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Enthalpy of Reaction
[2ΔHf(H2 (g)) + 1ΔHf(CO (g))] - [1ΔHf(CH3OH (ℓ methanol))]
[2(0) + 1(-110.54)] - [1(-239.03)] = 128.49 kJ
128.49 kJ (endothermic)
[2ΔSf(H2 (g)) + 1ΔSf(CO (g))] - [1ΔSf(CH3OH (ℓ methanol))]
[2(130.59) + 1(197.9)] - [1(127.24)] = 331.84 J/K
331.84 J/K (increase in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[2ΔGf(H2 (g)) + 1ΔGf(CO (g))] - [1ΔGf(CH3OH (ℓ methanol))]
[2(0) + 1(-137.28)] - [1(-166.82)] = 29.54 kJ
29.54 kJ (nonspontaneous)
From ΔG = ΔH - TΔS:
29.55 kJ (nonspontaneous)
Equilibrium Constant, K (at 298.15 K)
This process is not favorable at 25°C.
Kotz, John C. and Treichel, Paul. Chemistry & Chemical Reactivity 4th ed.; Thomson Brooks/Cole: Belmont, CA, 1999; p 164.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 158.