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1 June, 15:00

For the reaction CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H2] = 0.045, [H2O] = 0.025, and [CH4] = 0.046M, in which direction will the reaction shift to attain equilibrium?

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  1. 1 June, 17:19
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    the reaction will shift to the left and produce more reactants

    Explanation:

    Step 1: data given

    Kc = 190

    Temperature = 1000 K

    [CO] = 0.025 M

    [H2] = 0.045 M

    [H2O] = 0.025 M

    [CH4] = 0.046 M

    When Q=Kc, the system is at equilibrium and there is no shift to either the left or the right.

    When Q
    When Q>Kc, there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants

    Step 2: The balanced equation

    CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g)

    Step 3: calculate Q

    Q = [H2O][CH4] / [CO][H2]³

    Q = (0.025*0.046) / (0.025*0.045³)

    Q = 504.8

    Q > Kc

    This means there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants
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