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Chemical Thermodynamics and Statistical Aspects : Questions to Ask in Fundamentals and Principles.

Bibliographic Details
Main Author: Stephanos, Joseph J.
Corporate Author: ScienceDirect (Online service)
Other Authors: Addison, Anthony W.
Format: eBook
Language:English
Published: San Diego : Elsevier, 2023.
Subjects:
Thermodynamics.
Chemical equilibrium.
Chemical reactions.
Statistical thermodynamics.
Thermodynamique.
Équilibre chimique.
Thermodynamique statistique.
thermodynamics.
Chemical equilibrium
Chemical reactions
Statistical thermodynamics
Thermodynamics
Electronic books.
Online Access:Connect to the full text of this electronic book
Table of Contents:
  • Front Cover
  • Chemical Thermodynamics and Statistical Aspects
  • Chemical Thermodynamics and Statistical Aspects
  • Copyright
  • Contents
  • Preface
  • I
  • Chemical thermodynamics
  • 1
  • Thermodynamics: principles and fundamentals
  • Introduction
  • 1.1 Principles and definitions
  • 1.1.1 Thermodynamic systems and processes
  • 1.1.2 Thermodynamic variables
  • 1.1.3 Essential thermodynamic functions
  • 1.2 Energy
  • 1.2.1 Principles: definition, types, examples, and mathematic statement
  • 1.2.2 Energy and chemical reactions: spontaneity, equilibrium, and estimation
  • 1.3 Ideal gas
  • 1.3.1 Definition
  • 1.3.2 Properties
  • 1.3.3 Avogadro's law
  • 1.3.4 Boyle's law
  • 1.3.5 Charles' law
  • 1.3.6 Ideal gas law
  • 1.4 State function
  • 1.4.1 Principles: definition, examples, and significant
  • 1.4.2 Mathematics: exact/inexact differentials and Euler's criterion for exactness
  • 1.5 The kinetic theory for gases: assumption, definition, derivation, and temperature change
  • 1.6 Real gas: properties and equations
  • 1.6.1 Compression factor and virial coefficient
  • 1.6.2 van der Waals equation
  • 1.6.3 Principle of corresponding states
  • 1.6.4 Reduced variables
  • 1.7 Total and partial derivative expressions of temperature, pressure, and volume: expression for the finite change of thermody ...
  • 1.7.1 Partial derivative expressions of temperature, pressure, and volume: expressions for the finite change of thermodynamic mai ...
  • 1.8 Thermal equilibrium and zero law of thermodynamics
  • 1.9 Summary of the chapter equations
  • 2
  • Work, heat, internal energy, and enthalpy
  • Introduction
  • 2.1 The first law of thermodynamics: principles
  • 2.1.1 Energy change: definition
  • 2.1.2 Mathematic statement
  • 2.2 First case: isothermal expansion of perfect gas
  • 2.2.1 Into vacuum
  • 2.2.2 Against constant pressure (irreversible).
  • 2.12 Summary of the chapter equations
  • 3
  • Entropy: the second and third laws of thermodynamics
  • Introduction
  • 3.1 The second law of thermodynamics
  • 3.1.1 Definition
  • 3.1.2 Stability
  • 3.1.3 Thermodynamic stability
  • 3.1.4 Kinetic stability
  • 3.2 Entropy
  • 3.2.1 Definition
  • 3.2.2 Entropy and thermodynamic parameters
  • 3.2.3 Principle of Clausius
  • 3.3 Carnot cycle
  • 3.3.1 Reversible cycle
  • 3.3.2 The network: estimation
  • 3.3.3 Efficiency: definition and estimation
  • 3.3.4 Kelvin scale and absolute zero
  • 3.3.5 Reversible versus irreversible cycle
  • 3.4 Entropy basics
  • 3.4.1 Entropy equation
  • 3.4.2 Entropy and spontaneity
  • 3.4.3 Statement of the second law
  • 3.5 Calculating the entropy change
  • 3.5.1 First case: a change of state at constant temperature
  • 3.5.2 Second case: a perfect gas changing volume at constant temperature
  • 3.5.3 Third case: a substance being heated or cooled over temperature range
  • 3.5.4 Fourth case: an ideal gas undergoing an adiabatic irreversible expansion
  • 3.5.5 Entropy change for a chemical reaction
  • 3.5.6 Entropy and probability
  • 3.5.7 The third law of thermodynamics and absolute entropy
  • 3.5.8 Absolute entropy equation
  • 3.5.9 Entropy of mixing
  • 3.6 Entropy and internal energy relationships
  • 3.6.1 Entropy versus internal energy and volume as independent variables, fundamental equation
  • 3.6.2 Entropy and internal energy at constant volume
  • 3.6.3 Entropy and volume at constant internal energy
  • 3.6.4 Internal energy and volume at constant entropy
  • 3.7 Entropy and enthalpy relationships
  • 3.7.1 Entropy versus enthalpy and pressure as independent variables, fundamental equation
  • 3.7.2 Entropy and enthalpy at constant pressure
  • 3.7.3 Enthalpy and pressure at constant entropy
  • 3.8 Entropy, temperature, pressure, and volume.
  • 3.8.1 Entropy versus temperature and volume as independent variables, fundamental equation
  • 3.8.2 Entropy and temperature at constant volume
  • 3.8.3 Entropy and volume at constant temperature
  • 3.8.4 Entropy versus temperature and volume as independent variables
  • 3.8.5 Entropy versus temperature and pressure as independent variables
  • 3.8.6 Relations involving entropy
  • 3.8.7 Total and partial derivative expressions
  • 3.8.8 Entropy and temperature at constant pressure
  • 3.8.9 Entropy and volume at constant pressure
  • 3.8.10 Entropy and temperature at constant volume
  • 3.8.11 Entropy versus temperature and volume as independent variables: fundamental equation
  • 3.8.12 Maxwell relations
  • 3.9 Summary of the chapter equations
  • 4
  • Free energy of pure substance in single phase
  • Introduction
  • 4.1 Free energy: principles
  • 4.1.1 Definition
  • 4.1.2 Defining equations
  • 4.2 Gibbs energy and total entropy: equations and conditions
  • 4.3 Gibbs energy and reversibility
  • 4.4 The basic equations for free energy
  • 4.4.1 Gibbs energy taking pressure and temperature as independent variables
  • 4.4.2 Helmholtz energy taking volume and temperature as independent variables
  • 4.5 Equilibrium conditions
  • 4.5.1 Constant entropy and volume
  • 4.5.2 Constant entropy and pressure
  • 4.5.3 Constant pressure and temperature
  • 4.6 Free energy and maximum expansion work
  • 4.7 Isothermal free energy change
  • 4.7.1 Ideal gases, liquid, and solid
  • 4.7.2 Chemical reactions
  • 4.7.3 Chemical activity: fundamental equation
  • 4.8 Relations involving free energy: total and partial derivative expressions
  • 4.8.1 Gibbs change taking pressure and temperature as independent variables
  • 4.8.2 Helmholtz change taking volume and temperature as independent variables
  • 4.8.3 Maxwell relations
  • 4.8.4 Internal pressure
  • 4.8.5 Internal energy.
  • 4.8.6 Enthalpy
  • 4.8.7 Entropy
  • 4.9 Free energy, temperature, pressure, and volume
  • 4.9.1 Free energy and pressure at constant temperature
  • 4.9.2 Free energy and volume at constant temperature
  • 4.9.3 Free energy taking pressure and volume as independent variable
  • 4.9.4 Free energy and temperature at constant pressure
  • 4.9.5 Free energy and volume at constant pressure
  • 4.9.6 Free energy taking volume and temperature as independent variable
  • 4.9.7 Free energy and pressure at constant volume
  • 4.9.8 Free energy and temperature at constant volume
  • 4.9.9 Gibbs energy change taking pressure and temperature as independent variable
  • 4.9.10 Isothermal Gibbs energy change with pressure
  • 4.9.11 Isothermal Gibbs energy change with volume changes
  • 4.9.12 Helmholtz energy with temperature at constant volume
  • 4.9.13 Helmholtz energy versus the change of volume at constant temperature
  • 4.9.14 Enthalpy-entropy parallel behavior at constant temperature and pressure
  • 4.10 Chemical potential
  • 4.10.1 Definition
  • 4.10.2 Chemical potential change at constant temperature
  • 4.10.3 Chemical potential change at constant pressure
  • 4.10.4 Chemical potential and fugacity
  • 4.10.5 Real and standard state
  • 4.10.6 Thermodynamic quantities and fugacity coefficient
  • 4.10.7 Thermodynamic quantities and virial coefficient
  • 4.11 Summary of the chapter equations
  • 5
  • Thermodynamics of homogeneous and heterogeneous systems
  • Introduction
  • 5.1 Variables for open homogeneous system: principles
  • 5.2 Chemical potential and thermodynamics functions: basic equation
  • 5.3 Meaning of the chemical potential
  • 5.4 Partial molar quantities: definition
  • 5.5 Equilibrium conditions in open systems: applications
  • 5.6 Chemical potential and mole fraction: fundamental equation.