000			03487nam a2200241ui 4500
001			UK0620923120
003			OSt
008			110329s2011 us d f 001 00eng d
020			_a978-0-470-52264-6
040			_aUCA-CYT _cUCA
100	1		_aRogers, Donald W.
245	1	0	_aConcise physical chemistry / _cDonald W. Rogers
260			_aNew Jersey : _bJohn Wiley & Sons, _c2011
300			_aXXIV, 378 p. : _bgráf. ; _c24 cm
500			_aÍndice
520			_aINDICE: Chapter 1 Ideal Gas Laws. 1.1 Empirical Gas Laws. 1.2 The Mole. 1.3 Equations of State. 1.4 Dalton's Law. 1.5 The Mole Fraction. 1.6 Extensive and Intensive Variables. 1.7 Graham's Law of Effusion. 1.8 The Maxwell-Boltzmann Distribution. 1.9 A Digression on 'Space'. 1.10 The Sum-Over-States or Partition Function. Chapter 2 Real Gases: Empirical Equations. 2.1 The van der Waals Equation. 2.2 The Virial Equation: A Parametric Curve Fit. 2.3 The Compressibility Factor. 2.4 The Critical Temperature. 2.5 Reduced Variables. 2.6 The Law of Corresponding States, Another View. 2.7 Compressibility Factors Calculated From the van der Waals Constants. 2.8 Boyle's Law Plot for an Ideal Gas (lower curve) and for Nitrogen (upper curve). 2.9 Determining the Molecular Weight of a Nonideal Gas. Chapter 3 The Thermodynamics of Simple Systems. 3.1 Conservation Laws and Exact Differentials. 3.2 Thermodynamic Cycles. 3.3 Line Integrals in General. 3.3 Pythagorean Approximation to the Short Arc of a Curve. 3.4 Thermodynamic States and Systems. 3.5 State Functions. 3.6 Reversible Processes and Path Independence. 3.7 Heat Capacity. 3.8 Energy and Enthalpy. 3.9 The Joule and Joule-Thomson Experiments. 3.10 The Heat Capacity of an Ideal Gas. 3.11 Adiabatic Work. Chapter 4 Thermochemistry. 4.1 Calorimetry. 4.2 Energies and Enthalpies of Formation. 4.3 Standard States. 4.4 Molecular Enthalpies of Formation. 4.5 Enthalpies of Reaction. 4.6 Group Additivity. 4.7 from Classical Mechanics. 4.8 The Schroedinger Equation. 4.9 Variation of with T. 4.10 Differential Scanning Calorimetry. Chapter 5 Entropy and the Second Law. 5.1 Entropy. 5.2 Entropy Changes. 5.3 Spontaneous Processes. 5.4 The Third Law. Chapter 6 The Gibbs Free Energy. 6.1 Combining Enthalpy and Entropy. 6.2 Free Energies of Formation. 6.3 Some Fundamental Thermodynamic Identities. 6.4 The Free Energy of Reaction. 6.5 Pressure Dependence of the Chemical Potential. 6.6 The Temperature dependence of the Free Energy. Chapter 7 Equilibrium. 7.1 The Equilibrium Constant. 7.2 General Formulation. 7.3 The Extent of Reaction. 7.4 Fugacity and Activity. 7.5 Variation of the Equilibrium Constant with Temperature. 7.6 Computational Thermochemistry. 7.7 Chemical Potential: Nonideal Systems. 7.8 Free Energy and Equilibria in Biochemical Systems. Chapter 8 A Statistical Approach to Thermodynamics. 8.1 Equilibrium. 8.2 Degeneracy and Equilibrium. 8.3 Gibbs Free Energy and the Partition Function. 8.4 Entropy and Probability. 8.5 The Thermodynamic Functions. 8.6 The Partition Function of a Simple System. 8.7 The Partition Function for Different modes of Motion. 8.8 The Equilibrium Constant: A Statistical Approach. 8.9 Computational Statistical Thermodynamics. Chapter 9 The Phase Rule. 9.1 Components, Phases, and Degrees of Freedom. 9.2 Coexistance Curves. 9.3 The Clausius-Cl
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