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.