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]

The rate law is rate = k[NO][O₃]

Option E) is the right answer.

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).

yes it is balanced