The rate law for the reaction `A+B rarr C` is found to be rate = `k [A]^2 [B]`. The rate constant of the reaction at `25^@C` is 6.25 `M^(-2)S^(-1)`. What is the rate of reaction, When `[A] = 0.1 mol.dm^(-3)` and `[B] = 0.2 mol.dm^(-3)`?

Options

A. Concentrations of A and B are both dobuled.
B. [A] is doubled and [B] is kept constant
C. [B] is dobuled and [A] is halved
D. [A] is kept constant and [B} is halved.