powered by CoolJargon
  • Gas Pressure
  • Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
  • Stoichiometry of Gaseous Substances, Mixtures, and Reactions
  • Effusion and Diffusion of Gases
  • The Kinetic-Molecular Theory
  • Non-Ideal Gas Behavior
class="key-equations" title="Key-Equations" class="summary" title="Chapter Summary" class="exercises" title="Exercises" class="references" title="References"
The hot air inside these balloons is less dense than the surrounding cool air. This results in a buoyant force that causes the balloons to rise when their guy lines are untied. (credit: modification of work by Anthony Quintano)
A photograph shows about twenty colorful hot air balloons at varying stages of inflation. Some are deflated, while others are inflated. Three of the balloons are off the ground and are visible against a bright blue sky.

We are surrounded by an ocean of gas—the atmosphere—and many of the properties of gases are familiar to us from our daily activities. Heated gases expand, which can make a hot air balloon rise ([link]) or cause a blowout in a bicycle tire left in the sun on a hot day.

Gases have played an important part in the development of chemistry. In the seventeenth and eighteenth centuries, many scientists investigated gas behavior, providing the first mathematical descriptions of the behavior of matter.

In this chapter, we will examine the relationships between gas temperature, pressure, amount, and volume. We will study a simple theoretical model and use it to analyze the experimental behavior of gases. The results of these analyses will show us the limitations of the theory and how to improve on it.

© Feb 24, 2016 OpenStax College. Textbook content produced by OpenStax College is licensed under a Creative Commons Attribution License 4.0 license.

Download for free at http://cnx.org/contents/85abf193-2bd2-4908-8563-90b8a7ac8df6@9.124.