Answer:
The expected ratio of half-lives for a reaction will be 5:1.
Explanation:
Integrated rate law for zero order kinetics is given as:
[tex]k=\frac{1}{t}([A_o]-[A])[/tex]
[tex][A_o][/tex] = initial concentration
[A]=concentration at time t
k = rate constant
if, [tex][A]=\frac{1}{2}[A_o][/tex]
[tex]t=t_{\frac{1}{2}}[/tex], the equation (1) becomes:
[tex]t_{\frac{1}{2}}=\frac{[A_o]}{2k}[/tex]
Half life when concentration was 0.05 M=[tex]t_{\frac{1}{2}}[/tex]
Half life when concentration was 0.01 M=[tex]t_{\frac{1}{2}}'[/tex]
Ratio of half-lives will be:
[tex]\frac{t_{\frac{1}{2}}}{t_{\frac{1}{2}}'}=\frac{\frac{[0.05 M]}{2k}}{\frac{[0.01 M]}{2k}}=\frac{5}{1}[/tex]
The expected ratio of half-lives for a reaction will be 5:1.
