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A first order reaction has 1/16 of the original amount left after 500 seconds. What is the half-life of the reactant in this reaction

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A first order reaction, with a half-life of 125 s, has 1/16 of the original amount left after 500 seconds.

What is a first order reaction?

It is a chemical reaction in which the rate of reaction is directly proportional to the concentration of the reacting substance.

First, we will calculate the rate constant using the following expression.

ln ([A]/[A]₀) = - k × t

ln (1/16[A]₀/[A]₀) = - k × 500 s

k = 5.55 × 10⁻³ s⁻¹

where,

  • [A] is the final concentration of the reactant.
  • [A]₀ is the initial concentration of the reactant.
  • k is the rate constant.
  • t is the elapsed time.

Next, we can calculate the half-life (th) using the following expression.

th = ln 2 / k = ln 2 / (5.55 × 10⁻³ s⁻¹) = 125 s

A first order reaction, with a half-life of 125 s, has 1/16 of the original amount left after 500 seconds.

Learn more about first order reactions here: https://brainly.com/question/518682

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