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جداسازی اجزای قطران زغال سنگ (فنانترن)با استفاده از سیالات فوق بحرانی
اسماعیل زاده، فریدون.
اطلاعات کتابشناختی
جداسازی اجزای قطران زغال سنگ (فنانترن)با استفاده از سیالات فوق بحرانی
پدیدآور اصلی :
اسماعیل زاده، فریدون.
ناشر :
صنعتی شریف
سال انتشار :
1380
موضوع ها :
آنتراسن Anthracene فنانترن Phenanthrene کربازول Carbazole سیال فوق بحرانی Supercritical...
شماره راهنما :
06-33899
جستجو در محتوا
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فهرست مطالب
Cover
(1)
Title Page
(5)
Copyright Page
(6)
Preface
(9)
Contents
(15)
Chapter 1: Measured Thermodynamic Propertiesand Other Basic Concepts
(19)
Learning Objectives
(19)
1.1 Thermodynamics
(20)
1.2 Preliminary Concepts—The Language of Thermo
(21)
Thermodynamic Systems
(21)
Properties
(22)
Processes
(23)
Hypothetical Paths
(24)
Phases of Matter
(24)
Length Scales
(24)
Units
(25)
1.3 Measured Thermodynamic Properties
(25)
Volume (Extensive or Intensive)
(25)
Temperature (Intensive)
(26)
Pressure (Intensive)
(29)
The Ideal Gas
(31)
1.4 Equilibrium
(33)
Types of Equilibrium
(33)
Molecular View of Equilibrium
(34)
1.5 Independent and Dependent Thermodynamic Properties
(35)
The State Postulate
(35)
Gibbs Phase Rule
(36)
1.6 The PvT Surface and Its Projections for Pure Substances
(38)
Changes of State During a Process
(40)
Saturation Pressure vs. Vapor Pressure
(41)
The Critical Point
(42)
1.7 Thermodynamic Property Tables
(44)
1.8 Summary
(48)
1.9 Problems
(49)
Conceptual Problems
(49)
Numerical Problems
(52)
Chapter 2: The First Law of Thermodynamics
(54)
Learning Objectives
(54)
2.1 The First Law of Thermodynamics
(55)
Forms of Energy
(55)
Ways We Observe Changes in U
(57)
Internal Energy of an Ideal Gas
(58)
Work and Heat: Transfer of Energy Between the System and the Surroundings
(60)
2.2 Construction of Hypothetical Paths
(64)
2.3 Reversible and Irreversible Processes
(66)
Reversible Processes
(66)
Irreversible Processes
(66)
Efficiency
(73)
2.4 The First Law of Thermodynamics for Closed Systems
(73)
Integral Balances
(73)
Differential Balances
(75)
2.5 The First Law of Thermodynamics for Open Systems
(78)
Material Balance
(78)
Flow Work
(78)
Enthalpy
(80)
Steady-State Energy Balances
(80)
Transient Energy Balance
(81)
2.6 Thermochemical Data For U and H
(85)
Heat Capacity: cv and cp
(85)
Latent Heats
(94)
Enthalpy of Reactions
(98)
2.7 Reversible Processes in Closed Systems
(110)
Reversible, Isothermal Expansion (Compression)
(110)
Adiabatic Expansion (Compression) with Constant Heat Capacity
(111)
Summary
(113)
2.8 Open-System Energy Balances on Process Equipment
(113)
Nozzles and Diffusers
(114)
Turbines and Pumps (or Compressors)
(115)
Heat Exchangers
(116)
Throttling Devices
(119)
2.9 Thermodynamic Cycles and the Carnot Cycle
(120)
Efficiency
(122)
2.10 Summary
(126)
2.11 Problems
(128)
Conceptual Problems
(128)
Numerical Problems
(131)
Chapter 3: Entropy and the Second Law Of Thermodynamics
(145)
Learning Objectives
(145)
3.1 Directionality of Processes/Spontaneity
(146)
3.2 Reversible and Irreversible Processes (Revisited) and their Relationship to Directionality
(147)
3.3 Entropy, the Thermodynamic Property
(149)
3.4 The Second Law of Thermodynamics
(158)
3.5 Other Common Statements of the Second Law of Thermodynamics
(160)
3.6 The Second Law of Thermodynamics for Closed and Open Systems
(161)
Calculation of Δs for Closed Systems
(161)
Calculation of Δs for Open Systems
(165)
3.7 Calculation of Δs for an Ideal Gas
(169)
3.8 The Mechanical Energy Balance and the Bernoulli Equation
(178)
3.9 Vapor-Compression Power and Refrigeration Cycles
(182)
The Rankine Cycle
(182)
The Vapor-Compression Refrigeration Cycle
(187)
3.10 Exergy (Availability) Analysis
(190)
Exergy
(191)
Exthalpy—Flow Exergy in Open Systems
(196)
3.11 Molecular View of Entropy
(200)
Maximizing Molecular Configurations over Space
(203)
Maximizing Molecular Configurations over Energy
(204)
3.12 Summary
(208)
3.13 Problems
(209)
Conceptual Problems
(209)
Numerical Problems
(213)
Chapter 4: Equations of State and Intermolecular Forces
(227)
Learning Objectives
(227)
4.1 Introduction
(228)
Motivation
(228)
The Ideal Gas
(229)
4.2 Intermolecular Forces
(229)
Internal (Molecular) Energy
(229)
The Electric Nature of Atoms and Molecules
(230)
Attractive Forces
(231)
Intermolecular Potential Functions and Repulsive Forces
(241)
Principle of Corresponding States
(244)
Chemical Forces
(246)
4.3 Equations of State
(250)
The van der Waals Equation of State
(250)
Cubic Equations of State (General)
(256)
The Virial Equation of State
(258)
Equations of State for Liquids and Solids
(263)
4.4 Generalized Compressibility Charts
(264)
4.5 Determination of Parameters for Mixtures
(267)
Cubic Equations of State
(268)
Virial Equation of State
(269)
Corresponding States
(270)
4.6 Summary
(272)
4.7 Problems
(273)
Conceptual Problems
(273)
Numerical Problems
(275)
Chapter 5: The Thermodynamic Web
(283)
Learning Objectives
(283)
5.1 Types of Thermodynamic Properties
(283)
Measured Properties
(283)
Fundamental Properties
(284)
Derived Thermodynamic Properties
(284)
5.2 Thermodynamic Property Relationships
(285)
Dependent and Independent Properties
(285)
Hypothetical Paths (revisited)
(286)
Fundamental Property Relations
(287)
Maxwell Relations
(289)
Other Useful Mathematical Relations
(290)
Using the Thermodynamic Web to Access Reported Data
(291)
5.3 Calculation of Fundamental and Derived Properties Using Equations of State and Other Measured Quantities
(294)
Relation of ds in Terms of Independent Properties T and v and Independent Properties T and P
(294)
Relation of du in Terms of Independent Properties T and v
(295)
Relation of dh in Terms of Independent Properties T and P
(299)
Alternative Formulation of the Web using T and P as Independent Properties
(305)
5.4 Departure Functions
(308)
Enthalpy Departure Function
(308)
Entropy Departure Function
(311)
5.5 Joule-Thomson Expansion and Liquefaction
(316)
Joule-Thomson Expansion
(316)
Liquefaction
(319)
5.6 Summary
(322)
5.7 Problems
(323)
Conceptual Problems
(323)
Numerical Problems
(325)
Chapter 6: Phase Equilibria I: Problem Formulation
(333)
Learning Objectives
(333)
6.1 Introduction
(333)
The Phase Equilibria Problem
(334)
6.2 Pure Species Phase Equilibrium
(336)
Gibbs Energy as a Criterion for Chemical Equilibrium
(336)
Roles of Energy and Entropy in Phase Equilibria
(339)
The Relationship Between Saturation Pressure and Temperature: The Clapeyron Equation
(345)
Pure Component Vapor–Liquid Equilibrium: The Clausius–Clapeyron Equation
(346)
6.3 Thermodynamics of Mixtures
(352)
Introduction
(352)
Partial Molar Properties
(353)
The Gibbs–Duhem Equation
(358)
Summary of the Different Types of Thermodynamic Properties
(360)
Property Changes of Mixing
(361)
Determination of Partial Molar Properties
(375)
Relations Among Partial Molar Quantities
(384)
6.4 Multicomponent Phase Equilibria
(385)
The Chemical Potential—The Criteria for Chemical Equilibrium
(385)
Temperature and Pressure Dependence of μi
(388)
6.5 Summary
(390)
6.6 Problems
(391)
Conceptual Problems
(391)
Numerical Problems
(395)
Chapter 7: Phase Equilibria II: Fugacity
(409)
Learning Objectives
(409)
7.1 Introduction
(409)
7.2 The Fugacity
(410)
Definition of Fugacity
(410)
Criteria for Chemical Equilibria in Terms of Fugacity
(413)
7.3 Fugacity in the Vapor Phase
(414)
Fugacity and Fugacity Coefficient of Pure Gases
(414)
Fugacity and Fugacity Coefficient of Species i in a Gas Mixture
(421)
The Lewis Fugacity Rule
(429)
Property Changes of Mixing for Ideal Gases
(430)
7.4 Fugacity in the Liquid Phase
(432)
Reference States for the Liquid Phase
(432)
Thermodynamic Relations Between Υi
(440)
Models for Υi Using ɡΕ
(446)
Equation of State Approach to the Liquid Phase
(467)
7.5 Fugacity in the Solid Phase
(467)
Pure Solids
(467)
Solid Solutions
(467)
Interstitials and Vacancies in Crystals
(468)
7.6 Summary
(468)
7.7 Problems
(470)
Conceptual Problems
(470)
Numerical Problems
(472)
Chapter 8: Phase Equilibria III: Applications
(484)
Learning Objectives
(484)
8.1 Vapor–Liquid Equilibrium (VLE)
(485)
Raoult’s Law (Ideal Gas and Ideal Solution)
(485)
Nonideal Liquids
(493)
Azeotropes
(502)
Fitting Activity Coefficient Models with VLE Data
(508)
Solubility of Gases in Liquids
(513)
Vapor–Liquid Equilibrium Using the Equations of State Method
(519)
8.2 Liquid (a)-Liquid (β) Equilibrium: LLE
(529)
8.3 Vapor–Liquid (a)-Liquid (β) Equilibrium: VLLE
(537)
8.4 Solid–Liquid and Solid–Solid Equilibrium: SLE and SSE
(541)
Pure Solids
(541)
Solid Solutions
(547)
8.5 Colligative Properties
(549)
Boiling Point Elevation and Freezing Point Depression
(549)
Osmotic Pressure
(553)
8.6 Summary
(556)
8.7 Problems
(558)
Conceptual Problems
(558)
Numerical Problems
(562)
Chapter 9: Chemical Reaction Equilibria
(580)
Learning Objectives
(580)
9.1 Thermodynamics and Kinetics
(581)
9.2 Chemical Reaction and Gibbs Energy
(583)
9.3 Equilibrium for a Single Reaction
(586)
9.4 Calculation of K from Thermochemical Data
(590)
Calculation of K from Gibbs Energy of Formation
(590)
The Temperature Dependence of K
(592)
9.5 Relationship Between the Equilibrium Constant and the Concentrations of Reacting Species
(597)
The Equilibrium Constant for a Gas-Phase Reaction
(597)
The Equilibrium Constant for a Liquid-Phase (or Solid-Phase) Reaction
(604)
The Equilibrium Constant for a Heterogeneous Reaction
(605)
9.6 Equilibrium in Electrochemical Systems
(607)
Electrochemical Cells
(608)
Shorthand Notation
(609)
Electrochemical Reaction Equilibrium
(610)
Thermochemical Data: Half-Cell Potentials
(612)
Activity Coefficients in Electrochemical Systems
(615)
9.7 Multiple Reactions
(617)
Extent of Reaction and Equilibrium Constant for R Reactions
(617)
Gibbs Phase Rule for Chemically Reacting Systems and Independent Reactions
(619)
Solution of Multiple Reaction Equilibria by Minimization of Gibbs Energy
(628)
9.8 Reaction Equilibria of Point Defects in Crystalline Solids
(630)
Atomic Defects
(631)
Electronic Defects
(634)
Effect of Gas Partial Pressure on Defect Concentrations
(637)
9.9 Summary
(642)
9.10 Problems
(644)
Conceptual Problems
(644)
Numerical Problems
(646)
Appendix A Physical Property Data
(657)
A.1 Critical Constants, Acentric Factors, and Antoine Coefficients
(657)
A.2 Heat Capacity Data
(659)
A.3 Enthalpy and Gibbs Energy of Formation at 298 K and 1 Bar
(661)
Appendix B Steam Tables
(665)
B.1 Saturated Water: Temperature Table
(666)
B.2 Saturated Water: Pressure Table
(668)
B.3 Saturated Water: Solid-Vapor
(670)
B.4 Superheated Water Vapor
(671)
B.5 Subcooled Liquid Water
(677)
Appendix C Lee–Kesler Generalized Correlation Tables
(678)
Appendix D Unit Systems
(694)
D.1 Common Variables Used in Thermodynamics and Their Associated Units
(694)
D.2 Conversion between CGS (Gaussian) units and SI units
(697)
Appendix E ThermoSolver Software
(698)
E.1 Software Description
(698)
E.2 Corresponding States Using The Lee–Kesler Equation of State
(701)
Appendix F References
(703)
F.1 Sources of Thermodynamic Data
(703)
F.2 Textbooks and Monographs
(704)
Index
(705)
