Engineering and Chemical Thermodynamics 2nd edition by Milo D. Koretsky – Ebook PDF Instant Download/Delivery: 978-0470259610
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ISBN-13: 978-0470259610
Author: Milo D. Koretsky
Koretsky’s qualitative discussion of the role of molecular interactions and the visual approaches he uses helps students understand and visualize thermodynamics. Engineering and Chemical Thermodynamics, 2e is designed for Thermodynamics I and Thermodynamics II courses taught out of the Chemical Engineering department to chemical engineering majors. Specifically designed to accommodate students with different learning styles, this text helps establish a solid foundation in engineering and chemical thermodynamics. Clear conceptual development, worked-out examples and numerous end-of-chapter problems promote deep learning of thermodynamics and teach students how to apply thermodynamics to real-world engineering problems.By showing how principles of thermodynamics relate to molecular concepts learned in prior courses, Engineering and Chemical Thermodynamics, 2e helps students construct new knowledge on a solid conceptual foundation.
Engineering and Chemical Thermodynamics 2nd Table of contents:
Chapter 1 Measured Thermodynamic Properties and Other Basic Concepts
Learning Objectives
1.1 Thermodynamics
1.2 Preliminary Concepts—The Language of Thermo
Thermodynamic Systems
Properties
Processes
Hypothetical Paths
Phases of Matter
Length Scales
Units
1.3 Measured Thermodynamic Properties
Volume (Extensive or Intensive)
Temperature (Intensive)
Pressure (Intensive)
The Ideal Gas
1.4 Equilibrium
Types of Equilibrium
Molecular View of Equilibrium
1.5 Independent and Dependent Thermodynamic Properties
The State Postulate
Gibbs Phase Rule
1.6 The PvT Surface and Its Projections for Pure Substances
Changes of State During a Process
Saturation Pressure vs. Vapor Pressure
The Critical Point
1.7 Thermodynamic Property Tables
1.8 Summary
1.9 Problems
Conceptual Problems
Numerical Problems
Chapter 2 The First Law of Thermodynamics
Learning Objectives
2.1 The First Law of Thermodynamics
Forms of Energy
Ways We Observe Changes in U
Internal Energy of an Ideal Gas
Work and Heat: Transfer of Energy Between the System and the Surroundings
2.2 Construction of Hypothetical Paths
2.3 Reversible and Irreversible Processes
Reversible Processes
Irreversible Processes
Efficiency
2.4 The First Law of Thermodynamics for Closed Systems
Integral Balances
Differential Balances
2.5 The First Law of Thermodynamics for Open Systems
Material Balance
Flow Work
Enthalpy
Steady-State Energy Balances
Transient Energy Balance
2.6 Thermochemical Data For U and H
Heat Capacity: cv and cP
Latent Heats
Enthalpy of Reactions
2.7 Reversible Processes in Closed Systems
Reversible, Isothermal Expansion (Compression)
Adiabatic Expansion (Compression) with Constant Heat Capacity
Summary
2.8 Open-System Energy Balances on Process Equipment
Nozzles and Diffusers
Turbines and Pumps (or Compressors)
Heat Exchangers
Throttling Devices
2.9 Thermodynamic Cycles and the Carnot Cycle
Efficiency
2.10 Summary
2.11 Problems
Conceptual Problems
Numerical Problems
Chapter 3 Entropy and the Second Law Of Thermodynamics
Learning Objectives
3.1 Directionality of Processes/Spontaneity
3.2 Reversible and Irreversible Processes (Revisited) and their Relationship to Directionality
3.3 Entropy, the Thermodynamic Property
3.4 The Second Law of Thermodynamics
3.5 Other Common Statements of the Second Law of Thermodynamics
3.6 The Second Law of Thermodynamics for Closed and Open Systems
Calculation of s for Closed Systems
Calculation of s for Open Systems
3.7 Calculation of s for an Ideal Gas
3.8 The Mechanical Energy Balance and the Bernoulli Equation
3.9 Vapor-Compression Power and Refrigeration Cycles
The Rankine Cycle
The Vapor-Compression Refrigeration Cycle
3.10 Exergy (Availability) Analysis
Exergy
Exthalpy—Flow Exergy in Open Systems
3.11 Molecular View of Entropy
Maximizing Molecular Configurations over Space
Maximizing Molecular Configurations over Energy
3.12 Summary
3.13 Problems
Conceptual Problems
Numerical Problems
Chapter 4 Equations of State and Intermolecular Forces
Learning Objectives
4.1 Introduction
Motivation
The Ideal Gas
4.2 Intermolecular Forces
Internal (Molecular) Energy
The Electric Nature of Atoms and Molecules
Attractive Forces
Intermolecular Potential Functions and Repulsive Forces
Principle of Corresponding States
Chemical Forces
4.3 Equations of State
The van der Waals Equation of State
Cubic Equations of State (General)
The Virial Equation of State
Equations of State for Liquids and Solids
4.4 Generalized Compressibility Charts
4.5 Determination of Parameters for Mixtures
Cubic Equations of State
Virial Equation of State
Corresponding States
4.6 Summary
4.7 Problems
Conceptual Problems
Numerical Problems
Chapter 5 The Thermodynamic Web
Learning Objectives
5.1 Types of Thermodynamic Properties
Measured Properties
Fundamental Properties
Derived Thermodynamic Properties
5.2 Thermodynamic Property Relationships
Dependent and Independent Properties
Hypothetical Paths (revisited)
Fundamental Property Relations
Maxwell Relations
Other Useful Mathematical Relations
Using the Thermodynamic Web to Access Reported Data
5.3 Calculation of Fundamental and Derived Properties Using Equations of State and Other Measured Qu
Relation of ds in Terms of Independent Properties T and v and Independent Properties T and P
Relation of du in Terms of Independent Properties T and v
Relation of dh in Terms of Independent Properties T and P
Alternative Formulation of the Web using T and P as Independent Properties
5.4 Departure Functions
Enthalpy Departure Function
Entropy Departure Function
5.5 Joule-Thomson Expansion and Liquefaction
Joule-Thomson Expansion
Liquefaction
5.6 Summary
5.7 Problems
Conceptual Problems
Numerical Problems
Chapter 6 Phase Equilibria I: Problem Formulation
Learning Objectives
6.1 Introduction
The Phase Equilibria Problem
6.2 Pure Species Phase Equilibrium
Gibbs Energy as a Criterion for Chemical Equilibrium
Roles of Energy and Entropy in Phase Equilibria
The Relationship Between Saturation Pressure and Temperature: The Clapeyron Equation
Pure Component Vapor–Liquid Equilibrium: The Clausius–Clapeyron Equation
6.3 Thermodynamics of Mixtures
Introduction
Partial Molar Properties
The Gibbs–Duhem Equation
Summary of the Different Types of Thermodynamic Properties
Property Changes of Mixing
Determination of Partial Molar Properties
Relations Among Partial Molar Quantities
6.4 Multicomponent Phase Equilibria
The Chemical Potential—The Criteria for Chemical Equilibrium
Temperature and Pressure Dependence of μi
6.5 Summary
6.6 Problems
Conceptual Problems
Numerical Problems
Chapter 7 Phase Equilibria II: Fugacity
Learning Objectives
7.1 Introduction
7.2 The Fugacity
Definition of Fugacity
Criteria for Chemical Equilibria in Terms of Fugacity
7.3 Fugacity in the Vapor Phase
Fugacity and Fugacity Coefficient of Pure Gases
Fugacity and Fugacity Coefficient of Species i in a Gas Mixture
The Lewis Fugacity Rule
Property Changes of Mixing for Ideal Gases
7.4 Fugacity in the Liquid Phase
Reference States for the Liquid Phase
Thermodynamic Relations Between γi
Models for γi Using gE
Equation of State Approach to the Liquid Phase
7.5 Fugacity in the Solid Phase
Pure Solids
Solid Solutions
Interstitials and Vacancies in Crystals
7.6 Summary
7.7 Problems
Conceptual Problems
Numerical Problems
Chapter 8 Phase Equilibria III: Applications
Learning Objectives
8.1 Vapor–Liquid Equilibrium (VLE)
Raoult’s Law (Ideal Gas and Ideal Solution)
Nonideal Liquids
Azeotropes
Fitting Activity Coefficient Models with VLE Data
Solubility of Gases in Liquids
Vapor–Liquid Equilibrium Using the Equations of State Method
8.2 Liquid Equilibrium: LLE
8.3 Vapor–Liquid (α) Liquid (β) Equilibrium: VLLE
8.4 Solid–Liquid and Solid–Solid Equilibrium: SLE and SSE
Pure Solids
Solid Solutions
8.5 Colligative Properties
Boiling Point Elevation and Freezing Point Depression
Osmotic Pressure
8.6 Summary
8.7 Problems
Conceptual Problems
Numerical Problems
Chapter 9 Chemical Reaction Equilibria
Learning Objectives
9.1 Thermodynamics and Kinetics
9.2 Chemical Reaction and Gibbs Energy
9.3 Equilibrium for a Single Reaction
9.4 Calculation of K from Thermochemical Data
Calculation of K from Gibbs Energy of Formation
The Temperature Dependence of K
9.5 Relationship Between the Equilibrium Constant and the Concentrations of Reacting Species
The Equilibrium Constant for a Gas-Phase Reaction
The Equilibrium Constant for a Liquid-Phase (or Solid-Phase) Reaction
The Equilibrium Constant for a Heterogeneous Reaction
9.6 Equilibrium in Electrochemical Systems
Electrochemical Cells
Shorthand Notation
Electrochemical Reaction Equilibrium
Thermochemical Data: Half-Cell Potentials
Activity Coefficients in Electrochemical Systems
9.7 Multiple Reactions
Extent of Reaction and Equilibrium Constant for R Reactions
Gibbs Phase Rule for Chemically Reacting Systems and Independent Reactions
Solution of Multiple Reaction Equilibria by Minimization of Gibbs Energy
9.8 Reaction Equilibria of Point Defects in Crystalline Solids
Atomic Defects
Electronic Defects
Effect of Gas Partial Pressure on Defect Concentrations
9.9 Summary
9.10 Problems
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