AgBrO3 (s) → Ag+1 (aq) + BrO3-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Ag+1 (aq)) + 1ΔHf(BrO3-1 (aq))] - [1ΔHf(AgBrO3 (s))]
[1(105.58) + 1(-83.68)] - [1(-10.5)] = 32.4 kJ
32.40 kJ     (endothermic)

Entropy Change

[1ΔSf(Ag+1 (aq)) + 1ΔSf(BrO3-1 (aq))] - [1ΔSf(AgBrO3 (s))]
[1(72.68) + 1(163.18)] - [1(151.9)] = 83.96 J/K
83.96 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ag+1 (aq)) + 1ΔGf(BrO3-1 (aq))] - [1ΔGf(AgBrO3 (s))]
[1(77.12) + 1(1.67)] - [1(71.3)] = 7.49000000000001 kJ
7.49 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

0.048723194767
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.048723194767) will be used to calculate the equilibrium concentration for all species.

AgBrO3 Ag+1 BrO3-1
Initial M   0 0
Change -x +x +x
Equilibrium