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The first-order decomposition of n2o at 1000 k has a rate constant of 0.76 s-1. if the initial concentration of n2o is 10.9 m, what is the concentration of n2o after 9.6 s

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  1. Today, 03:16
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    For a first-order reaction, the rate law would be expressed as:

    r = dC / dt = - kC

    Integrating it from time zero and the initial concentration, Co, to time, t, and the final concentration, C. We will obtain the first-order integrated law as follows:

    ln C/Co = - kt

    To determine the concentration of N2O in the system at a certain time, we simply substitute the given values from the problem statement as follows:

    ln C / Co = - kt

    ln C / 10.9 = - 0.76 (9.6)

    e^ln C / 10.9 = e^-0.76 (9.6)

    C / 10.9 = 6.78 x 10^-4

    C = 7.39 x 10^-3 m

    Therefore, the concentration of N2O in the system after 9.6 s would be 7.39 x10^-3 m.
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