## La(IO3)3 (s) → La+3 (aq) + 3 IO3-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(La+3 (aq)) + 3ΔHf(IO3-1 (aq))] - [1ΔHf(La(IO3)3 (s))]
[1(-707.1) + 3(-221.33)] - [1(-1397.46)] = 26.3699999999999 kJ
26.37 kJ     (endothermic)

## Entropy Change

[1ΔSf(La+3 (aq)) + 3ΔSf(IO3-1 (aq))] - [1ΔSf(La(IO3)3 (s))]
[1(-217.57) + 3(118.41)] - [1(259.41)] = -121.75 J/K
-121.75 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(La+3 (aq)) + 3ΔGf(IO3-1 (aq))] - [1ΔGf(La(IO3)3 (s))]
[1(-683.67) + 3(-128.03)] - [1(-1131.35)] = 63.5899999999999 kJ
63.59 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

7.2259357937e-012
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (7.2259357937e-012) will be used to calculate the equilibrium concentration for all species.

 La(IO3)3 La+3 IO3-1 Initial M 0 0 Change -x +x +3x Equilibrium