1. Course name: Thermodynamic
2. Course Code: 104282
3. Semester credit: 3(3,0,6)
4. Degree: First year student
5. Course hours
   • Class 45 hours
   • Laboratory 0 hour
   • Home study 90 hours

6. Prerequisite: General chemistry 2104039 (a)
7. Course Objectives

 For students to: learn about thermodynamic systems and boundaries; study basic law of thermodynamics (conservation of mass, conservation of energy or first law, second law); understand various forms of energy including heat transfer and work; identify various type of properties (e.g.,extensive and intensive properties); use tables, equations and charts, in evaluation of thermodynamic properties; apply conservation of mass, first law and second law in thermodynamic analysis of systems (e.g., turbines, pumps compressors, heat exchangers, etc.); enhance their problem solving skills.

8. Course Description

 Fundamental concept; First and second laws; Analysis of open and closed systems; Properties and states of substances; Work and energy; Processes and power cycles; General equations.

9. Student duty

Class attandance, assay, examine acording to the regulation No. 43/2007-QĐ-BGD&ĐT date 15/08/2007 of MOET, regulation No 235/QĐ-ĐHCN-ĐT date 30/08/2007 of IUH.

10. Course material:

Textbook:

– Peter Atkins, Physical chemistry 8^th Edition, Oxford university 2006.

Reference:

2009. Borgnakke and R.E. Sonntag, Fundamentals of thermodynamics 7^th Edition, John wile and Sons, Inc., 2009.
2010. Grades:

• Class Participation
• Assay
• Short quizzes
• Mid term
• Final term
• Other

12. Grade Rule: Follow the credit regulation
13. Course Outline:

Chapter 1: The First Law of Thermodynamics

• Basic concepts
• The first law

1.2.1. Content of the first law

1.2.2. Calculation of amounts of heat and energy changes

• Hess’s law

1.3.1. Content of hess’s law

1.3.2. The Consequence of hess’s law

• Heat capacity

1.4.1. Definition

1.4.2. The effect of temperature on heat capacity

• Kirchhoff’s law

Chapter 2: The Second Law of Thermodynamics

2.1. Preface

2.2. The reversible and irreversible processes

2.3. The second law

2.3.1. Contents of the second law

2.3.2. The mathematical expression. Entropy

2.4. Trends and limits in isolated systems – Calculation entrpy

2.4.1. Trends and limits in isolated systems

2.4.2. Calculating entropy for a reversible process

Chapter 3: Chemical Equilibrium

3.1. Some basic concepts

3.2. Chemical equilibrium of homogeneous reactions

3.2.1. Relations between the constant pressure potential and equilibrium constants of reactions – Van’t Hoff equation isothermal

3.2.2. The type of equilibrium constants

3.3. Chemical equilibrium in heterogeneous reactions

3.3.1. The equilibrium constant

3.3.2. Pressure dissociation

3.4. Factors affecting on chemical equilibrium

3.4.1. How equilibria respond to pressure

3.4.2. The response of equilibria to temperature

3.4.3. Effect of mixture components first

3.4.4. Effect of inert gas

3.5. some of methods to specify equilirium constant

Chapter 4: Phase Equilibrium

4.1. Definitions

4.2. The equilibrium condition

4.2.1. Stability of the phase

4.2.2. The equilibrium condition

4.2.3. The Gibbs phase rule

4.3. The phase diagram

4.3.1. Method performing

4.3.2. The phase diagram rules

Chapter 5: Phase Equilibria in One – Component Systems

5.1. The basic characteristics

5.2. The Clapeyron – Clausius equation

5.2.1. Effect of pressure on the phase transition temperature

5.2.2. Effect of temperature on the vapor pressure

5.3. Effect of pressure on the vapor pressure

5.4. Effect of temperature on the heat of phase transition

5.5. Phase diagram of a one-component systems

Chapter 6:  Equilibria between  Liquid – Gas Phases

6.1. General characteristics of the solution

6.1.1. Definition

6.1.2. Representation component solution

6.1.3. Classification solution

6.2. Phase equilibrium of gases dissolved in liquids

6.2.1. Effect of pressure

6.2.2. Effect of temperature

6.3. Gas – liquid equilibria

6.3.1. The ideal dilute solution

6.3.2. The real dilute solution

6.3.3. The distilled liquid

6.3.4. System of two insoluble liquids

6.3.5. The system of two liquids mixed with a limited

6.3.6. The system of three liquids mixed with a limited

6.3.7.The process of extraction, extraction and distribution law

Chapter 7: Equilibria between  Liquid – Solid Phases

7.1. Properties of the dilute solutions of non-volatile solutes

7.2. Factors affecting the solubility of solids

7.3. The crystallization of two-component solution

7.4. Two-component system does not generate crystalline solid solution and chemical compounds