Question

The oxidation of NO by Oz is first order in each of the reactants, and its rate constant is 1.5 x 10PM-1.5-1. If the concentration of NO is 0.03 M and the concentration of Oz is 0.14 M. what is the rate of reaction in Mos-1?

Answer 1

The rate of the reaction for the oxidation of NO by O2, which is first order in NO and O2, with the given concentrations and rate constant, is 6.3 x 10^-4 M s^-1.

Step-by-step explanation:

The student wants to determine the rate of reaction for the oxidation of NO by O2 when the reaction is first order with respect to each reactant, and the rate constant (k) is given as 1.5 x 10-1.5 M-1 s-1. Given the concentrations of NO and O2 as 0.03 M and 0.14 M respectively, we can use the rate law to find the reaction rate.

The rate law for a reaction that is first order in NO and first order in O2 is given by:

rate = k[NO][O2]

Substituting the given values yields:

rate = (1.5 x 10-1.5 M-1 s-1)(0.03 M)(0.14 M)

rate = 6.3 x 10-4 M s-1

Therefore, the rate of the reaction is 6.3 x 10-4 M s-1.