## Mn(IO3)2 (s) → Mn+2 (aq) + 2 IO3-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Mn+2 (aq)) + 2ΔHf(IO3-1 (aq))] - [1ΔHf(Mn(IO3)2 (s))]
[1(-220.83) + 2(-221.33)] - [1(-669.44)] = 5.95000000000005 kJ
5.95 kJ     (endothermic)

## Entropy Change

[1ΔSf(Mn+2 (aq)) + 2ΔSf(IO3-1 (aq))] - [1ΔSf(Mn(IO3)2 (s))]
[1(-73.64) + 2(118.41)] - [1(263.59)] = -100.41 J/K
-100.41 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Mn+2 (aq)) + 2ΔGf(IO3-1 (aq))] - [1ΔGf(Mn(IO3)2 (s))]
[1(-228.03) + 2(-128.03)] - [1(-520.49)] = 36.4 kJ
36.40 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

4.1941220339e-007
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (4.1941220339e-007) will be used to calculate the equilibrium concentration for all species.

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