CHEMISTRY HELP!

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Consider the following reactions and their equilibrium constants.

(NO(g) + 0.5Br2(g) <===> NOBr(g) Kp = 5.3

2NO(g) <===> N2(g) + O2(g) Kp = 2.1 x 1030

Use these equations and their equilibrium constants to determine the equilibrium constant for the following reaction:

N2(g) + O2(g) + Br2(g) <===> 2NOBr(g) Kp = ?

  • CHEMISTRY HELP! -

    Write K expression for eqn 1.
    (NOBr)/(NO)(Br2)^1/2 = 5.3.
    Now square that.
    (NOBr)^2/(NO)^2(Br2) = 5.3^2
    Multiply that equation by Keq for equation #2 which is
    (NOBr)^2/(N2)(O2) = 2.1 x 10^30

    The (NO)^2 cancels and you are left with Keq for the reaction you want and K for the final reaction is just 5.3^2 x 2.1 x 10^30 = ??

  • CHEMISTRY HELP! -

    THANKS!

  • CHEMISTRY HELP! -

    Consider the following equilibrium:
    2NO(g) N2(g) + O2(g); Keq = 2.1 × 1030

  • CHEMISTRY HELP! -

    The previous answer is wrong by the way.

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