## CdCO3 (s) → Cd+2 (aq) + CO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Cd+2 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(CdCO3 (s))]
[1(-75.9) + 1(-677.14)] - [1(-750.61)] = -2.42999999999995 kJ
-2.43 kJ     (exothermic)

## Entropy Change

[1ΔSf(Cd+2 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(CdCO3 (s))]
[1(-73.2) + 1(-56.9)] - [1(92.47)] = -222.57 J/K
-222.57 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Cd+2 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(CdCO3 (s))]
[1(-77.6) + 1(-527.9)] - [1(-669.44)] = 63.9400000000001 kJ
63.94 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

6.2744164309e-012
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (6.2744164309e-012) will be used to calculate the equilibrium concentration for all species.

 CdCO3 Cd+2 CO3-2 Initial M 0 0 Change -x +x +x Equilibrium