Question

Suppose the formation of nitryl fluoride proceeds by the following mechanism:

Step. Elementary reaction. Rate constant
1. NO2(g)+F2(g)=NO2F(g)+F(g). K1
2. F(g)+NO2(g)=NO2F(g). K2
Suppose also k1<
Write the balanced chemical equation for the overall chemical reaction:

Write the experimentally observable rate law for the overall chemical reaction:
Note your answer should not contain concentrations or any intermediates.

Express the rate constant k for the overall chemical reaction in terms of k1, k2, and If necessary the rate constants k-1 and k-2 for the reverse of two elementary reactions in the mechanism.

Answer 1

The balanced chemical equation for the overall chemical reaction is 2NO2(g) + F2(g) → 2NO2F(g). The experimentally observable rate law for the overall chemical reaction is Rate = k [NO2]^2 [F2]. The rate constant k for the overall chemical reaction can be expressed in terms of k1, k2, k-1, and k-2 as k = k1 (k2/k-1).

Step-by-step explanation:

The balanced chemical equation for the overall chemical reaction is:

2NO2(g) + F2(g) → 2NO2F(g)

The experimentally observable rate law for the overall chemical reaction is:

Rate = k [NO2]2 [F2]

The rate constant k for the overall chemical reaction can be expressed in terms of k1, k2, k-1, and k-2 as:

k = k1 (k2/k-1)