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Use the free energies of formation to calculate the equilibrium constant (K) for the following reaction at 298 K. N2(g) + 3 H2(g) → 2 NH3(g) K = ? ΔG°f (kJ/mol).   0.0 0.0 -16.4 Select one: a. 1.78 x 10-6 b. 1.52×10-6 c. 5.62×105 d. 749 e. 1.33×10-3

Use the free energies of formation to calculate the equilibrium constant (K) for the following reaction at 298 K. N2(g) + 3 H2(g) → 2 NH3(g) K = ? ΔG°f (kJ/mol).   0.0 0.0 -16.4 Select one: a. 1.78 x 10-6 b. 1.52×10-6 c. 5.62×105 d. 749 e. 1.33×10-3

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 16P
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Use the free energies of formation to calculate the equilibrium constant (K) for the following reaction at 298 K.

N2(g) + 3 H2(g) → 2 NH3(g) K = ?
ΔG°f (kJ/mol).   0.0 0.0 -16.4

Select one:

a.
1.78 x 10-6

b.
1.52×10-6

c.
5.62×105

d.
749

e.
1.33×10-3 

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