A first-order reaction has a rate constant of [tex]3.2 \times 10^{-5} \text{ s}^{-1}[/tex]. If the initial concentration of the reactant is [tex]0.0835 \text{ M}[/tex], what is the concentration after [tex]172 \text{ s}[/tex]?

A. The concentration after [tex]172 \text{ s}[/tex] is [tex]0.0346 \text{ M}[/tex].
B. The concentration after [tex]172 \text{ s}[/tex] is [tex]0.0546 \text{ M}[/tex].
C. The concentration after [tex]172 \text{ s}[/tex] is [tex]0.0646 \text{ M}[/tex].
D. The concentration after [tex]172 \text{ s}[/tex] is [tex]0.0746 \text{ M}[/tex].

The given data relates to first-order reaction kinetics and we use a specific formula to calculate the concentration after a certain time has passed. However, the answer options do not seem to match expected calculations.

Explanation:

In this question, a first-order reaction kinetics is presented. Using the given rate constant of 3.2×10-5 M/s and the initial concentration of the reactant, 0.0835 M, we are asked to calculate the concentration after a certain time, 172s, has passed. The general formula that is used to get the concentration of a reactant in a first-order reaction after a given

time is given as [A]t = [A]0e-kt, where [A]t represents the concentration after time t, [A]0 is the initial concentration, k is the rate constant, and t is the time. However, the options given do not directly provide the correct answer, suggesting that the values provided might be incorrect or additional calculation might be needed to determine the final concentration.

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