Answer to Question #172094 in General Chemistry for Marie

Question

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

Determine the rate law and calculate the rate constant and determine the order of the reaction with respect to NO(g).

Answer 1

For the order of NO, comparing 1 and 2

As the concentration doubles, the rate quadruples, therefore implying a second order in NO

For the order of Cl2, comparing 2 and 3, the rate quadruples as the concentration quadruples, implying a first order I'm Cl2

Rate = k[NO]²[Cl₂]

Taking experiment 1

K = Rate /[NO]²[Cl₂]

= 3.4×10^-4/([0.03]²[0.01])

= 37.77 M^-2s^-1