BaCl2 (s) → Ba+2 (aq) + 2 Cl-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(Cl-1 (aq))] - [1ΔHf(BaCl2 (s))]
[1(-537.6) + 2(-167.15)] - [1(-858.14)] = -13.7600000000001 kJ
-13.76 kJ     (exothermic)

Entropy Change

[1ΔSf(Ba+2 (aq)) + 2ΔSf(Cl-1 (aq))] - [1ΔSf(BaCl2 (s))]
[1(9.6) + 2(56.48)] - [1(123.68)] = -1.12000000000002 J/K
-1.12 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(Cl-1 (aq))] - [1ΔGf(BaCl2 (s))]
[1(-560.8) + 2(-131.25)] - [1(-810.44)] = -12.8599999999999 kJ
-12.86 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-13.43 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

179.101774301069
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (179.101774301069) will be used to calculate the equilibrium concentration for all species.

BaCl2 Ba+2 Cl-1
Initial M   0 0
Change -x +x +2x
Equilibrium