## CuCl2 (s) → Cu+2 (aq) + 2 Cl-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Cu+2 (aq)) + 2ΔHf(Cl-1 (aq))] - [1ΔHf(CuCl2 (s))]
[1(64.77) + 2(-167.15)] - [1(-205.85)] = -63.68 kJ
-63.68 kJ     (exothermic)

## Entropy Change

[1ΔSf(Cu+2 (aq)) + 2ΔSf(Cl-1 (aq))] - [1ΔSf(CuCl2 (s))]
[1(-99.58) + 2(56.48)] - [1(108.07)] = -94.69 J/K
-94.69 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cu+2 (aq)) + 2ΔGf(Cl-1 (aq))] - [1ΔGf(CuCl2 (s))]
[1(65.52) + 2(-131.25)] - [1(-161.92)] = -35.06 kJ
-35.06 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-35.45 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1388634.7572
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1388634.7572) will be used to calculate the equilibrium concentration for all species.

 CuCl2 Cu+2 Cl-1 Initial M 0 0 Change -x +x +2x Equilibrium