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Basic of thermodynamic

by Dr. Srimala

srimala@eng.usm.myroom 2.07

Albert Einstein

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School Of Materials And Mineral Resources EngineeringEngineering Campus

Course Structure Form

Course Code : EBB 236

Course Title : Material Thermodynamic

Course Unit : 3

Type of Course : Core

OBEOBE

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Contribution of Assessment :

Final Examination 70% Coursework : 30%

Assessment Methods for Coursework:

Test 1 (Dr.Projjal Basu) =10marks Test 2 (Dr. Srimala)= 10 marks Quiz/ Tutorial (Dr. Srimala)= 5marks Quiz (Dr.Projjal Basu)= 5marks

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Course Outcomes (CO) :At the end of the course, the students should be able to:

interpret the fundamental aspects of thermodynamics which are related to general principles of matter such as structure and properties

predict behaviors of matters based on thermodynamic principles as it undergoes various changes in condition

design new process and improve the existing process using thermodynamic principles

create materials with desired properties.

derive relationship among the properties of matter based from few general and pervasive principles (the law of thermodynamics)

solve problems of practical interest using thermodynamic equation

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Teaching Plans / SyllabusEquilibrium (week 8)

• Phase Equilibrium• Liquid-Vapor Phase Equilibrium• Gibbs Phase Rule• P-T Phase Diagrams & Clausius Clapeyron Equation• The Clausius-Clapeyron Equation• Liquid-Vapour (Vaporization) Equlibrium• Triple Point• Calculation solid-liquid-gas triple point

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Teaching Plans / SyllabusThermodynamic of Phase Diagram (week 9 and 10)

• Thermodynamically stable phase• Unary Heterogeneous Systems• P - T Diagram -Unary, Single Component Phase Diagram• logP – 1/T Diagram -Unary, Single Component Phase Diagram• Conclusion-Unary P - T Diagrams• G-T Phase Diagrams• G - T Diagram - Unary, Single Component Phase Diagram – V• G-T Diagram - Unary, Single Component Phase Diagram - L,V• G-T Diagram - Unary, Single Component Phase Diagram-,L,V• G- T Diagram - Single Component Phase Diagram -,, L, V• 3.5 Metastability

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Teaching Plans / Syllabus

Thermodynamic of Phase Diagram• Chemical Potential and Gibbs Free Energy of Single Component Phases• Enthalpy & Entropy of Transformation• Compute Phase Equilibria from Free Energy Relations• Binary System• Binary liquid system• Binary solutions with total solid solubility• Binary systems without solid solution• Free Energy-Composition (G-X) Diagram• Free energy diagrams of total solubility systems• Free energy diagram for binary solutions with a miscibility gap• Free energy diagram of binary systems without solid solution

(eutectic system) • Phase boundary Calculations

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Teaching Plans / SyllabusCrystal Defects (week 11)

• Perfect Crystal• Processing, Microstructure and Properties • Crystal defect• Vacancies and Interstitials• Impurity Atoms• Point Defects in Ionic Crystals• Defect Complexes• Vacancies formation• Divacancy• Defects in the ionic compounds• Kroger-Vink notation• Frenkel Defect• Schottky defects

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Teaching Plans / SyllabusPhase Transformation (week 12)

• Homogeneous Nucleation• Gibbs Free Energy• Energies involved in homogeneous nucleation• Critical radius & Critical free energy• Nucleation rate• Heterogeneous Nucleation• Energies Involved in heterogeneous nucleation

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Teaching Plans / SyllabusEnergy of Interfaces (week 13)

• Surface tension • Surface free energy• Surface stress• Equilibrium shape of surfaces• Presence of secondary phase• Bulk• Face• Edge and Corner• Applications

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References

• Robert T. DeHoff, Thermodynamic in materials science, Mc Graw Hill,1993• Mac Geon Lee, Chemical thermodynamic for Metals and Materials, Imperial

College Press, 1999.• David V.Ragone, Thermodynamics of Materials, Volume I, John Wiley &

Sons, Inc.• David V.Ragone, Thermodynamics of Materials, Volume II, John Wiley &

Sons, Inc.• John D. Verhoeven, Fundermentals of Physical Metallurgy, , John Wiley &

Sons, Inc,1975

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Basic of thermodynamic

Content

1.0 What is Thermodynamics2.0 Thermodynamic Systems – Definitions3.0 Thermodynamic State Properties4.0 Idealized Thermodynamic Processes5.0 Spontaneous Reaction Direction

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1.0 What is Thermodynamics

Thermodynamics:

A set of of mathematical models and concepts that allow us to describe the way changes in the system state (temperature, pressure, and composition) affect equilibrium.

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Why are we interested in studying thermodynamics?

Thermodynamics allows us to predict the direction of natural change (reactions) and the final state (equilibrium composition) of a system.

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Examples

If we know the composition of a soil solution or a groundwater in contact with soil or aquifer solids, thermodynamics allows us to predict:

• If solids will dissolve• If solids will precipitate• If the system is at equilibrium

When several minerals are present and in contact with the same aqueous phase, we can predict the direction of mineral evolution.E.g., we may predict that a granites mineral composed of quartz, feldspar, and mica will eventually weather into smectite clay

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In discussing thermodynamics, we’ll refer frequently to systems

Mixture of stuff that may react (t=0)

System (contained in some fashion)

2.0 Thermodynamic Systems - Definitions

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Isolated System: No matteror energy cross systemboundaries. No work can bedone on the system.

Open System: Free exchangeacross system boundaries.

Closed System: Energy can beexchanged but matter cannot.

Adiabatic System: Special casewhere no heat can be exchangedbut work can be done on thesystem (e.g. PV work).

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What information can thermodynamics give us about a system?

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Thermodynamics deals with macroscopic phenomena – measurable at the laboratory scale. X

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Provided by Thermodynamics?Yes No

Whether change will occurDirection of changeRate of changeReaction mechanismsMicroscopic processesFinal composition of system

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3.0 Thermodynamic State Properties

• Extensive:These variables or properties depend on the amount of material present (e.g. mass or volume).

• Intensive:These variables or properties DO NOT depend on the amount of material (e.g. pressure, and temperature).

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4.0 Idealized Thermodynamic Processes

• Irreversible:Initial system state is unstable or metastable and spontaneous change in the system yields a system with a lower-energy final state.

• Reversible:Both initial and final states are stable equilibrium states and the path between them is a continuous sequence of equilibrium states. NOT ACTUALLY REALIZED IN NATURE.

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5.0 Spontaneous Reaction Direction