A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
(i) Doubled
(ii) reduced to half ?

Explanation

(i) ` r = k[A]^(2) rArr r = k[2A]^(2) rArr r 4k[A]^(2)`
Rate increases by four times.
(ii) ` r = k[A]^(2)`
`r = k[(A)/(2)]^(2) rArr = (1)/(4) k[A]^(2)`. Rate increases by four times.