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.

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okpalawalter8 okpalawalter8 · Answer 1 · 2020-05-30T02:35:12+02:00

Complete Question

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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