Question

An aqueous solution (b) The half-life period for a first order reaction is 10 sec. How much time will it take to reduce the initial concentration of its 1/16 th value​

Answer 1

Answer:

THE ANSWER IS B

Explanation:

BEACAUSE THE HALF LIFE PERIOD FOR A FIRST ORDER REACTION

Answer 2

The time that will be taken  to reduce the initial concentration of the aqueous solution to its $1/16$  th value​ is,$40.01s$

Explanation:

• Half life is the time taken by the reactant to become half of its initial concentration.
• Half life of first order reaction is independent of the initial concentration of the substrate.
• Given the reaction is of first order and its half life is equal to ten seconds.
• Then,we need to find the time required to reduce the initial concentration of the substrate to $1/16$ th value​.
• The rate constant of the given reaction will be  $& {{t}_{1/2}}=\frac{0.693}{k} \\ & k=0.0693{{s}^{-1}}$

• Now,

$\[t=\frac{2.303}{0.0693}\log \frac{1}{1/16}=40.01s\]$