Incorrect Your answer is incorrect. Suppose a 500. mL flask is filled with 0.90 mol of NO2, 1.4 mol of CO and 1.0 mol of NO. The following reaction becomes possible: NO2(g) +CO(g) = NO(g) +CO2(g) The equilibrium constant K for this reaction is 8.93 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. 0.69 M ☑

Incorrect Your answer is incorrect. Suppose a 500. mL flask is filled with 0.90 mol of NO2, 1.4 mol of CO and 1.0 mol of NO. The following reaction becomes possible: NO2(g) +CO(g) = NO(g) +CO2(g) The equilibrium constant K for this reaction is 8.93 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. 0.69 M ☑

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Help with the following question Please round the answer to 2 decimal places