For the reaction, 2A + B `to` products, when the concentrations of A and B both were doubled, the rate of the reaction increased from 0.3 mol `L^(-1)s^(-1)` to 2.4 mol `L^(-1)s^(-1).` When the concentration of A alone is doubled, the rate increased from 0.3 mol `L^(-1)s^(-1)` to 0.6 mol `L^(-1)s^(-1)`.
Which one of the following statements is correct ?

Options

A. Order of the reaction with respect to A is 2
B. Order of the reaction with respect to B is 1
C. Order of the reaction with respect to B is 2
D. Total order of the reaction is 4

Answer

C

Explanation

rate `=k [A]^(m) [B]^(n)`
So, `r_(1) =k [A]^(m) [B]^(n)`
`r_(2) =k [2A]^(m) [2B]^(n) rArr r_(3) =k [2A]^(m) [B]^(n) rArr (r_(2))/(r_(1))=8=2^(m+n)," so "m+n=3`
`(r_(3))/(r_(1))=2=2^(m)" so, "m=1," Hence "n=2`