CH3COOH (ℓ acetic acid) + 2 O2 (g) → 2 CO2 (g) + 2 H2O (g)

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Stoichiometry

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 CH3COOH        Mass: g O2             Mass: g or Gas Volume: L CO2            Mass: g or Gas Volume: L H2O            Mass: g or Gas Volume: L Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(CO2 (g)) + 2ΔHf(H2O (g))] - [1ΔHf(CH3COOH (ℓ acetic acid)) + 2ΔHf(O2 (g))]
[2(-393.51) + 2(-241.82)] - [1(-484.13) + 2(0)] = -786.53 kJ
-786.53 kJ     (exothermic)

Entropy Change

[2ΔSf(CO2 (g)) + 2ΔSf(H2O (g))] - [1ΔSf(CH3COOH (ℓ acetic acid)) + 2ΔSf(O2 (g))]
[2(213.68) + 2(188.72)] - [1(159.83) + 2(205.03)] = 234.91 J/K
234.91 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(CO2 (g)) + 2ΔGf(H2O (g))] - [1ΔGf(CH3COOH (ℓ acetic acid)) + 2ΔGf(O2 (g))]
[2(-394.38) + 2(-228.59)] - [1(-389.95) + 2(0)] = -855.99 kJ
-855.99 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-856.57 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

9.3606133256e+149
This process is favorable at 25°C.