Suppose a 250.mL flask is filled with 0.80mol of CO, 0.60mol of NO and 0.20mol of CO2. The following reaction becomes possible: NO2(g)+CO(g) <->NO(g)+CO2(g) The equilibrium constant K for this reaction is 9.16 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
Suppose a 250.mL flask is filled with 0.80mol of CO, 0.60mol of NO and 0.20mol of CO2. The following reaction becomes possible: NO2(g)+CO(g) <->NO(g)+CO2(g) The equilibrium constant K for this reaction is 9.16 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
General, Organic, and Biological Chemistry
7th Edition
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:H. Stephen Stoker
Chapter9: Chemical Reactions
Section: Chapter Questions
Problem 9.76EP: Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the...
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Suppose a 250.mL flask is filled with 0.80mol of CO, 0.60mol of NO and 0.20mol of CO2. The following reaction becomes possible:
NO2(g)+CO(g) <->NO(g)+CO2(g)
The equilibrium constant K for this reaction is 9.16 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
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