CuI (s) → Cu+1 (aq) + I-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Cu+1 (aq)) + 1ΔHf(I-1 (aq))] - [1ΔHf(CuI (s))]
[1(71.67) + 1(-55.19)] - [1(-67.78)] = 84.26 kJ
84.26 kJ     (endothermic)

Entropy Change

[1ΔSf(Cu+1 (aq)) + 1ΔSf(I-1 (aq))] - [1ΔSf(CuI (s))]
[1(40.58) + 1(111.29)] - [1(96.65)] = 55.22 J/K
55.22 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cu+1 (aq)) + 1ΔGf(I-1 (aq))] - [1ΔGf(CuI (s))]
[1(50) + 1(-51.59)] - [1(-69.45)] = 67.86 kJ
67.86 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

1.29056783927046E-12
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.29056783927046E-12) will be used to calculate the equilibrium concentration for all species.

CuI Cu+1 I-1
Initial M   0 0
Change -x +x +x
Equilibrium