Question

the half life period of a zero order reaction A,,- product is

Answer 1

t 1/2 of a Zero order reaction is: a/2k
Where, a=initial concentration, k=rate constant.

Answer 2

Answer:$t_\frac{1}{2}=\frac{[a_0]}{2k}$

Explanation: $A\rightarrow Products$

$rate=k[A]^0$    (1)

also$rate=-\frac{d[A]}{dt}$    (2)

equating (1) and (2) 

$k=-\frac{d[A]}{dt}$       $([A]^0=1)$

$kdt=-{d[A]}$

Integrating both sides and putting the limits for time as t=0 to t=t and for concentration from $[A]=[a_0]$ to $[A]=[a]$

Rate law expression for zero order kinetics is given by:

where, t = time taken for decomposition

k = rate constant

$[a_0]$ = initial concentration

$[a]$ = concentration left after time t

Half life period is the time taken to reduce the original reactants to half of its value.

$t=t_\frac{1}{2}$,  $[a]=\frac{[a_0]}{2}$

$t_\frac{1}{2}=\frac{[a_0]-\frac{[a_0]}{2}}{k}$

$t_\frac{1}{2}=\frac{[a_0]}{2k}$