Hg2Cl2 (s) → Hg2+2 (aq) + 2 Cl-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Hg2+2 (aq)) + 2ΔHf(Cl-1 (aq))] - [1ΔHf(Hg2Cl2 (s))]
[1(172.4) + 2(-167.15)] - [1(-265.22)] = 103.32 kJ
103.32 kJ     (endothermic)

Entropy Change

[1ΔSf(Hg2+2 (aq)) + 2ΔSf(Cl-1 (aq))] - [1ΔSf(Hg2Cl2 (s))]
[1(84.5) + 2(56.48)] - [1(192.46)] = 4.99999999999997 J/K
5.00 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Hg2+2 (aq)) + 2ΔGf(Cl-1 (aq))] - [1ΔGf(Hg2Cl2 (s))]
[1(153.5) + 2(-131.25)] - [1(-210.78)] = 101.78 kJ
101.78 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

1.47205243241425E-18
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.47205243241425E-18) will be used to calculate the equilibrium concentration for all species.

Hg2Cl2 Hg2+2 Cl-1
Initial M   0 0
Change -x +x +2x
Equilibrium