The following sections of this BookRags Literature Study Guide is offprint from Gale's For Students Series: Presenting Analysis, Context, and Criticism on Commonly Studied Works: Introduction, Author Biography, Plot Summary, Characters, Themes, Style, Historical Context, Critical Overview, Criticism and Critical Essays, Media Adaptations, Topics for Further Study, Compare & Contrast, What Do I Read Next?, For Further Study, and Sources.
(c)1998-2002; (c)2002 by Gale. Gale is an imprint of The Gale Group, Inc., a division of Thomson Learning, Inc. Gale and Design and Thomson Learning are trademarks used herein under license.
The following sections, if they exist, are offprint from Beacham's Encyclopedia of Popular Fiction: "Social Concerns", "Thematic Overview", "Techniques", "Literary Precedents", "Key Questions", "Related Titles", "Adaptations", "Related Web Sites". (c)1994-2005, by Walton Beacham.
The following sections, if they exist, are offprint from Beacham's Guide to Literature for Young Adults: "About the Author", "Overview", "Setting", "Literary Qualities", "Social Sensitivity", "Topics for Discussion", "Ideas for Reports and Papers". (c)1994-2005, by Walton Beacham.
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Boyle's law is one of the gas laws. It states that at constant temperature, the volume of a fixed mass of gas is inversely proportional to the pressure. The other way of expressing this l aw is pV = constant, where p is the pressure and V is the volume of the gas. It is named after British physicist and chemist Robert Boyle (1627-1691).
Boyle's law is sometimes known as the constant temperature law. It can be combined with Charles' law and the pressure law to give t he ideal gas law (also known as the universal gas law), pV = nRT, where p is pressure, V is volume, n is the number of moles of gas, R is the universal gas constant, and T is temperature.
Boyle's law is an approximation and works perfectly only for an ideal(theoretical) gas. In practice it works best at low pressures but once the pressures become high the predictions become less accurate. This inaccuracy is due to the size of the gas molecules and weak intermolecular forces, such as van der Waals fo rces. At high pressures the molecules are forced together whereas at low pressures the molecules are free to move with very little interaction from neighboring molecules.
Boyle's law is a good indicator of how a gas will react if the temperature is kept constant and the pressure and volume are altered.