The rate constant for a second-order reaction is 0.54 M-1s-1. What is the half-life of this reaction if the initial concentration is 0.39 M

4.748 seconds

Explanation:

second-order is one in which the rate is proportional to the square of the concentration of one reactant. This can be expressed below;

2A>P

Where

A is the reactant.

P is the product.

The rate can be expressed as

Rate= k[A]^2

Half-life reffers to time required to reduce the concentration of reactant to half of its initial value.

The half life of reaction can be calculated using below formula

Half-life =. 1/(K*I)

Where,

K = Rate constant = 0.54 1/ms

I = Initial concentration = 0.39 m

If we substitute these values we have

Half-life t(1/2) =1/(0.54×0.39)

=4.748 seconds

Therefore, the half life is 4.748 seconds

the answer would be b i believe