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)
