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

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Sr+2 (aq)) + 2ΔHf(IO3-1 (aq))] - [1ΔHf(Sr(IO3)2 (s))]
[1(-545.8) + 2(-221.33)] - [1(-1019.22)] = 30.76 kJ
30.76 kJ     (endothermic)

Entropy Change

[1ΔSf(Sr+2 (aq)) + 2ΔSf(IO3-1 (aq))] - [1ΔSf(Sr(IO3)2 (s))]
[1(-32.6) + 2(118.41)] - [1(234.3)] = -30.08 J/K
-30.08 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sr+2 (aq)) + 2ΔGf(IO3-1 (aq))] - [1ΔGf(Sr(IO3)2 (s))]
[1(-559.5) + 2(-128.03)] - [1(-855.21)] = 39.6500000000001 kJ
39.65 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

1.1304048567e-007
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.1304048567e-007) will be used to calculate the equilibrium concentration for all species.

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