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Question

For the reaction : aA+bB Products, the rate law is given by Rate = k[A]m[B]n. On making the concentration of A two-fold and halving that of B, the ratio of the new rate to the earlier rate of the reaction would be:


A

n1

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B

m+n

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C

2(m+n)

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D

2(mn)

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Solution

The correct option is D

2(mn)


(Rate)1=k[A]w[B]n;(Rate)2=k(2[A])w([B]2)n


Hence,(rate)2(rate)1=2m×(12)n=2mn


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