The rate law for a reaction of A, B and C has been found to be rate `= [A]^(2)[B][C]^((3)/(2))`. How would the rate of reaction change when
Concentration of [A] is reduced to `((1)/(3))` and concentration of [C] is quadrupled.

Options

A. `(2)/(3)`
B. `(4)/(3)`
C. `(4)/(9)`
D. `(8)/(9)`

Answer

c

Explanation

When `[A]=[(A)/(3)]` and [L] = [4L]
Rate `= k[(A)/(3)]^(2)[B][4L]^(3//2)`
Rate `=((8)/(9))(k[A]^(2)[B][L]^(3//2)) " "` ….(5)
Comparing (1) and (5) , rate is reduced to `(8)/(9)` times.