,857Kelvin
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Hydrogen radical plus oxygen gives hydrogen peroxide radical

Δ_{r}H = 215.9 kJmol^{1}
Δ_{r}S = 0.091 kJK^{1}mol^{1}
Δ_{r}G 298K = 188.8 kJmol^{1}
K_{eq} 298K = 1.24 x 10^{+33}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 2,376Kelvin
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Carbon monoxide + hydrogen gives methane + water equilibrium

Δ_{r}H = 250.1 kJmol^{1}
Δ_{r}S = 0.334 kJK^{1}mol^{1}
Δ_{r}G 298K = 150.7 kJmol^{1}
K_{eq} 298K = 2.61 x 10^{+26}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 750Kelvin
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Δ_{r}H = 197.8 kJmol^{1}
Δ_{r}S = 0.188 kJK^{1}mol^{1}
Δ_{r}G 298K = 141.7 kJmol^{1}
K_{eq} 298K = 6.98 x 10^{+24}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,052Kelvin
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Hydrogenation to ethylene to ethane

Δ_{r}H = 136.9 kJmol^{1}
Δ_{r}S = 0.121 kJK^{1}mol^{1}
Δ_{r}G 298K = 101.0 kJmol^{1}
K_{eq} 298K = 5.03 x 10^{+17}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,135Kelvin
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Hydrogenation of 1butene

Δ_{r}H = 126.0 kJmol^{1}
Δ_{r}S = 0.126 kJK^{1}mol^{1}
Δ_{r}G 298K = 88.4 kJmol^{1}
K_{eq} 298K = 3.15 x 10^{+15}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 999Kelvin
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Acetaldehyde reacting with water to give acetic acid and ethanol

Δ_{r}H = 91.8 kJmol^{1}
Δ_{r}S = 0.070 kJK^{1}mol^{1}
Δ_{r}G 298K = 71.0 kJmol^{1}
K_{eq} 298K = 2.74 x 10^{12}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,314Kelvin
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Hydrolysis of carbon disulfide

Δ_{r}H = 40.8 kJmol^{1}
Δ_{r}S = +0.096 kJK^{1}mol^{1}
Δ_{r}G 298K = 69.5 kJmol^{1}
K_{eq} 298K = 1.54 x 10^{12}
No equilibrium temperature: the reaction is feasible at all temperatures
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Formation of methane from its elements

Δ_{r}H = 74.8 kJmol^{1}
Δ_{r}S = 0.081 kJK^{1}mol^{1}
Δ_{r}G 298K = 50.7 kJmol^{1}
K_{eq} 298K = 7.76 x 10^{8}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 925Kelvin
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Δ_{r}H = 92.2 kJmol^{1}
Δ_{r}S = 0.199 kJK^{1}mol^{1}
Δ_{r}G 298K = 33.0 kJmol^{1}
K_{eq} 298K = 6.07 x 10^{5}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 464Kelvin
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Carbon monnoxide plus water gives hydrogen plus carbon dioxide equilibrium

Δ_{r}H = +2.9 kJmol^{1}
Δ_{r}S = +0.077 kJK^{1}mol^{1}
Δ_{r}G 298K = 20.0 kJmol^{1}
K_{eq} 298K = 3,270
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 37Kelvin
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Dimerisation of NO_{2} to N_{2}O_{4}

Δ_{r}H = 58.4 kJmol^{1}
Δ_{r}S = 0.176 kJK^{1}mol^{1}
Δ_{r}G 298K = 6.0 kJmol^{1}
K_{eq} 298K = 11.5
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 332Kelvin
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Hydrogen + iodine in equilibrium with hydrogen iodide

Δ_{r}H = +53.0 kJmol^{1}
Δ_{r}S = +0.166 kJK^{1}mol^{1}
Δ_{r}G 298K = +3.4 kJmol^{1}
K_{eq} 298K = 0.255
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 318Kelvin
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Δ_{r}H = +44.0 kJmol^{1}
Δ_{r}S = +0.119 kJK^{1}mol^{1}
Δ_{r}G 298K = +8.6 kJmol^{1}
K_{eq} 298K = 0.0314
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 370Kelvin
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Decomposing butane to its elements

Δ_{r}H = +126.2 kJmol^{1}
Δ_{r}S = +0.366 kJK^{1}mol^{1}
Δ_{r}G 298K = +17.0 kJmol^{1}
K_{eq} 298K = 1.03 x 10^{3}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 345Kelvin
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Δ_{r}H = 86.3 kJmol^{1}
Δ_{r}S = 0.361 kJK^{1}mol^{1}
Δ_{r}G 298K = +21.3 kJmol^{1}
K_{eq} 298K = 1.85 x 10^{4}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 239Kelvin
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Reduction of iron(III) oxide with hydrogen

Δ_{r}H = +98.7 kJmol^{1}
Δ_{r}S = +0.142 kJK^{1}mol^{1}
Δ_{r}G 298K = +56.5 kJmol^{1}
K_{eq} 298K = 1.23 x 10^{10}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 697Kelvin
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Carbon plus water shift reaction

Δ_{r}H = +131.3 kJmol^{1}
Δ_{r}S = +0.134 kJK^{1}mol^{1}
Δ_{r}G 298K = +91.4 kJmol^{1}
K_{eq} 298K = 9.45 x 10^{17}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 981Kelvin
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Carbon plus carbon dioxide gives carbon monoxide equilibrium

Δ_{r}H = +172.5 kJmol^{1}
Δ_{r}S = +0.176 kJK^{1}mol^{1}
Δ_{r}G 298K = +120.0 kJmol^{1}
K_{eq} 298K = 9.09 x 10^{22}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 981Kelvin
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Decomposition of calcium carbonate to CaO and CO_{2}

Δ_{r}H = +178.3 kJmol^{1}
Δ_{r}S = +0.161 kJK^{1}mol^{1}
Δ_{r}G 298K = +130.4 kJmol^{1}
K_{eq} 298K = 1.37 x 10^{23}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,110Kelvin
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Cracking butane to ethylene and hydrogen

Δ_{r}H = +230.7 kJmol^{1}
Δ_{r}S = +0.260 kJK^{1}mol^{1}
Δ_{r}G 298K = +153.3 kJmol^{1}
K_{eq} 298K = 1.34 x 10^{27}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 889Kelvin
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Oxidation of nitrogen to nitric oxide

Δ_{r}H = +180.5 kJmol^{1}
Δ_{r}S = +0.025 kJK^{1}mol^{1}
Δ_{r}G 298K = +173.1 kJmol^{1}
K_{eq} 298K = 4.53 x 10^{31}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 7,287Kelvin
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Dimerising methane to acetylene and hydrogen

Δ_{r}H = +376.4 kJmol^{1}
Δ_{r}S = +0.220 kJK^{1}mol^{1}
Δ_{r}G 298K = +310.7 kJmol^{1}
K_{eq} 298K = 3.54 x 10^{55}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 1,707Kelvin
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Dioxygen (O_{2}) ozone (O_{3}) equilibrium

Δ_{r}H = +285.4 kJmol^{1}
Δ_{r}S = 0.138 kJK^{1}mol^{1}
Δ_{r}G 298K = +326.4 kJmol^{1}
K_{eq} 298K = 6.16 x 10^{58}
No equilibrium temperature: the reaction is feasible at no temperature
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Partial oxidation of methane to acetylene, H_{2} and CO

Δ_{r}H = +681.3 kJmol^{1}
Δ_{r}S = +0.781 kJK^{1}mol^{1}
Δ_{r}G 298K = +448.4 kJmol^{1}
K_{eq} 298K = 2.51 x 10^{79}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 872Kelvin
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Decomposing steam into its elements

Δ_{r}H = +483.6 kJmol^{1}
Δ_{r}S = +0.089 kJK^{1}mol^{1}
Δ_{r}G 298K = +457.2 kJmol^{1}
K_{eq} 298K = 7.38 x 10^{81}
ΔG° = 0.0 (zero, and so the system is at equilibrium) at a temperature of 5,444Kelvin
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