consider the following reaction mechanism. no2 + f2 → no2f + f (slow) no2 + f → no2f (fast) overall: 2no2 +…
consider the following reaction mechanism. no2 + f2 → no2f + f (slow) no2 + f → no2f (fast) overall: 2no2 + f2 → 2no2f which is the correct rate law for this reaction? o kno2f2 o kno2ff2 o k2no2f o kno2f
Answer
Explanation:
Step1: Identify rate - determining step
The slow step determines the rate of the overall reaction. Here, the slow step is $\ce{NO2 + F2\rightarrow NO2F + F}$.
Step2: Write rate law for slow step
The rate law for a reaction is based on the reactants in the rate - determining step. For the reaction $\ce{NO2 + F2\rightarrow NO2F + F}$, the rate law is $rate = k[\ce{NO2}][\ce{F2}]$.
Answer:
$k[\ce{NO2}][\ce{F2}]$