In a study of the conversion of methane to other fuels, a chemical engineer mixes gaseous CH4 and H2O in a 0.32-L flask at 1200 K. At equilibrium the flask contains 0.26 mol of CO, 0.091 mol of H2, and 0.041 mol of CH4. What is the [H2O] at equilibrium

The at equilibrium is 0.561 M.

Explanation:

The given data is as follows.

    Volume of flask = 0.32 L,

 No. of moles of = 0.041 mol,

 No, of moles of CO = 0.26 mol,  No. of moles of = 0.091 mol

 Equilibrium constant, K = 0.26

Balanced chemical equation for this reaction is as follows.

Hence,

              K = ...... (1)

First, we will calculate the molarity or concentration of given species as follows.

= 0.128 M,

= 0.8125 M,

= 0.284 M

Therefore, using expression (1) we will calculate the as follows.

     K =

or,    

             =

             =

             = 0.561 M

Thus, we can conclude that the at equilibrium is 0.561 M.

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