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Suppose a 250. mL flask is filled with 0.40 mol of CO, 0.50 mol of CO2 and 1.0 mol of H2. The following reaction becomes possible: CO(g) + H2O(g) CO2(g) + H2(g) The equilibrium constant K for this reaction is 6.04 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. Шм G

Suppose a 250. mL flask is filled with 0.40 mol of CO, 0.50 mol of CO2 and 1.0 mol of H2. The following reaction becomes possible: CO(g) + H2O(g) CO2(g) + H2(g) The equilibrium constant K for this reaction is 6.04 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. Шм G

Chemistry
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
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Suppose a 250. mL flask is filled with 0.40 mol of CO, 0.50 mol of CO2 and 1.0 mol of H2. The following reaction becomes possible: CO(g) + H2O(g) CO2(g) + H2(g) The equilibrium constant K for this reaction is 6.04 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. Шм G
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.40 mol of CO, 0.50 mol of CO2 and 1.0 mol of H2. The following reaction becomes possible: CO(g) + H2O(g) CO2(g) + H2(g) The equilibrium constant K for this reaction is 6.04 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. Шм G
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