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13 May, 05:08

The unsaturated hydrocarbon butadiene (C4H6) dimerizes to 4-vinylcyclohexan (C8H12). When data collected in studies of the kinetics of this reaction were plotted against reaction time, plots of [C4H6] or ln[C4H6] produced curved lines, but the plot of 1/[C4H6] was linear. a) What is the rate law for the reaction? b) How many half-lives will it take for the [C4H6] to decrease to 3.1% of its original concentration? The relationship of [A]t/[A]o = 0.50^n, where n = the number of half-lives.

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  1. 13 May, 08:49
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    From the information of the graph plots, the reaction is a second order reaction.

    a) What is the rate law for the reaction?

    Rate = k [C4H6]²

    The superscript 2 signifies it is a second order reaction.

    b) How many half-lives will it take for the [C4H6] to decrease to 3.1% of its original concentration?

    Using the formular below;

    [A]t / [A]o = 0.50^n

    [A]t = 100%

    [A]o = 3.1%

    100 / 3.1 = 0.50^n

    32 = 0.50^n

    2^5 = 2^-n

    n = 5

    It would take five half lives.
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