K (g) + 1 Br (g) → KBr (s)

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Stoichiometry

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K              Mass: g  or Gas Volume: L
Br             Mass: g  or Gas Volume: L
KBr            Mass: g

Enthalpy of Reaction

[1ΔHf(KBr (s))] - [1ΔHf(K (g)) + 1ΔHf(Br (g))]
[1(-392.17)] - [1(89.12) + 1(111.88)] = -593.17 kJ
-593.17 kJ     (exothermic)

Entropy Change

[1ΔSf(KBr (s))] - [1ΔSf(K (g)) + 1ΔSf(Br (g))]
[1(96.44)] - [1(90.04) + 1(174.91)] = -168.51 J/K
-168.51 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(KBr (s))] - [1ΔGf(K (g)) + 1ΔGf(Br (g))]
[1(-379.2)] - [1(60.67) + 1(82.43)] = -522.3 kJ
-522.30 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-542.93 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

3.2217561275e+091
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 305.

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