The rate expression for the reaction `A_((g)) + B_((g)) rarr C_((g))" is rate" = k[A]^(2)[B]^(1//2)`. What changes in the initial concentrations of A and B will cause the rate of reaction to increase by a factor of eight?

Options

A. [A`]=[A] : [B`] = 2[B]
B. [A`]=2[A] : [B`] = 4[B]
C. [A`]=[A] : [B`] = 4[B]
D. [A`] = 4[A] : [B`] = [B]

Answer

b

Explanation

Given `r= k[A]^2[B]^(1//2)`
new rate will be 8 times when [A]. = 2[A] and [B]. = 4[B]
now `r. = [2A]^(2)[48]^(1//2)` = 8[A][B]