Suppose the reaction between nitric oxide and bromine proceeds by the

following mechanism:

Write the balanced

chemical equation for the

overall chemical reaction:

step

rate constant

elementary reaction

NO(g) + Br₂(9) NOBr₂(9)

1

k₁

2

NOBr₂(g) + NO(g) → 2 NOBr(g)

k₂

Suppose also k₁«k₂. That is, the first step is much slower than the second.

Write the experimentally-

observable rate law for the

overall chemical reaction.

Note: your answer should

not contain the

concentrations of any

intermediates.

Express the rate constant

k for the overall chemical

reaction in terms of k₁, K₂,

and (if necessary) the rate

constants k.1 and K-2 for

the reverse of the two

elementary reactions in

the mechanism.

0

rate=&

10

-

-0

ローロ

olo

11

8

X

G

Ar

12