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Enthalpy of Reaction
[1ΔHf(CH3COOH (ℓ acetic acid))] - [2ΔHf(C (s graphite)) + 2ΔHf(H2 (g)) + 1ΔHf(O2 (g))]
[1(-484.13)] - [2(0) + 2(0) + 1(0)] = -484.13 kJ
-484.13 kJ (exothermic)
[1ΔSf(CH3COOH (ℓ acetic acid))] - [2ΔSf(C (s graphite)) + 2ΔSf(H2 (g)) + 1ΔSf(O2 (g))]
[1(159.83)] - [2(5.69) + 2(130.59) + 1(205.03)] = -317.76 J/K
-317.76 J/K (decrease in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(CH3COOH (ℓ acetic acid))] - [2ΔGf(C (s graphite)) + 2ΔGf(H2 (g)) + 1ΔGf(O2 (g))]
[1(-389.95)] - [2(0) + 2(0) + 1(0)] = -389.95 kJ
-389.95 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-389.39 kJ (spontaneous)
Equilibrium Constant, K (at 298.15 K)
This process is favorable at 25°C.
Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 224.