AgCl (s) → Ag+1 (aq) + Cl-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ag+1 (aq)) + 1ΔHf(Cl-1 (aq))] - [1ΔHf(AgCl (s))]
[1(105.58) + 1(-167.15)] - [1(-127)] = 65.43 kJ
65.43 kJ     (endothermic)

Entropy Change

[1ΔSf(Ag+1 (aq)) + 1ΔSf(Cl-1 (aq))] - [1ΔSf(AgCl (s))]
[1(72.68) + 1(56.48)] - [1(96.3)] = 32.86 J/K
32.86 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ag+1 (aq)) + 1ΔGf(Cl-1 (aq))] - [1ΔGf(AgCl (s))]
[1(77.12) + 1(-131.25)] - [1(-109.8)] = 55.67 kJ
55.67 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

1.76398656732089E-10
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.76398656732089E-10) will be used to calculate the equilibrium concentration for all species.

AgCl Ag+1 Cl-1
Initial M   0 0
Change -x +x +x
Equilibrium