ScF3 (s) → Sc+3 (aq) + 3 F-1 (aq)

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Reaction Type:

Dissociation of an ionic compound in water

Enthalpy of Reaction

[1ΔHf(Sc+3 (aq)) + 3ΔHf(F-1 (aq))] - [1ΔHf(ScF3 (s))]
[1(-614.21) + 3(-332.6)] - [1(-1629.25)] = 17.2399999999998 kJ
17.24 kJ     (endothermic)

Entropy Change

[1ΔSf(Sc+3 (aq)) + 3ΔSf(F-1 (aq))] - [1ΔSf(ScF3 (s))]
[1(-255.22) + 3(-13.8)] - [1(92.05)] = -388.67 J/K
-388.67 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Sc+3 (aq)) + 3ΔGf(F-1 (aq))] - [1ΔGf(ScF3 (s))]
[1(-586.6) + 3(-278.8)] - [1(-1555.61)] = 132.61 kJ
132.61 kJ     (nonspontaneous)

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

Equilibrium Constant, K (at 298.15 K)

5.84037080172052E-24
This process is not favorable at 25°C.

Enter an initial concentration for the ionic compound. Upon hitting submit, Ksp (5.84037080172052E-24) will be used to calculate the equilibrium concentration for all species.

ScF3 Sc+3 F-1
Initial M   0 0
Change -x +x +3x
Equilibrium