## SrSO4 (s) → Sr+2 (aq) + SO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Sr+2 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(SrSO4 (s))]
[1(-545.8) + 1(-909.27)] - [1(-1453.1)] = -1.97000000000003 kJ
-1.97 kJ     (exothermic)

## Entropy Change

[1ΔSf(Sr+2 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(SrSO4 (s))]
[1(-32.6) + 1(20.08)] - [1(117.57)] = -130.09 J/K
-130.09 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sr+2 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(SrSO4 (s))]
[1(-559.5) + 1(-744.63)] - [1(-1340.97)] = 36.8399999999999 kJ
36.84 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

3.5119806026e-007
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (3.5119806026e-007) will be used to calculate the equilibrium concentration for all species.

 SrSO4 Sr+2 SO4-2 Initial M 0 0 Change -x +x +x Equilibrium