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

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