CdF2 (s) → Cd+2 (aq) + 2 F-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Cd+2 (aq)) + 2ΔHf(F-1 (aq))] - [1ΔHf(CdF2 (s))]
[1(-75.9) + 2(-332.6)] - [1(-700.4)] = -40.7 kJ
-40.70 kJ     (exothermic)

Entropy Change

[1ΔSf(Cd+2 (aq)) + 2ΔSf(F-1 (aq))] - [1ΔSf(CdF2 (s))]
[1(-73.2) + 2(-13.8)] - [1(77.4)] = -178.2 J/K
-178.20 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cd+2 (aq)) + 2ΔGf(F-1 (aq))] - [1ΔGf(CdF2 (s))]
[1(-77.6) + 2(-278.8)] - [1(-647.68)] = 12.4799999999999 kJ
12.48 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

0.0065084404535
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.0065084404535) will be used to calculate the equilibrium concentration for all species.

CdF2 Cd+2 F-1
Initial M   0 0
Change -x +x +2x
Equilibrium