The reaction 2 NO2(g)+F2(g) →2 NO2 F(g) has a second order rate law, rate =k[NO2][F2] . Suggest

step 1 In order for this rate law to be valid, we know that there must be some reaction where we have N

The reaction 2 NO2(g)+F2(g) →2 NO2 F(g) has a second order...

The reaction 2 $\mathrm{NO}_{2}(g)+\mathrm{F}_{2}(g) \rightarrow 2 \mathrm{NO}_{2} \mathrm{F}(g)$ has a second order rate law, rate $=k\left[\mathrm{NO}_{2}\right]\left[\mathrm{F}_{2}\right] .$ Suggest a mechanism that is consistent with this rate law.

Key Concepts

Intermediates

Intermediates are species that appear in one or more steps of the reaction mechanism but not in the overall balanced equation. They are generated and consumed during the process, and their concentrations are usually low. Their involvement is key to proposing a mechanism that accounts for the observed kinetics without affecting the overall stoichiometry.

Reaction Mechanism

A reaction mechanism is a detailed, step-by-step description of the pathway by which reactants are converted into products. It breaks down the overall reaction into elementary steps, each with its own rate law, and explains how the observed overall rate law arises from the kinetics of these individual steps.

Elementary Steps

Elementary steps are the individual reactions that occur in a proposed mechanism, and each one represents a single collision event or molecular process. Their rates combine to give the overall reaction rate, and understanding them helps in linking the molecular details with the observed macroscopic kinetics.

Rate?Determining Step

The rate?determining step is the slowest step in the reaction mechanism that controls the overall reaction rate. Its kinetic characteristics typically dictate the form of the observed rate law, so a mechanism must be consistent with the experimental rate law by identifying a step that involves the proper reaction order.

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