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.
All other sections in this Literature Study Guide are owned and copyrighted by BookRags, Inc.
Like water (H2, hydrogen peroxide is a compound of hydrogen and oxygen. However, as the its formula (H2O2) indicates, water are quite different. At room temperature, hydrogen peroxide is a pale-blue, syrupy, weakly acidic liquid. Pure, it is a stable compound, but any impurities, such as dust, may cause an explosive decomposition to oxygen and water. Since this explosive reaction is always a possibility, hydrogen peroxide is stored in bottles that allow the release of oxygen.
Typically, hydrogen peroxide is an oxidizing and reducing agent. As an oxidizing agent, it is used to oxidize particular water pollutants, such as hydrogen sulfide (H2S). For example, when hydrogen sulfide is exposed to hydrogen peroxide, it oxidizes to sulfate ion (SO42 ), which is not toxic.
In everyday life, hydrogen peroxide (a 3% solution) is used as an antiseptic. When hydrogen peroxide is applied to a superficial wound, it is reduced to oxygen and water by the action of a particular enzyme, catalase, which is found in blood and tissue.
Used as a hair bleach, hydrogen peroxide is also effective for bleaching paper pulp and textiles. It is also used in the manufacture of rocket fuels.