Suppose a 500. mL flask is filled with 2.0 mol of CO, 1.2 mol of NO and 0.70 mol of CO2. The following reaction becomes possible: NO2(g)+CO(g) → NO(g)+CO2(g) = The equilibrium constant K for this reaction is 7.03 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 2.0 mol of CO, 1.2 mol of NO and 0.70 mol of CO2. The following reaction becomes possible: NO2(g)+CO(g) → NO(g)+CO2(g) = The equilibrium constant K for this reaction is 7.03 at the temperature of the flask. Calculate the equilibrium molarity of CO. 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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