0.1 mole of H2(g) and 0.2 mole of CO2(g) are introduced into an evacuated flask at 450oC and the reaction H2(g) + CO2 (g) = H2O(g) + CO(g) occurs to give an equilibrium pressure of 0.507 bar. Analysis of the mixture shows that it contains 10 mole % water. Calculate the equilibrium constant Kp. Answer: [0.0757]
0.1 mole of H2(g) and 0.2 mole of CO2(g) are introduced into an evacuated flask at 450oC and the reaction H2(g) + CO2 (g) = H2O(g) + CO(g) occurs to give an equilibrium pressure of 0.507 bar. Analysis of the mixture shows that it contains 10 mole % water. Calculate the equilibrium constant Kp. Answer: [0.0757]
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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0.1 mole of H2(g) and 0.2 mole of CO2(g) are introduced into an evacuated flask at 450oC and the reaction
H2(g) + CO2 (g) = H2O(g) + CO(g)
occurs to give an equilibrium pressure of 0.507 bar. Analysis of the mixture shows that it contains 10 mole % water. Calculate the equilibrium constant Kp.
Answer: [0.0757]
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