Try Again Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +0,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. 3.36 M

Try Again Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +0,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. 3.36 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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Suppose a 500. mL flask is filled with 0.20 mol of Cl, and 1.5 mol of HCl. The following reaction becomes possible: H,(2) + Cl, (g) – 2HCI(3) The equilibrium constant K for this reaction is 0.754 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. |M ?
Suppose a 500. mL flask is filled with 0.80 mol of NO, and 1.7 mol of NO. The following reaction becomes possible: NO, (g)+NO (g)2NO, (g) The equilibrium constant K for this reaction is 5.51 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. | M ?
Subject: chemistry
Suppose a 250. mL flask is filled with 1.1 mol of NO,, 0.30 mol of CO and 1,3 mol of CO,. The following reaction becomes possible: NO, (g) +co(g) - NO(s)+Co,(g) The equilibrium constant K for this reaction is 7.86 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
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