   Chapter 13.5, Problem 2.2ACP

Chapter
Section
Textbook Problem

If the CO2 in the headspace escapes into the atmosphere where the partial pressure of CO2 is 3.7 × 10−4 atm, what volume would the CO2 occupy (at 25 °C)? By what amount did the CO2 expand when it was released?

Interpretation Introduction

Interpretation: The volume of CO2 and the amount did the carbon dioxide expand when it was released has to be determined.

Concept introduction:

Boyle’s law states that the pressure (P) of a given quantity of gas varies inversely with its volume (V) at constant temperature.

PV=ConstantP1V1=P2V2

Explanation

Given that the initial partial pressure (P1) of the gas is 4.0atm and the volume is 0.025L.

The given value of partial pressure of the gas is taken as the final partial pressure (P2)

Substituting the known values in the equation P1V1=P2V2

Therefore,

4.0atm(0.025L)=3.7×10-4atm(V2)V2 =4

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 