## Ba(NO3)2 (s) → Ba+2 (aq) + 2 NO3-1 (aq)

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## Reaction Type:

Dissociation of an ionic compound in water

## Enthalpy of Reaction

[1ΔHf(Ba+2 (aq)) + 2ΔHf(NO3-1 (aq))] - [1ΔHf(Ba(NO3)2 (s))]
[1(-537.6) + 2(-207.36)] - [1(-992.07)] = 39.75 kJ
39.75 kJ     (endothermic)

## Entropy Change

[1ΔSf(Ba+2 (aq)) + 2ΔSf(NO3-1 (aq))] - [1ΔSf(Ba(NO3)2 (s))]
[1(9.6) + 2(146.44)] - [1(213.8)] = 88.68 J/K
88.68 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Ba+2 (aq)) + 2ΔGf(NO3-1 (aq))] - [1ΔGf(Ba(NO3)2 (s))]
[1(-560.8) + 2(-111.34)] - [1(-796.72)] = 13.24 kJ
13.24 kJ     (nonspontaneous)

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

## Equilibrium Constant, K (at 298.15 K)

0.0047898651593
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (0.0047898651593) will be used to calculate the equilibrium concentration for all species.

 Ba(NO3)2 Ba+2 NO3-1 Initial M 0 0 Change -x +x +2x Equilibrium