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Question

For the reaction: A+B→C+D, doubling the concentration of both the reactants increases the reaction rate by 8 times and doubling the concentration of only B simply doubles the reaction rate. The rate law is given as:

A
r=k[A]12[B]12
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B
r=k[A][B]2
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C
r=k[A]2[B]
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D
r=k[A][B]
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Solution

The correct option is C r=k[A]2[B]r=kaαbβ ...(i) 8r=k(2a)α(2b)β ..(ii) 2r=kaα(2b)β ...(iii) Dividing eqn (ii) by eqn (iii) gives 82=2α 2α=4=22, α=2 Dividing eqn (iii) by eqn (i) gives 2=2β or β=1 Hence, rate = k[A]2[B]

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