A second-order reaction (2A $\rightarrow$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 for a second-order reaction is given by $ t_{1/2} = \frac{1}{k[A]_0} $. Rearranging for $[A]_0$, we get $[A]_0 = \frac{1}{k \cdot t_{1/2}} = \frac{1}{0.350 \, \text{M}^{-1}\text{s}^{-1} \cdot 3.45 \, \text{s}} = 0.828 \, \text{M} $.

A Second-Order Reaction (2A →\rightarrow→ B) with a Rate Constant of 0

A Second-Order Reaction (2A $\rightarrow$ B) with a Rate Constant of 0