A student ran the following reaction in the laboratory at 665 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 1.57 atm and the initial partial pressure of H2 was 0.363 atm, he found that the equilibrium partial pressure of H2 was 0.357 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.
A student ran the following reaction in the laboratory at 665 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 1.57 atm and the initial partial pressure of H2 was 0.363 atm, he found that the equilibrium partial pressure of H2 was 0.357 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 90E: In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317...
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A student ran the following reaction in the laboratory at 665 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 1.57 atm and the initial partial pressure of H2 was 0.363 atm, he found that the equilibrium partial pressure of H2 was 0.357 atm.
Calculate the equilibrium constant, Kp, she obtained for this reaction.
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