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Enthalpy of Reaction
[1ΔHf(CaF2 (s))] - [1ΔHf(Ca (s)) + 1ΔHf(F2 (g))]
[1(-1219.64)] - [1(0) + 1(0)] = -1219.64 kJ
-1,219.64 kJ (exothermic)
[1ΔSf(CaF2 (s))] - [1ΔSf(Ca (s)) + 1ΔSf(F2 (g))]
[1(68.87)] - [1(41.42) + 1(202.71)] = -175.26 J/K
-175.26 J/K (decrease in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(CaF2 (s))] - [1ΔGf(Ca (s)) + 1ΔGf(F2 (g))]
[1(-1167.34)] - [1(0) + 1(0)] = -1167.34 kJ
-1,167.34 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-1167.39 kJ (spontaneous)
Equilibrium Constant, K (at 298.15 K)
This process is favorable at 25°C.
Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 91.