A possible mechanism for the overall reaction represented above is the following.

NO (g) + NO (g) → N2O2 (g) slow

N2O2 (g) + O2 (g) → 2NO2 (g) fast

Which of the following rate expressions agrees best with this possible mechanism?

A) Rate = k[NO]2

(D) Rate = k[NO]2[O2]

(B) Rate = k[NO]

(E) Rate = k[N2O2][O2][O2]

(C) Rate = k[NO]2[O2]

Question

Marble

Chemistry

4 April, 19:24

A possible mechanism for the overall reaction represented above is the following.

NO (g) + NO (g) → N2O2 (g) slow

N2O2 (g) + O2 (g) → 2NO2 (g) fast

Which of the following rate expressions agrees best with this possible mechanism?

A) Rate = k[NO]2

(D) Rate = k[NO]2[O2]

(B) Rate = k[NO]

(E) Rate = k[N2O2][O2][O2]

(C) Rate = k[NO]2[O2]

+3

Answers (2)

Know the Answer?

Karley · Answer 1

The third answer on Edgen 2020

Explanation:

Just took the test

Krista Andrews · Answer 2

A

Explanation:

The slow step of the reaction is the rate determining step. This means to get the rate law for a chemical activity with slow and fast steps, we have to consider the slow step if we are to write the rate law successfully.

Since the compound NO is reacting with itself, we have to raise the value of the concentration in the square bracket by 2. That is why we have the concentration squared.