X 17X 18MX 1920X2122232425Suppose a 500. mL flask is filled with 0.90 mol of NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible:NO₂(g) + CO(g)NO(g) + CO₂(g)The equilibrium constant K for this reaction is 0.990 at the temperature of the flask.Calculate the equilibrium molarity of CO. Round your answer to two decimal places.26272829? 圖 8 民□□图]EArM

we have to calculate the equilibrium molarity of CO

Suppose a 500 ml flask is filled with 0.90 mol of NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant & for this reaction is 0.990 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 NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant & for this reaction is 0.990 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. 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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