Question

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]

Answer 1

Answer: it’s c

Step-by-step explanation:

Answer 2

A

Step-by-step 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.