BaI2 (s) → Ba+2 (aq) + 2 I-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(I-1 (aq))] - [1ΔHf(BaI2 (s))]
[1(-537.6) + 2(-55.19)] - [1(-605.42)] = -42.5600000000001 kJ
-42.56 kJ     (exothermic)

Entropy Change

[1ΔSf(Ba+2 (aq)) + 2ΔSf(I-1 (aq))] - [1ΔSf(BaI2 (s))]
[1(9.6) + 2(111.29)] - [1(165.14)] = 67.04 J/K
67.04 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(I-1 (aq))] - [1ΔGf(BaI2 (s))]
[1(-560.8) + 2(-51.59)] - [1(-601.41)] = -62.5700000000001 kJ
-62.57 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-62.55 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

91706409390
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (91706409390) will be used to calculate the equilibrium concentration for all species.

BaI2 Ba+2 I-1
Initial M   0 0
Change -x +x +2x
Equilibrium