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. please check your work. most people get this wrong!

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.

please check your work. most people get this wrong!

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