KMnO4 (s) → K+1 (aq) + MnO4-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(K+1 (aq)) + 1ΔHf(MnO4-1 (aq))] - [1ΔHf(KMnO4 (s))]
[1(-252.4) + 1(-541.41)] - [1(-813.37)] = 19.5600000000001 kJ
19.56 kJ     (endothermic)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(K+1 (aq)) + 1ΔGf(MnO4-1 (aq))] - [1ΔGf(KMnO4 (s))]
[1(-283.3) + 1(-447.27)] - [1(-713.79)] = -16.78 kJ
-16.78 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-16.81 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

870.747806733599
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (870.747806733599) will be used to calculate the equilibrium concentration for all species.

KMnO4 K+1 MnO4-1
Initial M   0 0
Change -x +x +x
Equilibrium

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 226.

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