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21 December, 18:16

Given the following data, determine the rate constant of the reaction 2NO (g) + Cl2 (g) - -> 2NOCl (g) Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4

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  1. 21 December, 18:35
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    k = 2.647 x 10-2 M-2 s-1

    Explanation:

    2NO (g) + Cl2 (g) - -> 2NOCl (g)

    Experiment [NO] (M) [Cl2] (M) Rate (M/s)

    1 0.0300 0.0100 3.4 x 10-4

    2 0.0150 0.0100 8.5 x 10-5

    3 0.0150 0.0400 3.4 x 10-4

    Frrom experiments 1 and 3;

    Reducing the concentration of NO by a factor of 2 decreases the rate of the reaction by a factor of 4. This means the reaction is second order with respect to NO.

    From experiments 2 and 3:

    Increasing the concentration of Cl2 by a factor of 4 increases the rate by a factor of 4. This means the reaction is first order with respect to Cl2

    The rate equation is given as;

    Rate = k [NO]² [Cl2]

    From experiment 1;

    k = [NO]² [Cl2] / Rate

    k = 0.0300² * 0.0100 / 3.4 x 10-4

    k = 2.647 x 10-2 M-2 s-1
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