Question

Consider this equilibrium process at 686°C.
CO2(g) + H2(g) 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.

(b) If the concentration of CO2 to raised to 0.40 mol/L by the addition of CO2, what would be the concentrations of all the gases when equilibrium is reestablished?

Answer 1

Can you do the Kc; i.e., the first part?

Answer 2

Yes, the answer Kc=0.517

Answer 3

........CO2(g) + H2(g)==> CO(g) + H2O(g)
E......0.086....0.045.....0.050...0.040
---------------------------------------
I.......0.400....0.045...0.050...0.040
C.........-x......-x.......+x.....+x
E.....0.400-x..0.045-x..0.050-x..0.040+x

Substitute the E line into Keq expression and solve. Post your work if get stuck.