Suppose a 250. mL flask is filled with 0.50 mol of Br,, 0.10 mol of BROCI and 0.40 mol of BrCl. The following reaction becomes possible: Br, (e) +OCl, (g) - BROCI(g) +BrCl(g) The equilibrium constant K for this reaction is 0.455 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.50 mol of Br,, 0.10 mol of BROCI and 0.40 mol of BrCl. The following reaction becomes possible: Br, (e) +OCl, (g) - BROCI(g) +BrCl(g) The equilibrium constant K for this reaction is 0.455 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. 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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Calculate the equilibrium molarity of OCl2.
![Suppose a 250. mL flask is filled with 0.50 mol of Br,, 0.10 mol of BrOCl and 0.40 mol of BrCl. The following reaction becomes possible:
Br, (g) +0Cl, (g) - BROCI(g) +BrC1(g)
The equilibrium constant K for this reaction is 0.455 at the temperature of the flask.
Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd37d50d8-93d1-467d-90d5-13298d0e52a9%2F37f08d2b-0413-460f-97e6-5dc919cdd5a4%2F7uy0bmo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.50 mol of Br,, 0.10 mol of BrOCl and 0.40 mol of BrCl. The following reaction becomes possible:
Br, (g) +0Cl, (g) - BROCI(g) +BrC1(g)
The equilibrium constant K for this reaction is 0.455 at the temperature of the flask.
Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.
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