Under the same reaction conditions, the intial concentration of `1.386 mol dm^(-3)` of a substance becomes half in `40 s` and `20 s` theough first order and zero order kinetics, respectively.
The ratio `(k_(1)//k_(0))` of the rate constants for first order `(k_(1))` and zero order `(k_(0))` of the reaction is

Options

A. `0.5" mol"^(-1)" dm"^(3)`
B. `1.0" mol dm"^(-3)`
C. `1.5" mol dm"^(-3)`
D. `2.0" mol"^(-1)" dm"^(3)`

Answer

A

Explanation

`k_(1) =(0.693)/(40) r_(o) =(1.386)/(2xx20) (k_(1))/(r_(o))=0.5" mol"^(-1)" dm"^(3)`