For a given reaction `A rarr ` Product, rate is `1xx10^(-4)M s^(-1)` when `[A]=0.01M` and rate is `1.41xx10^(-4)M s^(-1)` when `[A]=0.02 M`. Hence, rate law is `:`
A. `-(d[A])/(dt)=k[A]^(2)`
B. `-(d[A])/(dt)=k[A]`
C. `-(d[A])/(dt)=(k)/(4)[A]`
D. `-(d[A])/(dt)=k[A]^(1//2)`