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21 January, 14:33

The following data are for the reaction 2NO (g) + O2 (g) → 2NO2 (g) at some temperature. Experiment 1: [NO] = 0.0070 M; [O2] = 0.0070 M; rate = 9.6 10-1 M/s. Experiment 2: [NO] = 0.0070 M; [O2] = 0.014 M; rate = 1.9 M/s. Experiment 3: [NO] = 0.014 M; [O2] = 0.0070 M; rate = 3.8 M/s. Determine: (a) The order of the reaction with respect to nitrogen monoxide: order = WebAssign will check your answer for the correct number of significant figures. (b) The order of the reaction with respect to oxygen: order = (c) The value of the rate constant for the reaction at this temperature: k = WebAssign will check your answer for the correct number of significant figures. L2/mol2s

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  1. 21 January, 18:22
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    2NO (g) + O2 (g) → 2NO2 (g)

    Experiment 1:

    [NO] = 0.0070 M; [O2] = 0.0070 M; rate = 9.6 10-1 M/s

    Experiment 2:

    [NO] = 0.0070 M; [O2] = 0.014 M; rate = 1.9 M/s.

    Experiment 3:

    [NO] = 0.014 M; [O2] = 0.0070 M; rate = 3.8 M/s

    a) The order of the reaction with respect to nitrogen monoxide

    When the concentration of oxygen is held constant, doubling the concentration of NO leads to the rate being increased by a factor of 4. This means it is second order with respect to NO.

    (b) The order of the reaction with respect to oxygen:

    When the concentration of NO is held constant, doubling the concentration oxygen leads to the rate being increased by a factor of 2. This means it is first order with respect to oxygen.

    The overall rate of reaction is given as;

    rate = k [NO]^2[O]

    (c) The value of the rate constant for the reaction at this temperature:

    rate = k [NO]^2[O]

    Taking experiment 1;

    rate = 9.6*10-1 M/s

    [NO] = 0.0070 M

    [O2] = 0.0070 M

    k = ?

    9.6*10-1 = k * 0.0070^2 * 0.0070

    k = (9.6*10-1) / 3.43*10-7

    k = 2798833.82

    k = 2800000 (2. s. f)
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