## PbCO3 (s) → Pb+2 (aq) + CO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Pb+2 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(PbCO3 (s))]
[1(-1.7) + 1(-677.14)] - [1(-699.15)] = 20.3099999999999 kJ
20.31 kJ     (endothermic)

## Entropy Change

[1ΔSf(Pb+2 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(PbCO3 (s))]
[1(10.5) + 1(-56.9)] - [1(130.96)] = -177.36 J/K
-177.36 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Pb+2 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(PbCO3 (s))]
[1(-24.4) + 1(-527.9)] - [1(-625.51)] = 73.21 kJ
73.21 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

1.4909024771e-013
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.4909024771e-013) will be used to calculate the equilibrium concentration for all species.

 PbCO3 Pb+2 CO3-2 Initial M 0 0 Change -x +x +x Equilibrium