Ni(IO3)2 (s) → Ni+2 (aq) + 2 IO3-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ni+2 (aq)) + 2ΔHf(IO3-1 (aq))] - [1ΔHf(Ni(IO3)2 (s))]
[1(-53.97) + 2(-221.33)] - [1(-489.11)] = -7.51999999999998 kJ
-7.52 kJ     (exothermic)

Entropy Change

[1ΔSf(Ni+2 (aq)) + 2ΔSf(IO3-1 (aq))] - [1ΔSf(Ni(IO3)2 (s))]
[1(-128.87) + 2(118.41)] - [1(213.38)] = -105.43 J/K
-105.43 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ni+2 (aq)) + 2ΔGf(IO3-1 (aq))] - [1ΔGf(Ni(IO3)2 (s))]
[1(-45.61) + 2(-128.03)] - [1(-326.35)] = 24.68 kJ
24.68 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

4.7425342805516E-05
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (4.7425342805516E-05) will be used to calculate the equilibrium concentration for all species.

Ni(IO3)2 Ni+2 IO3-1
Initial M   0 0
Change -x +x +2x
Equilibrium