The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.293 M. What is the value of k for this reaction?

Answer 1

For a second-order reaction, we can use the following integrated rate law equation:

1/[A]t - 1/[A]0 = kt

where: [A]t = concentration of A at time t (0.293 M) [A]0 = initial concentration of A (0.740 M) t = time elapsed (13.5 s) k = rate constant (unknown)

Plugging in the values:

1/0.293 - 1/0.740 = k * 13.5

Let's calculate the value of k:

(3.416 - 1.351) / 13.5 = k 2.065 / 13.5 = k k ≈ 0.153

So the value of the rate constant, k, for this second-order reaction is approximately 0.153 M⁻¹s⁻¹.