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Question

A reaction : A2+B Products, involves the following mechanism :
A2 2A (fast)                 (A being the intermediate)
A+Bk2(slow).The rate law consistent to this mechanism is :



A

rate=k[A2][B]

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B

rate=k[A2]2[B]

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C

rate=k[A2]12[B]

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D

rate=k[A2][B]2

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Solution

The correct option is B

rate=k[A2]12[B]


From the slow step : rate =k2[A][B] ...............(i)

From fast step : Ke=[A]2[A2]or [A]=K12eA12 ..............(ii)


From (i) and (ii) rate =k2k12e[A2]12[B]=k[A2]12[B]


Chemistry

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