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8 September, 12:23

For the reaction a → b, the rate law is: rate = k * [a]. over the course of 4 minutes, the concentration of a reduces by one-half, from 1.00 mto 0.50 m. how is the rate affected?

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  1. 8 September, 12:51
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    The rate law for the equation is as follows;

    Rate = k [A]

    the order with respect to A is 1, therefore this is a first order reaction as A is the only reactant.

    At t = 0 minutes [A] = 1.00 M

    rate - initial rate

    rate = k [1.00 M] - - - 1)

    At t = 4 minutes [A] = 0.50 M

    rate' - new rate

    rate' = k [0.50] - - 2)

    Divide 2) / 1)

    rate'/rate = 0.5/1

    rate' = 0.5 rate

    rate has been reduced by half
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