## ZnSO4 (s) → Zn+2 (aq) + SO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Zn+2 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(ZnSO4 (s))]
[1(-153.9) + 1(-909.27)] - [1(-982.82)] = -80.35 kJ
-80.35 kJ     (exothermic)

## Entropy Change

[1ΔSf(Zn+2 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(ZnSO4 (s))]
[1(-112.1) + 1(20.08)] - [1(128.03)] = -220.05 J/K
-220.05 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Zn+2 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(ZnSO4 (s))]
[1(-147.1) + 1(-744.63)] - [1(-874.46)] = -17.27 kJ
-17.27 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-14.74 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1061.063687
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1061.063687) will be used to calculate the equilibrium concentration for all species.

 ZnSO4 Zn+2 SO4-2 Initial M 0 0 Change -x +x +x Equilibrium