Chemical Thermodynamics and its Application
Teacher
Dr. Suchismita Acharya
Category
Core Courses
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Code(Credit) : CUTM 1472(3-2-1)
Course Objectives
- The Course covers the fundamentals laws of Thermodynamics and its related Phenomena
- To understand the applicability of chemical thermodynamics in various industrial processes as well as day to day life incidents.
- To understand the conceptual basis of thermodynamic scale of temperature as standard scale
- To understand the concept of chemical equilibrium in attaining high products by controlling various factors.
- To understand the concept of ideal and non-ideal solution along with various colligative properties.
- To practice various thermochemical experiments
Course Outcomes
| COs | Course outcomes | Mapping COs with POs (High-3, Medium-2, Low-1) |
| CO1 | Able to gain entire Knowledge on Thermodynamics, Chemical Equilibria and Colligative properties. | PO1 (3) |
| CO2 | To know different thermodynamic equations, chemical equilibriums and their relationship among each other. | PO2 (3). PO4 (2) |
| CO3 | Able to interpret and analyse the data for publication | PO4 (3) |
Course Syllabus
Module I : Introduction to Thermodynamics
- Intensive and extensive variables; state and path functions; isolated, closed and open systems Zeroth law of thermodynamics
- First law: Concept of heat (q), work (w), internal energy (U), and statement of first law
- Enthalpy (H), relation between heat capacities,Calculations of q, w, U and H for reversible condition.
- Calculations of q, w, U and H for irreversible and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions
- Asignment 1 (Flip Class : Types of Systems and First law) (1 h)
- Asignment 2 (Flip Class : Calculation of Work done for various systems) (1 h)
Module II : Thermochemistry
- Heats of reactions: standard states; Enthalpy of formation of molecules and ions and enthalpy of combustion and its applications
- Effect of temperature (Kirchhoff’s equations) and pressure on enthalpy of reactions, Adiabatic flame temperature, explosion temperature
- Assignment 3 (Flip Class: Calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data) (2h)
- Practice 1: Determination of heat capacity of a calorimeter for different volumes using change of enthalpy data of a known system (method of back calculation of heat capacity of calorimeter from known enthalpy of solution or enthalpy of neutralization).
- Practice 2: Determination of heat capacity of the calorimeter and enthalpy of neutralization of hydrochloric acid with sodium hydroxide.
- Practice 3: Determination of heat capacity of the calorimeter and integral enthalpy (endothermic and exothermic) solution of salts.
- Practice 4: Determination of enthalpy of hydration of copper sulphate
Module III : Chemical Thermodynamics I
- Thermodynamic scale of temperature
- Statement of the second law of thermodynamics; molecular and statistical interpretation of entropy.
- Calculation of entropy change for reversible and irreversible processes
- Third Law: Statement of third law, concept of residual entropy , calculation of absolute entropy of molecules
- Free Energy Functions: Gibbs and Helmholtz energy; variation of S, G, A with T, V, P; Free energy change and spontaneity
- Relation between Joule-Thomson coefficient and other thermodynamic parameters; inversion temperature
- Thermodynamic equation of state
- Assignment 4 : (Flip Class) Gibbs-Helmholtz equation (1h)
- Assignment 5 : (Flip Class) Maxwell relations (1h)
Module IV : Chemical Thermodynamics and Open System
- Partial molar quantities, dependence of thermodynamic parameters on composition
- Gibbs Duhem equation, chemical potential of ideal mixtures, change in thermodynamic functions in mixing of ideal gases
- Assignment 6 (Flip class) (Problem Solving approach) (2h)
- Assignment 7 (Flip class) (Partial molar quantities) (1h)
Module V : Chemical Equilibrium: I
- Criteria of thermodynamic equilibrium
- Degree of advancement of reaction, chemical equilibria in ideal gases
- Thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient.
- Concept of fugacity
- Equilibrium constants and their quantitative dependence on temperature, pressure and concentration
- Coupling of exoergic and endoergic reactions
- Free energy of mixing and spontaneity
- Assignment 8 (Flip Class) (Concept of fugacity and equilibrium) (1h)
- Practice 5: To study the shift of equilibrium between ferric ions and thiocyanate ions by increasing the concentration of either of them
Module VI : Chemical Equilibrium: II
- Thermodynamic derivation of relations between the various equilibrium constants Kp, Kc and Kx. Le Chatelier principle (quantitative treatment)
- Equilibrium between ideal gases and a pure condensed phase.
- Introduction to dilute Solutions
- Introduction to Colligative Properties
- Practice 6 : Le Chatelier principle in Contact Process (Demonstration)
- Practice 7 : Le Chatelier principle in Haber Process (Demonstration)
Module VII: Colligative Properties
- Excess thermodynamic functions. Thermodynamic derivation using chemical potential to derive relations between the relative lowering of vapour pressure and amount of solute
- Thermodynamic derivation using chemical potential to derive relations between the elevation of boiling point and amount of solute
- Thermodynamic derivation using chemical potential to derive relations between Depression of freezing point and amount of solute
- Thermodynamic derivation using chemical potential to derive relations between the osmotic pressure and amount of solute.
- Assignment 9 (Flip class) ( Raoult’s and Henry’s Laws and their
applications) (1h) - Assignment 10 (Flip class) (Applications in calculating molar masses of normal, dissociated and associated solutes in solution) (1h)
- Practice 8: To find the freezing point depression of a solution
- Practice 9: To find the molar mass through freezing point depression of a solution
- Practice 10: Determining the Vant Hoff's factor
- Practice 11: To find the elevation of boiling point of a solution
- Practice 12: To find the molar mass through elevation of boiling point of a solution
Books for Reference
Text Books:
- Atkins P. and De Paula, J. Physical Chemistry Tenth Ed., OUP, 2014.
- Castellan, G. W. Physical Chemistry 4th Ed., Narosa, 2004.
Reference Books:
- Engel, T. and Reid, P. Physical Chemistry 3rd Ed., Prentice Hall, 2012
- .McQuarrie, D. A. and Simon, J. D. Molecular Thermodynamics Viva Books, 2004.
- Roy, B. N. Fundamentals of Classical and Statistical Thermodynamics Wiley, 2001
- Levine, I .N. Physical Chemistry 6th Ed. Tata Mc Graw Hill, 2010.
Session Plan
Session 1
Systems and Surroundings, intensive and extensive variables , state and path functions, isolated, closed and open systems, Zeroth law of thermodynamics
https://www.youtube.com/watch?v=oXxX1NmE7Ho
https://www.youtube.com/watch?v=dWwZIOSi_Vw
https://www.youtube.com/watch?v=FdXxJuRw7Ck
Session 2
First law: Concept of heat (q), work (w), internal energy (U), and statement of first law
Session 3
Enthalpy (H), relation between heat capacities, calculations of q, w, U and H for reversible condition.
https://www.youtube.com/watch?v=x_pbr5RFhVc
Session 4
Calculations of q, w, U and H for irreversible , and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions ,
https://www.youtube.com/watch?v=guP4wKNBtM4
https://www.youtube.com/watch?v=8zJrjEV9n8o
Session 5 (Assignment 1) (1h)
Asignment 1 (Flip Class : Types of Systems and First law)
Session 6 (Assignment 2) (1h)
Asignment 2 (Flip Class : Calculation of Work done for various systems)
Session 7
Heats of reactions: standard states; Enthalpy of formation of molecules and ions and enthalpy of combustion and its applications
https://www.youtube.com/watch?v=nASUmuqu7so
Session 8
Effect of temperature (Kirchhoff’s equations) and pressure on enthalpy of reactions, adiabatic flame temperature , explosion temperature
https://www.youtube.com/watch?v=mFRvwerRRag
Session 9 (Assignment 3) (1h)
Assignment 3 (Flip Class: Calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data
https://www.youtube.com/watch?v=QFzZdcMnlK4
Session 10 (Practice 1) (2h)
Practice 1: Determination of heat capacity of a calorimeter for different volumes using change of enthalpy data of a known system (method of back calculation of heat capacity of calorimeter from known enthalpy of solution or enthalpy of neutralization)
Session 11 (Practice 2) (2h)
Practice 2: Determination of heat capacity of the calorimeter and enthalpy of neutralization of hydrochloric acid with sodium hydroxide
Session 12 (Practice 3) (2h)
Practice 3: Determination of heat capacity of the calorimeter and integral enthalpy (endothermic and exothermic) solution of salts.
Session 13 (Practice 4) (2h)
Practice 4: Determination of enthalpy of hydration of copper sulphate
https://www.youtube.com/watch?v=lLUH13rXvVs,
Session 15
Statement of the second law of thermodynamics; molecular and statistical interpretation of entropy
Session 16
Calculation of entropy change for reversible and irreversible processes
Session 17
Third Law: Statement of third law, concept of residual entropy , calculation of absolute entropy of molecules
Session 18
Free Energy Functions: Gibbs and Helmholtz energy; variation of S, G, A with T, V, P; Free energy change and spontaneity
Session 19
Relation between Joule-Thomson coefficient and other thermodynamic parameters; inversion temperature
Session 21 (Assignment 4) (1h)
Assignment 4 : (Flip Class) Gibbs-Helmholtz equation
Session 22 (Assignment 5) (1h)
Assignment 5 : (Flip Class)
Session 23
Partial molar quantities, dependence of thermodynamic parameters on composition
Session 24
Gibbs Duhem equation, chemical potential of ideal mixtures, change in thermodynamic functions in mixing of ideal gases
Session 25 (Assignment 6) (2h)
Assignment 6 (Flip class) (Problem Solving approach)
Session 26 (Assignment 7) (1h)
Assignment 7 (Flip class) (Partial molar quantities)
Session 28
Degree of advancement of reaction, chemical equilibria in ideal gases
Session 29
Thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient
Session 31
Equilibrium constants and their quantitative dependence on temperature, pressure and concentration
Session 34 (Assignment 8) (1h)
Assignment 8 (Flip Class) (Concept of fugacity and equilibrium)
Session 35 (Practice 5) (2h)
Practice 5: To study the shift of equilibrium between ferric ions and thiocyanate ions by increasing the concentration of either of them
Session 36
Thermodynamic derivation of relations between the various equilibrium constants Kp, Kc and Kx. Le Chatelier principle (quantitative treatment)
Session 37
Equilibrium between ideal gases and a pure condensed phase.
Session 40 (Practice 6) (2h)
Practice 6: Le Chatelier principle in Contact Process (Demonstration)
Session 41 (Practice 7) (2h)
Practice 7: Le Chatelier principle in Haber Process (Demonstration)
Session 42
Thermodynamic derivation using chemical potential to derive relations between the relative lowering of vapour pressure and amount of solute
Session 43
Thermodynamic derivation using chemical potential to derive relations between the elevation of boiling point and amount of solute
Session 44
Thermodynamic derivation using chemical potential to derive relations between Depression of freezing point and amount of solute
Session 45
Thermodynamic derivation using chemical potential to derive relations between the osmotic pressure and amount of solute
Session 46 (Assignment 9) (1h)
Assignment 9 (Flip class) ( Raoult’s and Henry’s Laws and their applications)
Session 47 (Assignment 10) (1h)
Assignment 10 (Flip class) (Applications in calculating molar masses of normal, dissociated and associated solutes in solution (1h)
Session 48 (Practice 8) (2h)
Practice 8:To find the freezing point depression of a solution
Session 49 (Practice 9) (2h)
Practice 9:To find the molar mass through freezing point depression of a solution
Session 50 (Practice 10) (2h)
Practice 10: Determining the Vant Hoff's factor
Session 51 (Practice 11) (2h)
Practice 11: To find the elevation of boiling point of a solution
Session 52 (Practice 12) (2h)
Practice 12: To find the m find the molar mass through boiling point elevation of a solution
Our Main Teachers
Currently working as an Assistant Professor in the department of Chemistry, Centurion University of Technology and Management, Bhubaneswar campus.