Problem: An important step in the industrial production of hydrogen is the reaction of carbon monoxide with water (i.e. the water gas shift reaction):CO (g) + H2O (g) ⇋ CO2 (g) + H2 (g)At 775 K, the equilibrium constant K p for this reaction is 3.9. If 0.2 moles CO 2 and 0.4 moles H2 were introduced in a 10.0 L container and heated to 775 K, what are the equilibrium concentrations of all components?

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We are being asked to calculate the equilibrium concentrations where its Kp is given.

 CO (g) + H2O (g) ⇋ CO2 (g) + H2 (g)


When dealing with equilibrium:

Kc → equilibrium units are in molarity 
Kp → equilibrium units in terms of pressure


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Problem Details

An important step in the industrial production of hydrogen is the reaction of carbon monoxide with water (i.e. the water gas shift reaction):

CO (g) + H2O (g) ⇋ CO2 (g) + H2 (g)

At 775 K, the equilibrium constant K p for this reaction is 3.9. If 0.2 moles CO 2 and 0.4 moles H2 were introduced in a 10.0 L container and heated to 775 K, what are the equilibrium concentrations of all components?

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