## Hg2CO3 (s) → Hg2+2 (aq) + CO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Hg2+2 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(Hg2CO3 (s))]
[1(172.4) + 1(-677.14)] - [1(-553.54)] = 48.8 kJ
48.80 kJ     (endothermic)

## Entropy Change

[1ΔSf(Hg2+2 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(Hg2CO3 (s))]
[1(84.5) + 1(-56.9)] - [1(179.91)] = -152.31 J/K
-152.31 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Hg2+2 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(Hg2CO3 (s))]
[1(153.5) + 1(-527.9)] - [1(-468.19)] = 93.79 kJ
93.79 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

3.6964820907e-017
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (3.6964820907e-017) will be used to calculate the equilibrium concentration for all species.

 Hg2CO3 Hg2+2 CO3-2 Initial M 0 0 Change -x +x +x Equilibrium