Answered

Consider the following reaction mechanism.


NO2 + F2 mc020-1.jpg NO2F + F (slow)

NO2 + F mc020-2.jpg NO2F (fast)

Overall: 2NO2 + F2 mc020-3.jpg 2NO2F


Which is the correct rate law for this reaction?

k[NO2][F2]

k[NO2F][F2]

k[2NO2][F]

k[NO2][F]

Verified Answer :

The rate law for this reaction is:

r = k[NO2][F2].

Hope this helps!

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 \(k[NO_2][F_2]\)

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