Question

Using the given initial rate data for the reaction of nitrogen dioxide with fluorine, complete the rate law for this reaction in the box below. Rate law: ___?

a) Rate = k[NO2][F2]
b) Rate = k[NO2]^2[F2]
c) Rate = k[NO2][F2]^2
d) Rate = k[NO2]^2[F2]^2

Answer 1

The rate law for the reaction of nitrogen dioxide with fluorine, based on the second order for both NO2 and F2, is Rate = k[NO2]^2[F2]^2, where 'k' is the rate constant.

Step-by-step explanation:

The rate law for a chemical reaction is an equation that links the reaction rate with the concentrations of the reactants. It involves rate constants and concentration terms raised to exponential powers that reflect the reaction orders with respect to each reactant. In the student's question, the reaction of nitrogen dioxide (NO2) with fluorine (F2) is given. The experimentally determined rate law needs to be written based on the provided initial rate data.

As there is no specific data provided here, we will assume that the reaction order is determined to be second order with respect to NO2 and second order with respect to F2, as indicated in the question prompt (use of the exponent "2" for both reactants). Therefore, the rate law for the reaction would be:

Rate = k[NO2]2[F2]2

This rate law states that the rate of reaction is directly proportional to the square of the concentration of NO2 as well as to the square of the concentration of F2, with 'k' being the rate constant.