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

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Combustion

## 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 Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(CO2 (g)) + 2ΔHf(H2O (ℓ))] - [1ΔHf(CH3COOH (ℓ acetic acid)) + 2ΔHf(O2 (g))]
[2(-393.51) + 2(-285.83)] - [1(-484.13) + 2(0)] = -874.55 kJ
-874.55 kJ     (exothermic)

## Entropy Change

[2ΔSf(CO2 (g)) + 2ΔSf(H2O (ℓ))] - [1ΔSf(CH3COOH (ℓ acetic acid)) + 2ΔSf(O2 (g))]
[2(213.68) + 2(69.91)] - [1(159.83) + 2(205.03)] = -2.70999999999992 J/K
-2.71 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(CO2 (g)) + 2ΔGf(H2O (ℓ))] - [1ΔGf(CH3COOH (ℓ acetic acid)) + 2ΔGf(O2 (g))]
[2(-394.38) + 2(-237.18)] - [1(-389.95) + 2(0)] = -873.17 kJ
-873.17 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-873.74 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

9.5780601958e+152
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; pp 224-226.