## BaSeO4 (s) → Ba+2 (aq) + SeO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 1ΔHf(SeO4-2 (aq))] - [1ΔHf(BaSeO4 (s))]
[1(-537.6) + 1(-599.15)] - [1(-1146.42)] = 9.67000000000007 kJ
9.67 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ba+2 (aq)) + 1ΔSf(SeO4-2 (aq))] - [1ΔSf(BaSeO4 (s))]
[1(9.6) + 1(53.97)] - [1(175.73)] = -112.16 J/K
-112.16 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 1ΔGf(SeO4-2 (aq))] - [1ΔGf(BaSeO4 (s))]
[1(-560.8) + 1(-441.41)] - [1(-1044.74)] = 42.53 kJ
42.53 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

3.5371360876e-008
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (3.5371360876e-008) will be used to calculate the equilibrium concentration for all species.

 BaSeO4 Ba+2 SeO4-2 Initial M 0 0 Change -x +x +x Equilibrium