SrI2 (s) → Sr+2 (aq) + 2 I-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Sr+2 (aq)) + 2ΔHf(I-1 (aq))] - [1ΔHf(SrI2 (s))]
[1(-545.8) + 2(-55.19)] - [1(-561.49)] = -94.6899999999999 kJ
-94.69 kJ     (exothermic)

Entropy Change

[1ΔSf(Sr+2 (aq)) + 2ΔSf(I-1 (aq))] - [1ΔSf(SrI2 (s))]
[1(-32.6) + 2(111.29)] - [1(159.12)] = 30.86 J/K
30.86 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sr+2 (aq)) + 2ΔGf(I-1 (aq))] - [1ΔGf(SrI2 (s))]
[1(-559.5) + 2(-51.59)] - [1(-558.73)] = -103.95 kJ
-103.95 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-103.89 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.6302921097e+018
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (1.6302921097e+018) will be used to calculate the equilibrium concentration for all species.

SrI2 Sr+2 I-1
Initial M   0 0
Change -x +x +2x
Equilibrium