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16 August, 12:21

The rate constant for the first order decomposition of A at 500oC is 9.2 x 10-3 s-1. how long will it take for 90.8% of a 0.500 M sample of A to decompose? Question options:

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  1. 16 August, 14:54
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    For this problem, we assume a first-order kinetics which has a kinetics expression written as:

    ln (Ca/Cao) = - kt

    We use this formula to solve for time, t. First we list the needed values,

    k = 9.2 x 10-3 s-1

    Cao = 0.500 M

    Xa = 90.8% = 1 - (Ca/Cao)

    Ca = 0.046 M

    ln (0.046/0.500) = - 9.2 x 10-3 s-1 (t)

    t = 259.34 s
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