Question

2A → B + C

The above reaction is run and found to follow second order kinetics with a rate constant of 1.30 x 10^-3 M^-1sec^-1. If the initial concentration of A is 1.45 M, what is the concentration after 142 seconds?

Answer 1

Since the reaction is second order and we have to find final concentration after 142 second, we can use integrated rate equation for the second order.

Equation:

1/[A]_t = kt + 1/ [A]₀

Here subscript t and 0 are shown for concentration at time t and present initially respectively.

k is rate constant and t is time.

Lets plug in the given values in order to get [A]_t

1/[A]_t = (1.30 E-3 per M per s x 142 s ) + 1/ 1.45 M

We have to calculate value of [A]_t

[A]_t= 1.14 M