processes, such as the production of H2 for fuel cells. This reaction can be written as follows: H2(g)+CO2(g)⇌H2O(g)+CO(g)H2(g)+CO2(g)⇌H2O(g)+CO(g) K = 0.106 at 700 K. If a mixture of gases that initially contains 0.0150 M H2 and 0.0150 M CO2 is allowed to equilibrate at 700 K, what are the final concentrations of all substances present?
processes, such as the production of H2 for fuel cells. This reaction can be written as follows: H2(g)+CO2(g)⇌H2O(g)+CO(g)H2(g)+CO2(g)⇌H2O(g)+CO(g) K = 0.106 at 700 K. If a mixture of gases that initially contains 0.0150 M H2 and 0.0150 M CO2 is allowed to equilibrate at 700 K, what are the final concentrations of all substances present?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The water–gas shift reaction is important in several chemical processes, such as the production of H2 for fuel cells. This reaction can be written as follows:
H2(g)+CO2(g)⇌H2O(g)+CO(g)H2(g)+CO2(g)⇌H2O(g)+CO(g)
K = 0.106 at 700 K. If a mixture of gases that initially contains 0.0150 M H2 and 0.0150 M CO2 is allowed to equilibrate at 700 K, what are the final concentrations of all substances present?
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