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Chapter 7: Problem 18

The half-life period of a first-order reaction is 10 minutes. The time required for the concentration of the reactant to change from \(0.08 \mathrm{M}\) to \(0.02 \mathrm{M}\) is (a) 10 minutes (b) 20 minutes (c) 30 minutes (d) 40 minutes

Short Answer

Expert verified
The time required for the concentration of the reactant to change from 0.08 M to 0.02 M is 20 minutes (option b).

Step by step solution

01

Understand the half-life concept

The half-life of a reaction is the time required for the concentration of the reactant to reduce to half its initial value. In a first-order reaction, the rate of reaction is directly proportional to the concentration of the reactant.
02

Apply the concept to the given problem

The half-life period given in the problem is 10 minutes. This means that 0.08 M would reduce to 0.04 M in 10 minutes.
03

Calculate the time for the required concentration change

To go from 0.04 M to 0.02 M, yet another half-life period would pass, which is another 10 minutes. Thus, the time required for the concentration to change from 0.08 M to 0.02 M would be twice the half-life period, or 20 minutes.

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Most popular questions from this chapter

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