Thus a change in a state function depends on only the difference between the initial and final states, not the pathway used to go from one to the other. In Chapter 5 "Energy Changes in Chemical Reactions", we also introduced the concept of a state function A property of a system whose magnitude depends on only the present state of the system, not its previous history., a property of a system that depends on only the present state of the system, not its history. (For more information on reaction rates and kinetics, see Chapter 14 "Chemical Kinetics".)Įquation 18.1 system + surroundings = universeĪ closed system, such as the contents of a sealed jar, cannot exchange matter with its surroundings, whereas an open system can in this case, we can convert a closed system (the jar) to an open system by removing the jar’s lid. The rate of a reaction and its pathway are described by chemical kinetics. It does not, however, say anything about whether an energetically feasible reaction will actually occur as written, and it tells us nothing about the reaction rate or the pathway by which it will occur. Thermodynamics tells chemists whether a particular reaction is energetically possible in the direction in which it is written, and it gives the composition of the reaction system at equilibrium. (from the Greek thermo and dynamic, meaning “heat” and “power,” respectively), the study of the interrelationships among heat, work, and the energy content of a system at equilibrium. Our goal in this chapter is to extend the concepts of thermochemistry to an exploration of thermodynamics The study of the interrelationships among heat, work, and the energy content of a system at equilibrium. In Chapter 5 "Energy Changes in Chemical Reactions", you also learned about thermochemistry, the study of energy changes that occur during chemical reactions. For example, the energy stored in chemical bonds can be released as heat during a chemical reaction. (For more information on energy, see Chapter 5 "Energy Changes in Chemical Reactions".) Instead, energy takes various forms that can be converted from one form to another. The second, the law of conservation of energy, states that energy can be neither created nor destroyed. (For more information on matter, see Chapter 1 "Introduction to Chemistry".) The law of conservation of mass is the basis for all the stoichiometry and equilibrium calculations you have learned thus far in chemistry. The first of these, the law of conservation of mass, states that matter can be neither created nor destroyed. zip file containing this book to use offline, simply click here.Ĭhemical reactions obey two fundamental laws. You can browse or download additional books there. More information is available on this project's attribution page.įor more information on the source of this book, or why it is available for free, please see the project's home page. Additionally, per the publisher's request, their name has been removed in some passages. However, the publisher has asked for the customary Creative Commons attribution to the original publisher, authors, title, and book URI to be removed. Normally, the author and publisher would be credited here. This content was accessible as of December 29, 2012, and it was downloaded then by Andy Schmitz in an effort to preserve the availability of this book. See the license for more details, but that basically means you can share this book as long as you credit the author (but see below), don't make money from it, and do make it available to everyone else under the same terms. This book is licensed under a Creative Commons by-nc-sa 3.0 license.
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