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Consider the following equilibrium process at 686C: CO2(g) + H2(g) CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] =...

Consider the following 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.  
(I got Kc=.52 which is correct but now I don't know how to do part B)
(b) If we add CO2 to increase its concentration to 0.25 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?
Can you help?

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