Hg2SO4 (s) → Hg2+2 (aq) + SO4-2 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Hg2+2 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(Hg2SO4 (s))]
[1(172.4) + 1(-909.27)] - [1(-743.12)] = 6.25 kJ
6.25 kJ     (endothermic)

Entropy Change

[1ΔSf(Hg2+2 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(Hg2SO4 (s))]
[1(84.5) + 1(20.08)] - [1(200.66)] = -96.08 J/K
-96.08 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Hg2+2 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(Hg2SO4 (s))]
[1(153.5) + 1(-744.63)] - [1(-625.88)] = 34.75 kJ
34.75 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

8.1606479144617E-07
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (8.1606479144617E-07) will be used to calculate the equilibrium concentration for all species.

Hg2SO4 Hg2+2 SO4-2
Initial M   0 0
Change -x +x +x
Equilibrium