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

F(g)+NO_2(g)---->NO_2F(g)

Step-by-step explanation:

Answer retrieved from ALEKS

Answer 2

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 = ( k [NO_2]^2 [F_2])/([NO_2F])`

Step-by-step 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 = ( k [NO_2]^2 [F_2])/([NO_2F])`

This rate law is derived from the balanced chemical equation