Question

Consider the following reaction mechanism.

Answer 1

Answer: The correct answer is $k[NO_2][F_2]$

Explanation:

Rate law states that the rate of a reaction is directly proportional to the concentration of the reactants each raised to power a stoichiometric coefficient which is determined experimentally and is called as order.

$Rate=k[A]^x[B]^y$

where,

k = Rate constant

x = Order with respect to A

y = Order with respect to B

In a mechanism, it is determined from the slow step of the reaction.

The slow step of the mechanism is:

$NO_2+F_2\rightarrow NO_2F+F$

The rate of this reaction is given by the expression:

$rate=k[NO_2][F_2]$

Thus, the correct answer is $k[NO_2][F_2]$

Answer 2

The rate law for this reaction is:

r = k[NO2][F2].

Hope this helps!