One reaction that destroys O3 molecules in the stratosphere is NO + O3  NO2 + O2

When this reaction was studied in the laboratory, it was found to be first order with respect to both NO and O3 with a rate constant of 1.9 x 104 mol L-1S-1. If [NO] = 1.2 x 10-5 mol L-1 and [O3] = 2.0 x 10-5mol L-1, what is the rate of this reaction?

I got it!!!

the answer is 4.6x10^-6

good work

To find the rate of this reaction, we need to use the rate law expression and plug in the given values. The rate law expression for the given reaction is:

Rate = k[NO]^1[O3]^1

Where:
- Rate is the rate of the reaction
- k is the rate constant
- [NO] and [O3] are the concentrations of NO and O3, respectively, raised to their respective powers in the rate law expression.

Given values:
- k = 1.9 x 10^4 mol L^-1 s^-1
- [NO] = 1.2 x 10^-5 mol L^-1
- [O3] = 2.0 x 10^-5 mol L^-1

Substituting the values into the rate law expression, we have:

Rate = (1.9 x 10^4 mol L^-1 s^-1)(1.2 x 10^-5 mol L^-1)(2.0 x 10^-5 mol L^-1)

Simplifying the expression, we get:

Rate = (1.9 x 1.2 x 2.0) x (10^4 x 10^-5 x 10^-5) mol L^-1 s^-1

Rate = 4.56 x 10^-5 mol L^-1 s^-1

Therefore, the rate of this reaction is 4.56 x 10^-5 mol L^-1 s^-1.