Suppose a 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes possible: NO2(g) + CO (g) NO(g) + CO2(g) 772 The equilibrium constant K for this reaction is 0.566 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. □ M
Suppose a 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes possible: NO2(g) + CO (g) NO(g) + CO2(g) 772 The equilibrium constant K for this reaction is 0.566 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. □ M
Chemistry: Principles and Practice
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Chapter14: Chemical Equilibrium
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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 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes
possible:
NO2(g) + CO (g) NO(g) + CO2(g)
772
The equilibrium constant K for this reaction is 0.566 at the temperature of the flask.
Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
□ M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e0c18cd-873b-4b76-ba81-a06b4c32b2ee%2F83a518f6-b13e-416d-88e8-9939ba018578%2Fazk7lf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.20 mol of NO2, 1.3 mol of CO and 1.8 mol of NO. The following reaction becomes
possible:
NO2(g) + CO (g) NO(g) + CO2(g)
772
The equilibrium constant K for this reaction is 0.566 at the temperature of the flask.
Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
□ M
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