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Suppose a 500. mL flask is filled with 1.7 mol of NO2, 1.4 mol of NO and 1.1 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 1.89 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X S

Suppose a 500. mL flask is filled with 1.7 mol of NO2, 1.4 mol of NO and 1.1 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 1.89 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X S

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Chemistry
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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 500. mL flask is filled with 1.7 mol of NO2, 1.4 mol of NO and 1.1 mol of CO₂. The following reaction becomes possible: NO₂(g)+CO(g) NO(g) + CO₂(g) OKINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant pdf The equilibrium constant K for this reaction is 1.89 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. o search M Explanation = Check X S 2072 McGraw BIL UC. All Rights Reserved. Terms of se
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.7 mol of NO2, 1.4 mol of NO and 1.1 mol of CO₂. The following reaction becomes possible: NO₂(g)+CO(g) NO(g) + CO₂(g) OKINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant pdf The equilibrium constant K for this reaction is 1.89 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. o search M Explanation = Check X S 2072 McGraw BIL UC. All Rights Reserved. Terms of se
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