## Ba(BrO3)2 (s) → Ba+2 (aq) + 2 BrO3-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(BrO3-1 (aq))] - [1ΔHf(Ba(BrO3)2 (s))]
[1(-537.6) + 2(-83.68)] - [1(-752.66)] = 47.6999999999999 kJ
47.70 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ba+2 (aq)) + 2ΔSf(BrO3-1 (aq))] - [1ΔSf(Ba(BrO3)2 (s))]
[1(9.6) + 2(163.18)] - [1(242.67)] = 93.29 J/K
93.29 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(BrO3-1 (aq))] - [1ΔGf(Ba(BrO3)2 (s))]
[1(-560.8) + 2(1.67)] - [1(-577.39)] = 19.9300000000001 kJ
19.93 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.00032227066829
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.00032227066829) will be used to calculate the equilibrium concentration for all species.

 Ba(BrO3)2 Ba+2 BrO3-1 Initial M 0 0 Change -x +x +2x Equilibrium