In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) H2O (g) CO2 (g) H2 (g) In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. Keq at the temperature of the experiment is . A) 5.47 B) 1.0 C) 1.78 D) 0.75 E) 0.56

at  the temperature of the experiment is 0.56.

Explanation:

Moles of   = 0.35 mole

Moles of   = 0.40 mole

Volume of solution = 1.00 L

Initial concentration of =

Initial concentration of =

Equilibrium concentration of =

The given balanced equilibrium reaction is,

Initial conc.          0.35 M         0.40 M                  0 M        0M

    At eqm. conc.     (0.35-x) M   (0.40-x) M   (x) M      (x) M

Given:  (0.35-x) = 0.19

x= 0.16 M

The expression for equilibrium constant for this reaction will be,

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

Thus at  the temperature of the experiment is 0.56.

the answer to your question is c