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
Asked Nov 2, 2019

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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Step 1

Initial concentration of CO = number of mol/volume (L) = 0.80 mol /0.250 L = 3.2 M

Initial concentration of NO = 0.60 mol/ 0.250 L...

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Chemistry

Equilibrium Concepts

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