Suppose a 500. mL flask is filled with 1.2 mol of N, and 0.10 mol of O2. The following reaction becomes possible: N2(g) + O2(g) ~ 2NO(g) The equilibrium constant K for this reaction is 9.60 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.2 mol of N, and 0.10 mol of O2. The following reaction becomes possible: N2(g) + O2(g) ~ 2NO(g) The equilibrium constant K for this reaction is 9.60 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places.
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 1.2 mol of N, and 0.10 mol of O,. The following reaction becomes possible:
N2(g)+ O2(g) – 2NO(g)
The equilibrium constant K for this reaction is 9.60 at the temperature of the flask.
Calculate the equilibrium molarity of O2. Round your answer to two decimal places.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa21199a8-7a5a-4751-9685-1126762a8cde%2F17e0a929-5649-4ff2-b76f-a594a4459a2f%2Flxh66w9_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.2 mol of N, and 0.10 mol of O,. The following reaction becomes possible:
N2(g)+ O2(g) – 2NO(g)
The equilibrium constant K for this reaction is 9.60 at the temperature of the flask.
Calculate the equilibrium molarity of O2. Round your answer to two decimal places.
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