BaBr2 (s) → Ba+2 (aq) + 2 Br-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(Br-1 (aq))] - [1ΔHf(BaBr2 (s))]
[1(-537.6) + 2(-121.55)] - [1(-757.3)] = -23.4000000000001 kJ
-23.40 kJ     (exothermic)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(Br-1 (aq))] - [1ΔGf(BaBr2 (s))]
[1(-560.8) + 2(-103.97)] - [1(-736.8)] = -31.9400000000001 kJ
-31.94 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-31.75 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

394418.48927
This process is favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (394418.48927) will be used to calculate the equilibrium concentration for all species.

BaBr2 Ba+2 Br-1
Initial M   0 0
Change -x +x +2x
Equilibrium