## ZnCO3 (s) → Zn+2 (aq) + CO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Zn+2 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(ZnCO3 (s))]
[1(-153.9) + 1(-677.14)] - [1(-812.78)] = -18.26 kJ
-18.26 kJ     (exothermic)

## Entropy Change

[1ΔSf(Zn+2 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(ZnCO3 (s))]
[1(-112.1) + 1(-56.9)] - [1(82.42)] = -251.42 J/K
-251.42 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Zn+2 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(ZnCO3 (s))]
[1(-147.1) + 1(-527.9)] - [1(-731.57)] = 56.5700000000001 kJ
56.57 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

1.2269117394e-010
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.2269117394e-010) will be used to calculate the equilibrium concentration for all species.

 ZnCO3 Zn+2 CO3-2 Initial M 0 0 Change -x +x +x Equilibrium