A second-order reaction (2A B) with a rate constant of 0.350 M ^-1s ^-1 is found to have a half-life of 3.45 s. What was the initial concentration of the reactant, [A]₀?

Question

Quizplus · Accepted Answer

The half-life of a second-order reaction can be calculated using the equation:
t1/2 = 1 / k[A]0

Where t1/2 is the half-life, k is the rate constant, and [A]0 is the initial concentration of the reactant.

Rearranging this equation, we can solve for [A]0:

[A]0 = 1 / (k * t1/2)

Plugging in the given values:

[A]0 = 1 / (0.350 M^-1s^-1 * 3.45 s)
[A]0 = 0.828 M

Therefore, the initial concentration of the reactant was 0.828 M. So the answer is A.

A Second-Order Reaction (2A B) with a Rate Constant