Suppose a 250. mL flask is filled with 1.7 mol of NO and 0.70 mol of NO,. The following reaction becomes possible: NO; (2) +NO(2) – 2NO,(g) The equilibrium constant K for this reaction is 3.09 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. IM

Suppose a 250. mL flask is filled with 1.7 mol of NO and 0.70 mol of NO,. The following reaction becomes possible: NO; (2) +NO(2) – 2NO,(g) The equilibrium constant K for this reaction is 3.09 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. IM

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 1.2 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co(2) + H,0(g) – Co,(3) +H,(g) The equilibrium constant K for this reaction is 0.545 at the temperature of the flask. Calculate the equilibrium molarity of H,0. Round your answer to two decimal places.
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Suppose a 500. mL flask is filled with 0.70 mol of CO, 1.7 mol of NO and 1.0 mol of CO,. The following reaction becomes possible: NO, (g) +CO(g)- NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.97 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM Continue MacBook Air
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