Suppose a 500 ml flask is filled with 0.20 mol of OCI,, 0.90 mol of BrOCI and 0.10 mol of BrCl. The following reaction becomes possible: Br₂(g) + OCI, (g) BrOCI(g) + BrC1 (g) 1 The equilibrium constant K for this reaction is 7.85 at the temperature of the flask. Calculate the equilibrium molarity of OCI₂. Round your answer to two decimal places.
Suppose a 500 ml flask is filled with 0.20 mol of OCI,, 0.90 mol of BrOCI and 0.10 mol of BrCl. The following reaction becomes possible: Br₂(g) + OCI, (g) BrOCI(g) + BrC1 (g) 1 The equilibrium constant K for this reaction is 7.85 at the temperature of the flask. Calculate the equilibrium molarity of OCI₂. Round your answer to two decimal places.
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 17A
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![Suppose a 500 ml flask is filled with 0.20 mol of OCI,, 0.90 mol of BrOCI and 0.10 mol of BrCl. The following reaction becomes
possible:
Br₂(g) + OCI, (g) BrOCI(g) + BrC1 (g)
The equilibrium constant K for this reaction is 7.85 at the temperature of the flask.
Calculate the equilibrium molarity of OCI₂. Round your answer to two decimal places.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa3d40dd0-5734-4b19-8135-e99e0d47822d%2Faf3b0fa6-b192-4381-8b99-9871a5de0c73%2F13hazu9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 500 ml flask is filled with 0.20 mol of OCI,, 0.90 mol of BrOCI and 0.10 mol of BrCl. The following reaction becomes
possible:
Br₂(g) + OCI, (g) BrOCI(g) + BrC1 (g)
The equilibrium constant K for this reaction is 7.85 at the temperature of the flask.
Calculate the equilibrium molarity of OCI₂. Round your answer to two decimal places.
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