6 Li (s) + 1 N2 (g) → 2 Li3N (s)

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Reaction Type:

Synthesis

Stoichiometry

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Li             Mass: g
N2             Mass: g  or Gas Volume: L
Li3N           Mass: g

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)

Entropy Change

[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)

8.94861452690387E+53
This process is favorable at 25°C.

Reference(s):

Atkins, Jones, and Laverman. Chemical Principles 6th ed.; W.H. Freeman and Company: New York, NY, 2013; p F94.

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