CuCl (s) → Cu+1 (aq) + Cl-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Cu+1 (aq)) + 1ΔHf(Cl-1 (aq))] - [1ΔHf(CuCl (s))]
[1(71.67) + 1(-167.15)] - [1(-137.24)] = 41.76 kJ
41.76 kJ     (endothermic)

Entropy Change

[1ΔSf(Cu+1 (aq)) + 1ΔSf(Cl-1 (aq))] - [1ΔSf(CuCl (s))]
[1(40.58) + 1(56.48)] - [1(86.19)] = 10.87 J/K
10.87 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cu+1 (aq)) + 1ΔGf(Cl-1 (aq))] - [1ΔGf(CuCl (s))]
[1(50) + 1(-131.25)] - [1(-119.87)] = 38.62 kJ
38.62 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

1.7127431861e-007
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.7127431861e-007) will be used to calculate the equilibrium concentration for all species.

CuCl Cu+1 Cl-1
Initial M   0 0
Change -x +x +x
Equilibrium