## Ag2SO3 (s) → 2 Ag+1 (aq) + SO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[2ΔHf(Ag+1 (aq)) + 1ΔHf(SO3-2 (aq))] - [1ΔHf(Ag2SO3 (s))]
[2(105.58) + 1(-635.55)] - [1(-490.78)] = 66.39 kJ
66.39 kJ     (endothermic)

## Entropy Change

[2ΔSf(Ag+1 (aq)) + 1ΔSf(SO3-2 (aq))] - [1ΔSf(Ag2SO3 (s))]
[2(72.68) + 1(-29.29)] - [1(158.16)] = -42.09 J/K
-42.09 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Ag+1 (aq)) + 1ΔGf(SO3-2 (aq))] - [1ΔGf(Ag2SO3 (s))]
[2(77.12) + 1(-486.6)] - [1(-411.29)] = 78.93 kJ
78.93 kJ     (nonspontaneous)

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

1.4835180402e-014
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.4835180402e-014) will be used to calculate the equilibrium concentration for all species.

 Ag2SO3 Ag+1 SO3-2 Initial M 0 0 Change -x +2x +x Equilibrium