Suppose a 500. mL flask is filled with 0.60 mol of NO and 2.0 mol of N0,. The following reaction becomes possible: 2' NO, (g) + NO(g) = 2NO, (g) The equilibrium constant K for this reaction is 0.225 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ) M
Suppose a 500. mL flask is filled with 0.60 mol of NO and 2.0 mol of N0,. The following reaction becomes possible: 2' NO, (g) + NO(g) = 2NO, (g) The equilibrium constant K for this reaction is 0.225 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ) M
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 0.60 mol of NO and 2.0 mol of NO,. The following reaction becomes possible:
NO, (g) +NO(g)–
2NO,(g)
The equilibrium constant K for this reaction is 0.225 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
| M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9ac4fab7-4126-49f3-8d16-60074d8271b3%2F418ef596-fe93-4ab6-8d66-5387c74d66c7%2Fc3bhhy2_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.60 mol of NO and 2.0 mol of NO,. The following reaction becomes possible:
NO, (g) +NO(g)–
2NO,(g)
The equilibrium constant K for this reaction is 0.225 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
| M
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