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    equilibrium consant Kc and concentrations

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    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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    Solution Preview

    (a) Kc =[CO]*[H2O] / {[CO2]*[H2]}
    then Kc = (0.050 * 0.040) /(0.086 * 0.045) = 0.52

    (b) Write the initial, change and equilibrium concentrations of all chemicals.
    Treat the concentrations of previous equilibrium as the initial concentrations except ...

    Solution Summary

    The solution is comprised of step-by-step calculations of the equilibrium constant Kc and the concentrations of the chemicals when a new equilibrium is re-established by adding more reactant.