Jj.53. Suppose a 250. mL flask is filled with 1.0 mol of N₂ and 0.70 mol of NO. The following reaction becomes possible:N₂(g) + O₂(g) 2NO(g)PThe equilibrium constant K for this reaction is 0.243 at the temperature of the flask.Calculate the equilibrium molarity of O₂. Round your answer to two decimal places.MXŚ

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Suppose a 250. mL flask is filled with 1.0 mol of N₂ and 0.70 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) 2NO(g) The equilibrium constant K for this reaction is 0.243 at the temperature of the flask. Calculate the equilibrium molarity of O₂. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.0 mol of N₂ and 0.70 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) 2NO(g) The equilibrium constant K for this reaction is 0.243 at the temperature of the flask. Calculate the equilibrium molarity of O₂. Round your answer to two decimal places.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 60QRT

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