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Enthalpy of Reaction
[2ΔHf(Li3N (s))] - [6ΔHf(Li (s)) + 1ΔHf(N2 (g))]
[2(-197.48)] - [6(0) + 1(0)] = -394.96 kJ
-394.96 kJ (exothermic)
[2ΔSf(Li3N (s))] - [6ΔSf(Li (s)) + 1ΔSf(N2 (g))]
[2(37.66)] - [6(29.1) + 1(191.5)] = -290.78 J/K
-290.78 J/K (decrease in entropy)
Free Energy of Reaction (at 298.15 K)
From ΔGf° values:
[2ΔGf(Li3N (s))] - [6ΔGf(Li (s)) + 1ΔGf(N2 (g))]
[2(-153.97)] - [6(0) + 1(0)] = -307.94 kJ
-307.94 kJ (spontaneous)
From ΔG = ΔH - TΔS:
-308.26 kJ (spontaneous)
Equilibrium Constant, K (at 298.15 K)
This process is favorable at 25°C.
Atkins, Jones, and Laverman. Chemical Principles 6th ed.; W.H. Freeman and Company: New York, NY, 2013; p F94.