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Question

The rate of reaction; A+2BProducts is given by,

d[A]dt=k[A][B]2. If B is present in large excess, the order of reaction is:

A
3
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B
2
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C
1
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D
zero
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Solution

The correct option is C 1

The given relation is:

A+2BProduct

Rate d[A]dt=k[A][B]2 (given)

If [B] is present in large excess, then change in concentration of [B] does no alter the rate means rate becomes independent on [B]

Hence order is counted only for [A]1

Overall order =1


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