Question

Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) (g) Suppose also ≫. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction.

Answer 1

Complete Question

The complete question is shown on the first uploaded image  

Answer:

a

  $2NO_2 _{(g)} + F_2_{(g)} ----> 2NO_2 F_{(g)}$

b

  $r = \frac{ k [NO_2]^2 [F_2]}{[NO_2F]}$

Explanation:

      From the question we are told that

          The formation mechanism is  

                      $NO_2_{(g)} + F_2 _{(g)} ----> NO_2 F_{(g)} + F_{(g)}$

                      $F_{(g)} + NO_2 _{(g)} ---> NO_2 F_{(g)}$

The overall balanced equation is

              $2NO_2 _{(g)} + F_2_{(g)} ----> 2NO_2 F_{(g)}$

We combined the first reactant and the last product and the balanced the number of mole

     The observable rate law is

                 $r = \frac{ k [NO_2]^2 [F_2]}{[NO_2F]}$

This rate law is derived from the balanced chemical equation