The time for half-life period of a certain reaction, `A rarr` products is `1 h`. When the initial concentration of the reactant `'A'` is `2.0 "mol" L^(-1)`, how much time does it take for its concentration to come from `0.50` to `0.25 "mol" L^(-1)`, if it is zero order reaction ?

Options

A. 4h
B. `0.5h`
C. `0.25h`
D. `1h`

Answer

C

Explanation

For a zero order reaction `k =(x)/(t)` ,brgt where x= amount decomposed .
k = zero order reaction `k=([A]_(0))/(2t_(1//2))`
since `[A_(0)]=2M,t_(1//2)=2hr , k=1`
` therefore ` from equation (1) , `t = (0.25)/(1)=0.25hr`