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7 November, 14:22

Azomethane decomposes into nitrogen and ethane at elevated temperature:

H3C_N=N_CH3 _ N2 + C2H6

A chemist studying this reaction at 300ÁC begins an experiment with an azomethane concentration of 4.25 mM and obtains the following dаta:

Time (s) 100 150 200 250 300

[Azomethane] (mM) 3.29 2.90 2.55 2.25 1.98

Calculate the rate constant. Give an answer with concentration units of molarity and time units of seconds.

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  1. 7 November, 14:51
    0
    For a 1st order reaction:

    In (n/n0) = - k * (time difference)

    so k = - In (n/n0) / (t/t0)

    n is concentration at time t and n0 is the concentration at an earlier time t0.

    where k is constant.
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