For the reaction A+B `rarr` C+D doubling the concentration of both the reactants increases the reaction rate by eight times and doubling the concentration of only B simply doubles reaction the rate law is given as

Options

A. `r=k[A]^(1//2)[B]^(1//2)`
B. `r=k[A]^(1//2)[B]^(2)`
C. `r=k[A]^(2)[B]`
D. `r=k[A][B]`

Answer

C

Explanation

Given that `r=k[A]^(x)[B]^(y)…(1) 8r=k[2A]^(x)[2B]^(y) ..(2) 2r =k[A]^(x)[2B]^(y)..(3)`
on dividing Eq (1) by Eq (3) so the rate equation is r =k `[A]^(2) [B]`