AgBr (s) → Ag+1 (aq) + Br-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ag+1 (aq)) + 1ΔHf(Br-1 (aq))] - [1ΔHf(AgBr (s))]
[1(105.58) + 1(-121.55)] - [1(-100.37)] = 84.4 kJ
84.40 kJ     (endothermic)

Entropy Change

[1ΔSf(Ag+1 (aq)) + 1ΔSf(Br-1 (aq))] - [1ΔSf(AgBr (s))]
[1(72.68) + 1(82.42)] - [1(107.11)] = 47.99 J/K
47.99 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ag+1 (aq)) + 1ΔGf(Br-1 (aq))] - [1ΔGf(AgBr (s))]
[1(77.12) + 1(-103.97)] - [1(-96.9)] = 70.05 kJ
70.05 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

5.33443084205409E-13
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (5.33443084205409E-13) will be used to calculate the equilibrium concentration for all species.

AgBr Ag+1 Br-1
Initial M   0 0
Change -x +x +x
Equilibrium