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Suppose a 500. mL flask is filled with 1.2 mol of H2O, 0.50 mol of CO2 and 1.8 mol of H₂. The following reaction becomes possible: CO(g)+H2O(g) CO2(g) + H2(g) L The equilibrium constant K for this reaction is 0.876 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐ □ M

Suppose a 500. mL flask is filled with 1.2 mol of H2O, 0.50 mol of CO2 and 1.8 mol of H₂. The following reaction becomes possible: CO(g)+H2O(g) CO2(g) + H2(g) L The equilibrium constant K for this reaction is 0.876 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐ □ M

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Suppose a 500. mL flask is filled with 1.2 mol of H2O, 0.50 mol of CO2 and 1.8 mol of H₂. The following reaction becomes possible: CO(g)+H2O(g) CO2(g) + H2(g) L The equilibrium constant K for this reaction is 0.876 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐ □ M
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.2 mol of H2O, 0.50 mol of CO2 and 1.8 mol of H₂. The following reaction becomes possible: CO(g)+H2O(g) CO2(g) + H2(g) L The equilibrium constant K for this reaction is 0.876 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐ □ M
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