Question

For the second-order reaction below, the initial concentration of reactant A is 0.24 M. If the rate constant for the reaction is 1.5 x10–2 M–1s–1, what is the concentration of A after 265 seconds?2A --> B + Crate = k[A]20.12 M0.19 M0.95 M4.0 M5.2 M

Answer 1

Answer:

Concentration of A after 265 seconds is 0.12 M

Explanation:

Integrated rate law for the given second order reaction is-

                            $\frac{1}{[A]}=\frac{1}{[A]_{0}}+kt$

where [A] is concentration of A after "t" time, $[A]_{0}$ is intital concentration of A and k is rate constant.

Here $[A]_{0}$ is 0.24 M, k is 0.015 $M^{-1}S^{-1}$ and t is 265 S

Plug in all the values in the above equation-

                               $\frac{1}{[A]}=\frac{1}{0.24}+(0.015\times 265)$

                              or, [A] = 0.12

So concentration of A after 265 seconds is 0.12 M