Question

A certain reaction has the following general form.

aA → bB
At a particular temperature and [A]0 = 2.57 ✕ 10-3 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of +3.39 ✕ 10-2 L/mol · s.

(b) Calculate the half-life for this reaction.

(c) How much time is required for the concentration of A to decrease to 7.43 ✕ 10-4 M?

Answer 1

Rate law: r= k[A]^2

Integrated rate law: 1/[A] = kt + 1/[A]0

Rate constant: k= 3.40x10^-2 L/mol*s

Step-by-step explanation:

Hello,

In this case, since the slope is obtained by plotting 1/[A] and it has the units L/(mol*s) or 1/(M*s), we can infer the reaction is second-order, therefore, its rate law is:

The integrated rate law:

That is obtained from the integration of:

And of course, since the slope equals the rate constant, its value is: