Suppose a IS lOwing reaction becOmes possible: NO,(2) - CO(2) → NO(g) +CO,(g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. 0.37 M
Suppose a IS lOwing reaction becOmes possible: NO,(2) - CO(2) → NO(g) +CO,(g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. 0.37 M
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 30P
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![Suppose a 500. mL flask is filled with 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible:
NO,(9) + CO(2) = No(g) + CO,(g)
The equilibrium constant K for this reaction is 0.953 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
0.37 M
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c0fcb54-e854-49ef-aa69-39559bab08de%2Ff537c7b5-5982-4f18-aefc-ddb1d5e43d50%2Fbtpj7o6_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible:
NO,(9) + CO(2) = No(g) + CO,(g)
The equilibrium constant K for this reaction is 0.953 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
0.37 M
?
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