In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,what is the half-life of the reaction?

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Quizplus · Accepted Answer

The half-life of a first-order reaction is given by $t_{1/2} = \frac{0.693}{k}$, where $k$ is the rate constant. To find $k$, we use the first-order rate law: $\ln\left(\frac{[A]_0}{[A]}\right) = kt$. Substituting the given values, $\ln\left(\frac{0.400}{0.250}\right) = k \times 15.0$, we can solve for $k$ and then calculate $t_{1/2}$. The calculation yields a half-life of approximately 22.1 minutes.

In the First-Order,reaction a → Products,[A] = 0