## PbSeO4 (s) → Pb+2 (aq) + SeO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Pb+2 (aq)) + 1ΔHf(SeO4-2 (aq))] - [1ΔHf(PbSeO4 (s))]
[1(-1.7) + 1(-599.15)] - [1(-609.19)] = 8.34000000000003 kJ
8.34 kJ     (endothermic)

## Entropy Change

[1ΔSf(Pb+2 (aq)) + 1ΔSf(SeO4-2 (aq))] - [1ΔSf(PbSeO4 (s))]
[1(10.5) + 1(53.97)] - [1(167.78)] = -103.31 J/K
-103.31 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Pb+2 (aq)) + 1ΔGf(SeO4-2 (aq))] - [1ΔGf(PbSeO4 (s))]
[1(-24.4) + 1(-441.41)] - [1(-505.01)] = 39.2 kJ
39.20 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

1.3554234362e-007
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.3554234362e-007) will be used to calculate the equilibrium concentration for all species.

 PbSeO4 Pb+2 SeO4-2 Initial M 0 0 Change -x +x +x Equilibrium