A reaction is first order in A and second order in B. (i) Write the differential rate equation. (ii) How is the rate affected on increasing the concentration of B three times? (iii) How is the rate affected when the concentrations of both A and B are doubled?
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It is given that a reaction is first order in AA and second order in BB.
i) The differential rate equation is as follows:
Rate \displaystyle = k[A][B]^2=k[A][B]
2
(ii) On increasing the concentration of BB three times, rate becomes 99 times.
\displaystyle (d[B])^2 = 3^2 = 9(d[B])
2
=3
2
=9
(iii) When the concentrations of both AA and BB are doubled, rate becomes 88 times.
\displaystyle d[A] (d[B])^2 = 2 \times 2^2 = 8d[A](d[B])
2
=2×2
2
=8
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