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Question

For reaction: A + B Products, the rate if the reaction at various concentration are given below:

Expt. No.(A)(B)Rate10.20.2220.20.4430.60.436


A

Rate=k[A]2[B]2

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B

Rate=k[A]2[B]

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C

Rate=k[A][B]2

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D

Rate=k[A]3[B]

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Solution

The correct option is B

Rate=k[A]2[B]


Let the rate law be r=k[A]x[B]y
Divide (2) by (1)
2=[2]y,y=1
Divide (3) by (2)
9=(3)x,x=2
Hence rate equation, R=k[A]2[B]1


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