## Li2CO3 (s) → 2 Li+1 (aq) + CO3-2 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[2ΔHf(Li+1 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(Li2CO3 (s))]
[2(-278.5) + 1(-677.14)] - [1(-1216.04)] = -18.0999999999999 kJ
-18.10 kJ     (exothermic)

## Entropy Change

[2ΔSf(Li+1 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(Li2CO3 (s))]
[2(13.4) + 1(-56.9)] - [1(90.17)] = -120.27 J/K
-120.27 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(Li+1 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(Li2CO3 (s))]
[2(-293.3) + 1(-527.9)] - [1(-1132.19)] = 17.6900000000001 kJ
17.69 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.00079556127911
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.00079556127911) will be used to calculate the equilibrium concentration for all species.

 Li2CO3 Li+1 CO3-2 Initial M 0 0 Change -x +2x +x Equilibrium