## AgI (s) → Ag+1 (aq) + I-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ag+1 (aq)) + 1ΔHf(I-1 (aq))] - [1ΔHf(AgI (s))]
[1(105.58) + 1(-55.19)] - [1(-61.84)] = 112.23 kJ
112.23 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ag+1 (aq)) + 1ΔSf(I-1 (aq))] - [1ΔSf(AgI (s))]
[1(72.68) + 1(111.29)] - [1(115.48)] = 68.49 J/K
68.49 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ag+1 (aq)) + 1ΔGf(I-1 (aq))] - [1ΔGf(AgI (s))]
[1(77.12) + 1(-51.59)] - [1(-66.19)] = 91.72 kJ
91.72 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
91.81 kJ     (nonspontaneous) ## Equilibrium Constant, K (at 298.15 K)

8.520343335e-017
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (8.520343335e-017) will be used to calculate the equilibrium concentration for all species.

 AgI Ag+1 I-1 Initial M 0 0 Change -x +x +x Equilibrium