A reaction was experimentally determined to follow the rate law, Rate = k[A] where k = 0.15 s^-1. Starting with [A]_o = 0.225M, how many seconds will it take for [A]_t = 0.0350M

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Quizplus · Accepted Answer

Given the rate law is first order, we can use the first-order kinetics equation: $t = \frac{1}{k} \ln \left(\frac{[A]_0}{[A]_t}\right)$. Substituting $k = 0.15 \, \text{s}^{-1}$, $[A]_0 = 0.225 \, \text{M}$, and $[A]_t = 0.0350 \, \text{M}$, we find $t \approx 12 \, \text{s}$.

A Reaction Was Experimentally Determined to Follow the Rate Law