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Question

A two-step mechanism has been suggested for the reaction of nitric oxide and bromine.
NO(g)+Br2(g)K1NOBr2(g)
NOBr2(g)+NO(g)K22NOBr(g)
The observed rate law is, rate =k[NO]2[Br2]. Hence, the rate-determining step is :

A
NO(g)+Br2(g)NOBr2(g)
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B
NOBr2(g)+NO(g)2NOBr(g)
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C
2NO(g)+Br2(g)2NOBr(g)
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D
none of these
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Solution

The correct option is B NOBr2(g)+NO(g)2NOBr(g)
NO(g)+Br2(g)k1NOBr2(g) .....(i)
NOBr2(g)+NO(g)k2−−RDS2NOBr2(g) .....(ii)
Rate = k2 [NOBr2][NO]
Since, NOBr2 is the reactive intermediate, so its constant ratio is dertermined from step (i).
k1orkeq=[NOBr2][NO][Br2]
or [NOBr2]=k1[NO][Br2]
Substitute the [NOBr2] in step (iii),
Rate = k1k2[NO]2[Br2]=K[NO]2[Br2]

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