G The decomposition reaction of A to B is a first-order reaction with a half-life of 2.42×103 seconds: A → 2B If the initial concentration of A is 0.163 M, how many minutes will it take for the concentration of A to be 66.8% of the initial concentration?

In 23.49 minutes the concentration of A to be 66.8% of the initial concentration.

Explanation:

The equation used to calculate the constant for first order kinetics:

.....(1)

Rate law expression for first order kinetics is given by the equation:

......(2)

where,  

k = rate constant

=Half life of the reaction =

t = time taken for decay process = ?

= initial amount of the reactant = 0.163 M

[A] = amount left after time t =  66.8% of

[A]=

t = 1,409.19 s

1 minute = 60 sec

In 23.49 minutes the concentration of A to be 66.8% of the initial concentration.