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Chemistry Chemistry: An Atoms First Approach 2nd Edition

A form of Boyle’s law is PV = k (at constant T and n ) . Table 8-1 contains actual data from pressure−volume experiments conducted by Robert Boyle. The value of k in most experiments is 14.1 × 10 2 in Hg • in 3 . Express k in units of atm • L. In Example 8−3, k was determined for NH 3 at various pressures and volumes. Give some reasons why the k values differ so dramatically between Example 8-3 and Table 8-1.

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Chapter 8, Problem 125AE

Textbook Problem

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A form of Boyle’s law is PV = k (at constant T and n). Table 8-1 contains actual data from pressure−volume experiments conducted by Robert Boyle. The value of k in most experiments is 14.1 × 10² in Hg • in³. Express k in units of atm • L. In Example 8−3, k was determined for NH₃ at various pressures and volumes. Give some reasons why the k values differ so dramatically between Example 8-3 and Table 8-1.

Interpretation Introduction

Interpretation:

For the given details, it should be given the reason for the different values of k between example 8-3 and table 8-1 and value of K should be expressed in unit of atm. L.

Concept introduction:

Boyle’s law can be defined as,

A gas kept in the particular container at constant temperature. If the container of gas is compressed, the gaseous particle is compressed and the volume of container is decreased.. That is the volume of container is inversely proportional to the pressure of gas. As increasing the pressure of a particular gas the volume of gas will reduce. This indirect relationship between the pressure and volume of gas is termed as Boyles’s law.

Mathematically this law can be written as,

P ∝ V

PV=k

Where P is pressure and k is proportionality constant.

Explanation of Solution

Explanation

Value of K can be expressed in the unit of atm. L.as follows;

14.1×102in Hg.in3× 2.54cmin × 10mm1 cm × 1atm760 mm×(2

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Chapter 8 Solutions

Chemistry: An Atoms First Approach

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