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

Answer 1

The rate of the reaction between nitric oxide and ozone is 4.56 x 10^-4 mol L^-1 s^-1, calculated using the rate law rate = k[NO][O3] with the given rate constant and reactant concentrations.

Step-by-step explanation:

The student is asking about the rate at which nitric oxide (NO) and ozone (O3) react in the stratosphere, based on given concentrations and a known rate constant. Since the reaction is first order with respect to both NO and O3, the rate law can be written as rate = k[NO][O3], where k is the rate constant. Using the provided concentrations of NO and O3 along with the rate constant, one can calculate the rate of the reaction.

Given: k = 1.9 x 104 L​mol-1s-1, [NO] = 1.2 × 10-5 mol L-1, [O3] = 2.0 x 10-5 mol L-1

The rate can be calculated as follows:

rate = k[NO][O3] = (1.9 x 104 L​mol-1s-1)(1.2 × 10-5 mol L-1)(2.0 x 10-5 mol L-1)

rate = 4.56 x 10-4 mol L-1s-1

The rate of the reaction is 4.56 x 10-4 mol L-1s-1.