Question

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?

Answer 1

Answer:

ANSWER

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