Question

High-flying aircraft release NO Into the stratosphere, which catalyzes this process. When O_3 and NO concentrations are 5 x 10^1^2 molecule/cm^3 and 2 x 10^9 molecule/cm^3, respectively, what is the rate of O_3 depletion? The rate constant k for the rate-determining step Is 6 times 10-15 (cm^3)2/molecules. Give your answer in scientific notation

Answer 1

The rate of ozone depletion due to the reaction of O3 with NO, given the concentrations of O3 and NO, and the rate constant k, is 6 x 10^-1 molecules/cm^3 per second.

Step-by-step explanation:

The question asks for the rate of ozone depletion in the stratosphere due to reactions with nitric oxide (NO) released by high-flying aircraft. Given the concentrations of ozone (O3) and NO, and the rate constant (k) for the rate-determining step, we can calculate the rate of O3 depletion using the provided rate equation:

rate = k[NO][O3]

Using the given concentrations, O3 = 5 x 1012 molecules/cm3 and NO = 2 x 109 molecules/cm3, and the rate constant, k = 6 x 10-15 cm3/molecules2, the rate of O3 depletion is calculated as follows:

rate = (6 x 10-15 cm3/molecules2) × (5 x 1012 molecules/cm3) × (2 x 109 molecules/cm3)

rate = 6 x 10-15 × 5 x 1012 × 2 x 109 cm3/molecules × molecules2/cm6

rate = 60 x 10-2 molecules/cm3·s

rate = 6 x 10-1 molecules/cm3·s

Therefore, the rate of ozone depletion is 6 x 10-1 molecules/cm3
per second.