2 AlCl3 (ℓ) → 2 Al (s) + 3 Cl2 (g)

Back to reactions list

 

Reaction Type:

Decomposition

Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

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.

Reference(s):

Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 369.

Back to list of reactions