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Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OCI, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) BrOCI(g) + BrC1 (g) The equilibrium constant X for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OCI, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) BrOCI(g) + BrC1 (g) The equilibrium constant X for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

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 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.
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