Consider the following equilibrium process at 686°C. CO2(g) + H2(g) equilibrium reaction arrow CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.050 M, [H2] = 0.045 M, [CO2] = 0.086 M, and [H2O] = 0.040 M. (a) Calculate Kc for the reaction at 686°C. WebAssign will check your answer for the correct number of significant figures. (b) If we add CO2 to increase its concentration to 0.50 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?

a) The value of the is 0.52.

b)Concentration of all species when equilibrium reestablishes:

Explanation:

a)  

Equilibrium concentration of species :

The expression of equilibrium constant is given as :

b)

Initially:

0.50 M    0.045 M      0.050 M   0.040 M

At equilibrium ;

(0.50-x) M    (0.045-x) M      (0.050+x) M   (0.040+x) M

Solving fro x;

x = 0.0252

Concentration of all species when equilibrium reestablishes:

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