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Suppose a 500. ml flask is filled with 0.90 mol of CO, 1.8 mol of CO₂ and 0.50 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂(g) + H₂(g) 1 The equilibrium constant K for this reaction is 0.831 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M 5

Suppose a 500. ml flask is filled with 0.90 mol of CO, 1.8 mol of CO₂ and 0.50 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂(g) + H₂(g) 1 The equilibrium constant K for this reaction is 0.831 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M 5

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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Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 0.90 mol of CO, 1.8 mol of CO₂ and 0.50 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.831 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M
Transcribed Image Text:Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 0.90 mol of CO, 1.8 mol of CO₂ and 0.50 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.831 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M
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