Chemistry Class

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Dinitrogentetraoxide partially decomposes according to the following equilibrium:

N2O4 (g) -> 2NO2 (g)
<-

A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol ofN2O4
remains. Keq for this reaction is ?.

hOw can i set up this problem?

  • Chemistry Class -

    Set up an ICE chart, substitute into the Keq expression, and solve for Keq. You want to convert moles to M (but that's easy since it's a 1 L flask.)
    initial:
    N2O4 = 0.400 M
    NO2 = 0

    change:
    NO2 = +2x
    N2O4 = -x

    equilibrium:
    NO2 = 2x
    N2O4 = 0.400-x and the problem tells you this is 0.0055

    Now do a little reasoning. Solve 0.400-x=0.0055 for x.
    Multiply that by 2 to find NO2 at equilibrium.
    Then substitute into Keq expression and solve for Keq.
    Check my work.
    0

  • Chemistry Class -

    whats the keq expression??'
    sorry we're learning about ice charts tomorrow but the teacher gave us a practice worksheet for the coming quiz and i wanted to see if i could figure out some of the problems early.

  • Chemistry Class -

    i did everything you said and got
    0.789 im at the step of setting up the keq expression

  • Chemistry Class -

    sorry to have gotten into this post, im solving a similar question and wanted to know how to do the final step

  • Chemistry Class -

    Your 0.789 is 2x and that is (NO2).
    (N2O4) = 0.0055 from the problem.
    Keq expression is
    Keq = (NO2)^2/(N2O4)

    If 0.400-x = 0.0055, then x = 0.3945
    So (N2O4) = 0.0055
    and NO2 = 2x = 0.3945*2 = 0.789

    Now substitute into Keq above to obtain:
    Keq = (0.789)^2/(0.0055) = ??
    about 113 or so.

  • Chemistry Class -

    I got the problem from my book, and it says the answer is 0.87?

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