2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container and they react according to the equation CO2(g) + H2(g) ⇄ CO(g) + H2O(g) K = 2.50 What will be the concentration of carbon monoxide when equilibrium is reached? 0.191 M 0.091 M 0.209 M (Your correct answer) 0.913 M 1.05 M

0.209 M

Explanation:

Moles of   = 2.00 mole

Moles of   = 1.50 mole

Volume of container = 5.00 L

Initial concentration of =

Initial concentration of =

The given balanced equilibrium reaction is,

Initial conc.          0.400 M          0.300M             0 M        0 M

   At eqm. conc.     (0.400-x) M   (0.300-x) M   (x) M      (x)  M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving the term 'x', we get :

x = 0.209 M

Concentration of at equilibrium = x M  =  0.209 M

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