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)
This process is favorable at 25°C.
Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (394418.489267529) will be used to calculate the equilibrium concentration for all species.