ZnF2 (s) → Zn+2 (aq) + 2 F-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Zn+2 (aq)) + 2ΔHf(F-1 (aq))] - [1ΔHf(ZnF2 (s))]
[1(-153.9) + 2(-332.6)] - [1(-764.42)] = -54.6800000000001 kJ
-54.68 kJ     (exothermic)

Entropy Change

[1ΔSf(Zn+2 (aq)) + 2ΔSf(F-1 (aq))] - [1ΔSf(ZnF2 (s))]
[1(-112.1) + 2(-13.8)] - [1(73.68)] = -213.38 J/K
-213.38 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Zn+2 (aq)) + 2ΔGf(F-1 (aq))] - [1ΔGf(ZnF2 (s))]
[1(-147.1) + 2(-278.8)] - [1(-713.37)] = 8.66999999999996 kJ
8.67 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

3.02689390025789E-02
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (3.02689390025789E-02) will be used to calculate the equilibrium concentration for all species.

ZnF2 Zn+2 F-1
Initial M   0 0
Change -x +x +2x
Equilibrium