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Consider the following equilibrium process at 686C: CO2() + H2(8)=CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, [H2) = 0.0400 M, (CO2) = 0.0890 M, and [H,0] = 0.0370 M. (a) Calculate K for the reaction at 686C. (b) If we add CO2 to increase its concentration to 0.460 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M (a) Calculate K for the reaction at 686C. (b) If we add CO2 to increase its concentration to 0.460 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H: M CO: M H20: M