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For a reaction : A+B Products, the rate of the reaction at various concentrations are given below:

Expt No[A][B]rate (mol dm3s1)
10.20.22
20.20.44
30.60.436
The rate law for the above reaction is :

A
r=K[A]2[B]
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B
r=K[A][B]2
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C
r=K[A]3[B]
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D
r=K[A]2[B]2
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Solution

The correct option is A r=K[A]2[B]
From second and third experiment, we observe that when the concentration of B is kept constant at 0.4 M and the concentration of A is trebled from 0.2 M to 0.6 M, the rate increases 9 times from 4 to 36. Hence, the order of the reaction with respect to A is 2.
From first and second experiment, we observe that when the concentration of A is kept constant at 0.2 M and the concentration of A is doubled from 0.2 M to 0.4 M, the rate doubles from 2 to 4. Hence, the order of the reaction with respect to B is 1.
The rate law for the reaction is r=K[A]2[B]

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