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Enthalpy of Reaction
[1ΔHf(UF6 (s))] - [1ΔHf(UF4 (s)) + 1ΔHf(F2 (g))]
[1(-2197)] - [1(-1853.51) + 1(0)] = -343.49 kJ
-343.49 kJ (exothermic)
[1ΔSf(UF6 (s))] - [1ΔSf(UF4 (s)) + 1ΔSf(F2 (g))]
[1(227.6)] - [1(151.04) + 1(202.71)] = -126.15 J/K
-126.15 J/K (decrease in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[1ΔGf(UF6 (s))] - [1ΔGf(UF4 (s)) + 1ΔGf(F2 (g))]
[1(-2068.5)] - [1(-1761.46) + 1(0)] = -307.04 kJ
-307.04 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-305.88 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 230.