homework #1 (page 1 out of 2)
1. Calculate the molar enthalpy of pure iron at 1500 K and one atmosphere pressure. The molar heats of phase transformations for iron are: H = 670 J/mol; H = 840 J/mol; H liquid = 13770 J/mol. The constant pressure heat capac
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (1) First Law - Energy Balance Thermodynamic functions of state Internal energy, heat and work Types of paths (isobaric, isochoric, isothermal, adiabatic, cyclic) Enthalpy, heat
The Statistical Interpretation of Entropy
Physical meaning of entropy
Microstates and macrostates
Statistical interpretation of entropy and Boltzmann equation
Configurational entropy and thermal entropy
Calculation of the equilibrium vacancy concentration
Theoretical calculation of the heat capacity
Principle of equipartition of energy
Heat capacity of ideal and real gases
Heat capacity of solids: Dulong-Petit, Einstein, Debye models
Heat capacity of metals electronic contribution
Reading: Chapter 6.2 of G
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (3)
Fundamental equations
The Helmholtz Free Energy
The Gibbs Free energy
Changes in composition
Chemical potential
Thermodynamic relations
Reading: Chapter 5.1 5.9 of Gaskell
o
Phase Transitions and Phase Diagrams
One-component systems
Enthalpy and entropy dependence on P and T
Gibbs free energy dependence on P and T
Clapeyron equation
Understanding phase diagrams for one-component systems
Polymorphic phase transitions
Driving f
Theoretical calculation of the heat capacity
Principle of equipartition of energy
Heat capacity of ideal and real gases
Heat capacity of solids: Dulong-Petit, Einstein, Debye models
Heat capacity of metals electronic contribution
Reading: Chapter 6 Se
MSE 3050: Thermodynamics and Kinetics of Materials
Tuesday and Thursday, 9:30 10:45 am
Mechanical Engineering Building 339
Contact Information:
Instructor: Giovanni Zangari
Office: Wilsdorf Hall 320
Office Hours: 11:00 am to noon Monday & open
Telephone:
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (2)
Entropy and the Second Law
Concepts of equilibrium
Reversible and irreversible processes
The direction of spontaneous change
Entropy and spontaneous/irreversible processes
C
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (3)
Fundamental equations
The Helmholtz Free Energy
The Gibbs Free energy
Changes in composition
Chemical potential
Thermodynamic relations
Reading: Chapter 5.1 5.9 of Gaskell
o
Phase Transitions and Phase Diagrams
One-component systems
Enthalpy and entropy dependence on P and T
Gibbs free energy dependence on P and T
Clapeyron equation
Understanding phase diagrams for one-component systems
Polymorphic phase transitions
Driving f
The Statistical Interpretation of Entropy
Physical meaning of entropy
Microstates and macrostates
Statistical interpretation of entropy and Boltzmann equation
Configurational entropy and thermal entropy
Calculation of the equilibrium vacancy concentration
Kinetics and Diffusion
Basic concepts in kinetics
Kinetics of phase transformations
Activation free energy barrier
Arrhenius rate equation
Diffusion in Solids - Phenomenological description
Flux, steady-state diffusion, Ficks first law
Nonsteady-state dif
Binary Solutions
Composition as a thermodynamic variable
Gibbs free energy of binary solutions
Entropy of formation and Gibbs free energy of an ideal
solution
Regular solutions: Heat of formation of a solution
Real solutions: interstitial solid solut
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (1)
First Law - Energy Balance
Thermodynamic functions of state
Internal energy, heat and work
Types of paths (isobaric, isochoric, isothermal, adiabatic, cyclic)
Enthalpy, heat
Binary Solutions
Composition as a thermodynamic variable
Gibbs free energy of binary solutions
Entropy of formation and Gibbs free energy of an ideal
solution
Regular solutions: Heat of formation of a solution
Real solutions: interstitial solid solutions,
Solutions to the diffusion equation
Numerical integration
finite difference method
spatial and time discretization
initial and boundary conditions
stability
Analytical solution for special cases
plane source
thin film on a semi-infinite substrate
d
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (2)
Entropy and the Second Law
Concepts of equilibrium
Reversible and irreversible processes
The direction of spontaneous change
Entropy and spontaneous/irreversible processes
C
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (2) Entropy and the Second Law Concepts of equilibrium Reversible and irreversible processes The direction of spontaneous change Entropy and spontaneous/irreversible processes C
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (3) Fundamental equations The Helmholtz Free Energy The Gibbs Free energy Changes in composition Chemical potential Thermodynamic relations
Reading: Chapter 5.1 5.9 of Gaskell o
Binary Solutions
Composition as a thermodynamic variable Gibbs free energy of binary solutions Entropy of formation and Gibbs free energy of an ideal solution Chemical potential of an ideal solution Regular solutions: Heat of formation of a solution Activ
Theoretical calculation of the heat capacity
Principle of equipartition of energy Heat capacity of ideal and real gases Heat capacity of solids: Dulong-Petit, Einstein, Debye models Heat capacity of metals electronic contribution
Reading: Chapter 6.2 of G
homework #2 (page 1 or 2)
1. One mole of copper at a uniform temperature of 0C is placed in thermal contact with a second mole of copper which, initially, is at a uniform temperature of 100C. The pressure in the system is maintained at 1 atm. The two mole
homework #3 (page 1 of 2)
1. The molar volumes of solid and liquid lead under the atmospheric pressure are, respectively, 18.92 cm3 and 19.47 cm3, melting temperature Tm = 600 K, molar heat of melting Hm = 4810 J. Calculate the pressure which must be appl
Phase Transitions and Phase Diagrams
One-component systems Enthalpy and entropy dependence on P and T Gibbs free energy dependence on P and T Clapeyron equation Understanding phase diagrams for one-component systems Polymorphic phase transitions Driving f
The Statistical Interpretation of Entropy
Physical meaning of entropy Microstates and macrostates Statistical interpretation of entropy and Boltzmann equation Configurational entropy and thermal entropy Calculation of the equilibrium vacancy concentration
MSE 6080 THERMODYNAMICS AND KINETICS OF MATERIALS
Spring 2017
Homework 1
Assigned:
Due:
January 26, 2017
February 2, 2017, in class
1. Calculate the molar enthalpy of pure cobalt at 2,000 K and one atmosphere pressures.
The molar heats of phase transfo
Review of classical thermodynamics
Fundamental Laws, Properties and Processes (1)
First Law - Energy Balance
Thermodynamic functions of state
Internal energy, heat and work
Types of paths (isobaric, isochoric, isothermal, adiabatic, cyclic)
Enthalpy, heat
Nucleation and growth kinetics
Homogeneous nucleation
Critical radius, nucleation rate
Heterogeneous nucleation
Nucleation in melting and boiling
Growth mechanisms
Rate of a phase transformation
Reading: Chapters 4.1and 4.2 of Porter and Easterling,
MSE 3