## KClO4 (s) → K+1 (aq) + ClO4-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(K+1 (aq)) + 1ΔHf(ClO4-1 (aq))] - [1ΔHf(KClO4 (s))]
[1(-252.4) + 1(-129.33)] - [1(-430.12)] = 48.39 kJ
48.39 kJ     (endothermic)

## Entropy Change

[1ΔSf(K+1 (aq)) + 1ΔSf(ClO4-1 (aq))] - [1ΔSf(KClO4 (s))]
[1(102.5) + 1(182)] - [1(151.04)] = 133.46 J/K
133.46 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(K+1 (aq)) + 1ΔGf(ClO4-1 (aq))] - [1ΔGf(KClO4 (s))]
[1(-283.3) + 1(-8.62)] - [1(-300.41)] = 8.49000000000001 kJ
8.49 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.032548695583
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.032548695583) will be used to calculate the equilibrium concentration for all species.

 KClO4 K+1 ClO4-1 Initial M 0 0 Change -x +x +x Equilibrium