Ag2C2O4 (s) → 2 Ag+1 (aq) + C2O4-2 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[2ΔHf(Ag+1 (aq)) + 1ΔHf(C2O4-2 (aq))] - [1ΔHf(Ag2C2O4 (s))]
[2(105.58) + 1(-825.1)] - [1(-673.21)] = 59.27 kJ
59.27 kJ     (endothermic)

Entropy Change

[2ΔSf(Ag+1 (aq)) + 1ΔSf(C2O4-2 (aq))] - [1ΔSf(Ag2C2O4 (s))]
[2(72.68) + 1(45.6)] - [1(209.2)] = -18.24 J/K
-18.24 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Ag+1 (aq)) + 1ΔGf(C2O4-2 (aq))] - [1ΔGf(Ag2C2O4 (s))]
[2(77.12) + 1(-673.9)] - [1(-584.09)] = 64.4300000000001 kJ
64.43 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

5.1490164189e-012
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (5.1490164189e-012) will be used to calculate the equilibrium concentration for all species.

 Ag2C2O4 Ag+1 C2O4-2 Initial M 0 0 Change -x +2x +x Equilibrium