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) = H20(g) + CO(g) with K = 0.106 at 700 K. If a mixture of gases that initially contains 0.632 M CO, and 0.570 M H2 is allowed to equilibrate at 700 K, what is the final concentrations of CO?

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) = H20(g) + CO(g) with K = 0.106 at 700 K. If a mixture of gases that initially contains 0.632 M CO, and 0.570 M H2 is allowed to equilibrate at 700 K, what is the final concentrations of CO?

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 H, for fuel cells. This reaction can be written as follows: H:(g) - CO:(g) = H,0(g) + CO(g) with K = 0.106 at 700 K. If a mixture of gases that initially contains 0.632 M CO, and 0.570 M H, is allowed to equilibrate at 700 K, what is the final concentrations of CO? Add your answer