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

Explanation

(i) rate ` = - (dx)/(dt) = k[A]^(1) [B]^(2)`
(ii) rate ` = k[A]^(!) [3B]^(2) = 9k[A]^(1) [B]^(2)`. Rate increases by 9 times.
(iii) `r = k[2A]^(1) [2B]^(2) = 8k [A}^(1) [B]^(2)` . Rate increases by 8 times.