K2CO3 (s) → 2 K+1 (aq) + CO3-2 (aq)

Back to reactions list

 

Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[2ΔHf(K+1 (aq)) + 1ΔHf(CO3-2 (aq))] - [1ΔHf(K2CO3 (s))]
[2(-252.4) + 1(-677.14)] - [1(-1150.18)] = -31.76 kJ
-31.76 kJ     (exothermic)

Entropy Change

[2ΔSf(K+1 (aq)) + 1ΔSf(CO3-2 (aq))] - [1ΔSf(K2CO3 (s))]
[2(102.5) + 1(-56.9)] - [1(155.52)] = -7.42000000000002 J/K
-7.42 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(K+1 (aq)) + 1ΔGf(CO3-2 (aq))] - [1ΔGf(K2CO3 (s))]
[2(-283.3) + 1(-527.9)] - [1(-1064.41)] = -30.0899999999999 kJ
-30.09 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-29.55 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

186996.4033
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (186996.4033) will be used to calculate the equilibrium concentration for all species.

K2CO3 K+1 CO3-2
Initial M   0 0
Change -x +2x +x
Equilibrium