## K2SO4 (s) → 2 K+1 (aq) + SO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[2ΔHf(K+1 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(K2SO4 (s))]
[2(-252.4) + 1(-909.27)] - [1(-1433.69)] = 19.6200000000001 kJ
19.62 kJ     (endothermic)

## Entropy Change

[2ΔSf(K+1 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(K2SO4 (s))]
[2(102.5) + 1(20.08)] - [1(175.73)] = 49.35 J/K
49.35 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(K+1 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(K2SO4 (s))]
[2(-283.3) + 1(-744.63)] - [1(-1316.37)] = 5.13999999999987 kJ
5.14 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.12573635124
This process is close to or at equilibrium at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.12573635124) will be used to calculate the equilibrium concentration for all species.

 K2SO4 K+1 SO4-2 Initial M 0 0 Change -x +2x +x Equilibrium