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.

Question

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.