## PbSO4 (s) → Pb+2 (aq) + SO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Pb+2 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(PbSO4 (s))]
[1(-1.7) + 1(-909.27)] - [1(-919.94)] = 8.97000000000003 kJ
8.97 kJ     (endothermic)

## Entropy Change

[1ΔSf(Pb+2 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(PbSO4 (s))]
[1(10.5) + 1(20.08)] - [1(148.57)] = -117.99 J/K
-117.99 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Pb+2 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(PbSO4 (s))]
[1(-24.4) + 1(-744.63)] - [1(-813.2)] = 44.1700000000001 kJ
44.17 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

1.8252409873e-008
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.8252409873e-008) will be used to calculate the equilibrium concentration for all species.

 PbSO4 Pb+2 SO4-2 Initial M 0 0 Change -x +x +x Equilibrium