## Ag2SO4 (s) → 2 Ag+1 (aq) + SO4-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[2ΔHf(Ag+1 (aq)) + 1ΔHf(SO4-2 (aq))] - [1ΔHf(Ag2SO4 (s))]
[2(105.58) + 1(-909.27)] - [1(-715.88)] = 17.77 kJ
17.77 kJ     (endothermic)

## Entropy Change

[2ΔSf(Ag+1 (aq)) + 1ΔSf(SO4-2 (aq))] - [1ΔSf(Ag2SO4 (s))]
[2(72.68) + 1(20.08)] - [1(200.41)] = -34.97 J/K
-34.97 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Ag+1 (aq)) + 1ΔGf(SO4-2 (aq))] - [1ΔGf(Ag2SO4 (s))]
[2(77.12) + 1(-744.63)] - [1(-618.48)] = 28.09 kJ
28.09 kJ     (nonspontaneous)

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

1.1983152433e-005
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.1983152433e-005) will be used to calculate the equilibrium concentration for all species.

 Ag2SO4 Ag+1 SO4-2 Initial M 0 0 Change -x +2x +x Equilibrium