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Suppose a 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes possible: NO2(g) + CO (g) NO(g) + CO2(g) 772 The equilibrium constant K for this reaction is 0.566 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. □ M

Suppose a 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes possible: NO2(g) + CO (g) NO(g) + CO2(g) 772 The equilibrium constant K for this reaction is 0.566 at the temperature of the flask. Calculate the equilibrium molarity of CO. 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 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes possible: NO2(g) + CO (g) NO(g) + CO2(g) 772 The equilibrium constant K for this reaction is 0.566 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. □ M
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes possible: NO2(g) + CO (g) NO(g) + CO2(g) 772 The equilibrium constant K for this reaction is 0.566 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. □ M
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