   # A certain substance, initially present at 0.0800 M, decomposes by zero-order kinetics with a rate constant of 2.50 × 10 −2 mol/L·s. Calculate the time (in seconds) required for the system to reach a concentration of 0.0210 M. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 11, Problem 96CWP
Textbook Problem
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## A certain substance, initially present at 0.0800 M, decomposes by zero-order kinetics with a rate constant of 2.50 × 10−2 mol/L·s. Calculate the time (in seconds) required for the system to reach a concentration of 0.0210 M.

Interpretation Introduction

Interpretation: The initial and final concentration of a substance in a reactaion that follows the zero-order kinetics and the rate constant is given. By using these values, the time reaquired for the concentration change of substance is to be calculated.

Concept introduction: Rate of a chemical reaction which follows zero order kinetics, is independent of the concentration and time. In other words the rate does not change with concentration and time. Time taken between initial and final concentration can be calculated by the following expression:

[A]=[A]0kt

To determine: Time taken in the zero order reaction for the given concentration change.

### Explanation of Solution

Given

The initial concentration of reactant is 0.0800M .

The final concentration of reactant is 0.0210M .

The rate constant of reaction is 2.50×102mol/Ls .

The time required for the change in concentration is calculated using the formula,

[A]=[A]0kt

Where,

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

Substitute the values of [A]0, [A] and k in the above equation

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