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Suppose a 250. mL flask is filled with 0.40 mol of OCl2, 0.80 mol of BrOC1 and 1.1 mol of BrCl. The following reaction becomes possible: Br2(g) + OCl2(g) BrOCI (g) + BrCl (g) The equilibrium constant K for this reaction is 0.727 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. Пм X G

Suppose a 250. mL flask is filled with 0.40 mol of OCl2, 0.80 mol of BrOC1 and 1.1 mol of BrCl. The following reaction becomes possible: Br2(g) + OCl2(g) BrOCI (g) + BrCl (g) The equilibrium constant K for this reaction is 0.727 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. Пм X G

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.52QE: Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium...
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Suppose a 250. mL flask is filled with 0.40 mol of OCl2, 0.80 mol of BrOC1 and 1.1 mol of BrCl. The following reaction becomes possible: Br2(g) + OCl2(g) BrOCI (g) + BrCl (g) The equilibrium constant K for this reaction is 0.727 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. Пм X G
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.40 mol of OCl2, 0.80 mol of BrOC1 and 1.1 mol of BrCl. The following reaction becomes possible: Br2(g) + OCl2(g) BrOCI (g) + BrCl (g) The equilibrium constant K for this reaction is 0.727 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. Пм X G
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