Question

Consider the formation of nitrogen dioxide and oxygen: NO(g)+O3(g)⇌NO2(g)+O2(g) The reaction is first order in O3 and second order overall. What is the rate law? (A) rate=k[NO]2[O3]2(B) rate=k[NO][O3]2(C) rate=k[O3](D) rate=k[NO](E) rate=k[NO][O3](G) rate=k[NO]2[O3]

Answer 1

The rate law is rate = k[NO][O₃]

Option E) is the right answer.

Step-by-step explanation:

Hi there!

For this generic reaction:

A + B → products

the rate law will be:

rate = k[A]ⁿ[B]ᵃ

this reaction is n-order in A and a-order in B. The overall reaction is the sum of the orders of each reactant, in this case:

Overall order of the reaction = n + a

In our problem, we know that the reaction is first order in O₃ and second order overall. Then:

Overall order of the reaction = Order in NO + Order in O₃

2 = n + 1

2 - 1 = n

n = 1

Then, the reaction is first order in NO and first order in O₃.

The rate law will be:

rate = k[NO][O₃]

The right answer is the option E).