## 2 AlCl3 (ℓ) → 2 Al (s) + 3 Cl2 (g)

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Decomposition

## Stoichiometry

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 Heat Added: kJ AlCl3          Mass: g Al             Mass: g Cl2            Mass: g or Gas Volume: L

## Enthalpy of Reaction

[2ΔHf(Al (s)) + 3ΔHf(Cl2 (g))] - [2ΔHf(AlCl3 (ℓ))]
[2(0) + 3(0)] - [2(-674.8)] = 1349.6 kJ
1,349.60 kJ     (endothermic)

## Entropy Change

[2ΔSf(Al (s)) + 3ΔSf(Cl2 (g))] - [2ΔSf(AlCl3 (ℓ))]
[2(28.33) + 3(222.97)] - [2(172.92)] = 379.73 J/K
379.73 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Al (s)) + 3ΔGf(Cl2 (g))] - [2ΔGf(AlCl3 (ℓ))]
[2(0) + 3(0)] - [2(-618.19)] = 1236.38 kJ
1,236.38 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
1236.38 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

2.4184815481e-217
This process is not favorable at 25°C.