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Suppose a 500. mL flask is filled with 0.90 mol of CO, 1.3 mol of NO and 0.70 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.576 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M

Suppose a 500. mL flask is filled with 0.90 mol of CO, 1.3 mol of NO and 0.70 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.576 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
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Suppose a 500. mL flask is filled with 0.90 mol of CO, 1.3 mol of NO and 0.70 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.576 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.90 mol of CO, 1.3 mol of NO and 0.70 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.576 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X
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