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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)
[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)
This process is not favorable at 25°C.
Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 369.