## Ag2CO3 (s) → 2 Ag+1 (aq) + CO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[2ΔHf(Ag+1 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(Ag2CO3 (s))]
[2(105.58) + 1(-677.14)] - [1(-505.85)] = 39.87 kJ
39.87 kJ     (endothermic)

## Entropy Change

[2ΔSf(Ag+1 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(Ag2CO3 (s))]
[2(72.68) + 1(-56.9)] - [1(167.36)] = -78.9 J/K
-78.90 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Ag+1 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(Ag2CO3 (s))]
[2(77.12) + 1(-527.9)] - [1(-436.81)] = 63.15 kJ
63.15 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

8.6294487236e-012
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (8.6294487236e-012) will be used to calculate the equilibrium concentration for all species.

 Ag2CO3 Ag+1 CO3-2 Initial M 0 0 Change -x +2x +x Equilibrium