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Question

A reaction is first order in A and second order in B :
(i) Write differential rate equation.
(ii) How is the rate affected when the concentration of B is tripled?
(iii) How is the rate affected when the concentration of both A and B is doubled?

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Solution

It is given that a reaction is first order in A and second order in B.
i) The differential rate equation is as follows:
Rate =k[A][B]2
(ii) On increasing the concentration of B three times, rate becomes 9 times.
(d[B])2=32=9
(iii) When the concentrations of both A and B are doubled, rate becomes 8 times.
d[A](d[B])2=2×22=8

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