Question

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 L
mol⁻¹s⁻¹. If [NO] = 1.2 x 10-5 mol L⁻¹ and [O₃] = 2.0 x 10⁻⁵, what is the rate of this reaction?

Answer 1

The rate of reaction for NO reacting with O₃, given a rate constant of 1.9 x 10⁴ Lmol⁻¹s⁻¹ and the concentrations for NO and O₃, is calculated to be 4.56 x 10⁻¶ mol L⁻¹s⁻¹.

Step-by-step explanation:

The rate of the reaction between nitric oxide (NO) and ozone (O₃) can be calculated using the provided rate law, which is first order with respect to both NO and O₃. In this case, the rate constant provided is 1.9 x 10⁴ Lmol⁻¹s⁻¹, and the concentrations of NO and O₃ are 1.2 x 10⁻µ mol L⁻¹ and 2.0 x 10⁻µ mol L⁻¹, respectively.

The rate of the reaction is calculated as follows:

Rate = k[NO][O₃]

Rate = (1.9 x 10⁴ Lmol⁻¹s⁻¹)(1.2 x 10⁻µ mol L⁻¹)(2.0 x 10⁻µ mol L⁻¹)

Rate = (1.9 x 10⁴) x (1.2 x 10⁻µ) x (2.0 x 10⁻µ)

Rate = 4.56 x 10⁻¶ mol L⁻¹s⁻¹

Thus, the rate of reaction for the reaction between NO and O₃ under the given conditions is 4.56 x 10⁻¶ mol L⁻¹s⁻¹.