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    Concentrations of Components in an Equilibrium

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    The following equilibrium process at 686 deg. C.
    CO2(g) + H2(g) f/r CO(g) + H20 (g)
    The equilibrium concentration of the reacting species are [CO]=0.050 M, [H2]=0.045 M, [CO2]=0.086 M, and [H2O]=0.040 M.

    I calculate Kc for the reaction at 686 deg. C. = 0.52

    If CO2 is added to increase concentration ot 0.55 mol/L, what will the concentrations of all the gases be when equilibrium is re-established?


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    Solution Preview

    Because stress is added to the left hand side of the equilibrium, equilibrium shifts left to relief the stress according to the le Chatelier Principle:

    | CO2(g) + H2(g) <--> CO(g) + H20 (g)
    Initial ...

    Solution Summary

    The solution uses and explains le Chatelier's Principle in order to do the necessary calculations to finding the concentrations of the reactants and products of the re-established equilibrium described in the question.