N2(g) + 3H2(g) 2NH3(g) When he introduced N2(g) and H2(g) into a 1.00 L evacuated container, so that the initial partial pressure of N2 was 1.16 atm and the initial partial pressure of H2 was 0.476 atm, he found that the equilibrium partial pressure of NH3 was 6.22×10-3 atm. Calculate the equilibrium constant, Kp,
N2(g) + 3H2(g) 2NH3(g) When he introduced N2(g) and H2(g) into a 1.00 L evacuated container, so that the initial partial pressure of N2 was 1.16 atm and the initial partial pressure of H2 was 0.476 atm, he found that the equilibrium partial pressure of NH3 was 6.22×10-3 atm. Calculate the equilibrium constant, Kp,
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 33P
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Question
A student ran the following reaction in the laboratory at 653 K:
N2(g) + 3H2(g) 2NH3(g)
When he introduced N2(g) and H2(g) into a 1.00 L evacuated container, so that the initial partial pressure of N2 was 1.16 atm and the initial partial pressure of H2 was 0.476 atm, he found that the equilibrium partial pressure of NH3 was 6.22×10-3 atm.
Calculate the equilibrium constant, Kp, he obtained for this reaction.
Kp =
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