2NO2(g)+F2(g)→NO2F(g) ΔH∘rxn=−284kJ/molrxn

NO2(g) and F2(g) can react to produce NO2F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below.

Step 1: NO2+F2→NO2F+F (slow)

Step 2: NO2+F→NO2F (fast)
(a) Write a rate law for the overall reaction that is consistent with the proposed mechanism.

(b) On the incomplete reaction energy diagram below, draw a curve that shows the following two details.

The relative activation energies of the two elementary steps
The enthalpy change of the overall reaction