Basic chemical thermodynamics
The fourth edition of this widely acclaimed textbook provides a concise and easy-to-understand introduction to chemical thermodynamics. Beginning with an examination of equilibrium in familiar mechanical objects, the book gives a straightforward account of the factors that determine equilibrium in chemical systems. The underlying principles of thermodynamics are discussed, then applied to a wide range of physicochemical systems. The problems of non-ideal solutions and the concept of activity are covered, and the text offers a useful introduction to the molecular basis of thermodynamics. This new edition is fully illustrated, and features a clearer text design and larger format. Many new sample problems and worked examples are included. Students in thermodynamics will continue to find this popular book a clear introduction to an important subject.
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atm pressure behaviour benzene boiling point cell reaction change on combustion chemical potential chemical reactions chemical systems chemical thermodynamics components concentration consider constant pressure constant volume defined determine dilute solution dimer dissociation dwrev electrochemical cell enthalpies of formation entropy change equation equilibrium constant equilibrium mixture equilibrium position example expansion follows Raoult's Law free-energy change freezing point function gases Gibbs free energy heat capacity Henry's Law ideal solution illustrated in Fig internal energy irreversible isothermal maximum measure mechanical system melting molality molar mole fraction mole of gas mole of reaction molecular weight molecules n-butane naphthalene negative number of moles obtain partial pressure perfect gas phase position of equilibrium potential energy pure liquid pure substance Raoult's Law reactants relation reversible change RT\n section 4.4 solid solubility standard electrode potential system at constant temperature vapour pressure write zinc