Question

Regular flights of supersonic aircraft in the stratosphere are of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO + O3 ⟶ NO2 + O2 is first order with respect to both NO and O3 with a rate constant of 2.20 × 10⁷ L/mol/s. What is the instantaneous rate of disappearance of NO when [NO] = 3.3 × 10^−6 M and [O3] = 5.9 × 10^−7 M?

a) 1.32 × 10¹ M/s

b) 1.65 × 10² M/s

c) 2.42 × 10⁰ M/s

d) 4.84 × 10⁷ M/s

Answer 1

The instantaneous rate of disappearance of NO in the reaction NO + O3 ⟶ NO2 + O2 is 1.32 × 10^1 M/s. option (A)

Step-by-step explanation:

The question is asking for the instantaneous rate of disappearance of NO in the given reaction. The reaction is first order with respect to both NO and O3, and has a rate constant of 2.20 × 10^7 L/mol/s. The concentration of NO is given as [NO] = 3.3 × 10^-6 M, and the concentration of O3 is given as [O3] = 5.9 × 10^-7 M. To calculate the instantaneous rate of disappearance of NO, we can use the rate law:

Rate = k[NO][O3]

Substituting the given values:

Rate = (2.20 × 10^7 L/mol/s)(3.3 × 10^-6 M)(5.9 × 10^-7 M)

Rate = 1.32 × 10^1 M/s