## Hg2F2 (s) → Hg2+2 (aq) + 2 F-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Hg2+2 (aq)) + 2ΔHf(F-1 (aq))] - [1ΔHf(Hg2F2 (s))]
[1(172.4) + 2(-332.6)] - [1(-485.34)] = -7.46000000000009 kJ
-7.46 kJ     (exothermic)

## Entropy Change

[1ΔSf(Hg2+2 (aq)) + 2ΔSf(F-1 (aq))] - [1ΔSf(Hg2F2 (s))]
[1(84.5) + 2(-13.8)] - [1(158.99)] = -102.09 J/K
-102.09 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Hg2+2 (aq)) + 2ΔGf(F-1 (aq))] - [1ΔGf(Hg2F2 (s))]
[1(153.5) + 2(-278.8)] - [1(-426.77)] = 22.67 kJ
22.67 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.00010670059414
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.00010670059414) will be used to calculate the equilibrium concentration for all species.

 Hg2F2 Hg2+2 F-1 Initial M 0 0 Change -x +x +2x Equilibrium