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

Explanation:

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)