## BaCrO4 (s) → Ba+2 (aq) + CrO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 1ΔHf(CrO4-2 (aq))] - [1ΔHf(BaCrO4 (s))]
[1(-537.6) + 1(-881.15)] - [1(-1445.99)] = 27.24 kJ
27.24 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ba+2 (aq)) + 1ΔSf(CrO4-2 (aq))] - [1ΔSf(BaCrO4 (s))]
[1(9.6) + 1(50.21)] - [1(158.57)] = -98.76 J/K
-98.76 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 1ΔGf(CrO4-2 (aq))] - [1ΔGf(BaCrO4 (s))]
[1(-560.8) + 1(-727.85)] - [1(-1345.28)] = 56.6299999999999 kJ
56.63 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

1.1975707824e-010
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.1975707824e-010) will be used to calculate the equilibrium concentration for all species.

 BaCrO4 Ba+2 CrO4-2 Initial M 0 0 Change -x +x +x Equilibrium