Complete Question
The complete question is shown on the first uploaded image
Answer:
a
[tex]2NO_2 _{(g)} + F_2_{(g)} ----> 2NO_2 F_{(g)}[/tex]
b
[tex]r = \frac{ k [NO_2]^2 [F_2]}{[NO_2F]}[/tex]
Explanation:
From the question we are told that
The formation mechanism is
[tex]NO_2_{(g)} + F_2 _{(g)} ----> NO_2 F_{(g)} + F_{(g)}[/tex]
[tex]F_{(g)} + NO_2 _{(g)} ---> NO_2 F_{(g)}[/tex]
The overall balanced equation is
[tex]2NO_2 _{(g)} + F_2_{(g)} ----> 2NO_2 F_{(g)}[/tex]
We combined the first reactant and the last product and the balanced the number of mole
The observable rate law is
[tex]r = \frac{ k [NO_2]^2 [F_2]}{[NO_2F]}[/tex]
This rate law is derived from the balanced chemical equation
