KClO3 (s) → K+1 (aq) + ClO3-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(K+1 (aq)) + 1ΔHf(ClO3-1 (aq))] - [1ΔHf(KClO3 (s))]
[1(-252.4) + 1(-99.16)] - [1(-391.2)] = 39.64 kJ
39.64 kJ     (endothermic)

Entropy Change

[1ΔSf(K+1 (aq)) + 1ΔSf(ClO3-1 (aq))] - [1ΔSf(KClO3 (s))]
[1(102.5) + 1(162.34)] - [1(142.97)] = 121.87 J/K
121.87 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(K+1 (aq)) + 1ΔGf(ClO3-1 (aq))] - [1ΔGf(KClO3 (s))]
[1(-283.3) + 1(-3.35)] - [1(-289.91)] = 3.25999999999999 kJ
3.26 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

0.26843610608
This process is close to or at equilibrium at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.26843610608) will be used to calculate the equilibrium concentration for all species.

KClO3 K+1 ClO3-1
Initial M   0 0
Change -x +x +x
Equilibrium