Ca (s) + 1 F2 (g) → CaF2 (s)

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Reaction Type:

Synthesis

Stoichiometry

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Ca             Mass: g
F2             Mass: g  or Gas Volume: L
CaF2           Mass: g
Heat Released: kJ

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)

Entropy Change

[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)

3.3151218901e+204
This process is favorable at 25°C.

Reference(s):

Swaddle, T.W. Inorganic Chemistry; Academic Press: San Diego, 1997; p 91.

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