THERMODYNAMICS

Paper Code: 
CHY 213
Credits: 
3
Contact Hours: 
45.00
Max. Marks: 
100.00
Objective: 

Course Objective(s):

This course will enable the students to –

  • learn various laws of thermodynamics and their applications.
  • make students aware about thermodynamic conditions for equilibrium and open system.

Course Outcomes (COs):

Course Outcomes

 

Teaching Learning Strategies

Assessment

Strategies

On completion of this course, the students will be able to;

CO45:  describe the concept of thermal equilibrium and laws of thermodynamics.

CO46: apply the first law of thermodynamics for closed systems to calculate thermodynamic properties.

CO47:  describe Hess's law of constant heat summation and  Kirchoff's relations to calculate enthalpy change.

CO48: calculate entropy for various processes and transformation.

CO49: explain the concept of partial molar properties for open system.

CO50: apply various laws of thermodynamics to explain the behavior of chemical equilibrium.
  • Interactive lectures
  • Discussions
  • Tutorials
  • Problem solving exercise
  • Presentations by individual student/ group of students
  • Class tests at periodic intervals.
  • Written assignment(s)

 

 

9.00
Unit I: 
First Law of Thermodynamics

Importance and scope, system and surroundings, type of systems (isolated, closed and open), extensive and intensive properties, steady state and equilibrium state, concept of thermodynamic equilibrium, zeroth-law of thermodynamics, state of a system, state functions and path functions, partial derivatives and cyclic rule.
Concept of heat(q), work(W), internal energy(U), enthalpy(H) and first law of thermodynamics, calculation of q, W, U and H for reversible and irreversible processes and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions, graphical explanation of work done during expansion and compression of an ideal gas.
Heat changes at constant volume and constant pressure, relation between CP and CV using ideal gas and van der Waals’ equations, Joule's experiment and its consequence, explanation of term (δU/δV)T, Joule-Thomson experiment and its consequences, Joule-Thomson coefficient for a van der Waals’ gas, inversion temperature.

 

9.00
Unit II: 
Thermochemistry

Heat changes during physicochemical processes at constant pressure/volume. Heat of reaction- enthalpy of formation, enthalpy of combustion, enthalpy of neutralization, enthalpy of ionization, enthalpy of solution, enthalpy of phase transition, Hess's law of constant heat summation and applications, bond enthalpy, Kirchoff's relations.

 

9.00
Unit III: 
Second & Third Law of Thermodynamics

Second law of thermodynamics- need for the second law, concept of heat reservoirs and heat engines, Kelvin, Planck and Clausius statements, Carnot cycle, Carnot theorem.
Physical concept of entropy, variation of entropy with temperature, pressure and volume, entropy change for various processes, entropy change during the isothermal mixing of ideal gases.
Third law of thermodynamics, Nernst Heat Theorem, concept of residual entropy, auxiliary state functions (G and A) and their variation with T, P and V, criteria for spontaneity and equilibrium.
Thermodynamic relations- Maxwell's relations, thermodynamic equation of state, Gibbs-Helmholtz equation.

 

9.00
Unit IV: 
Thermodynamic Functions

Open system, chemical potential, partial molar quantities, variation of chemical potential with temperature and pressure, Gibbs-Duhem equation, chemical potential for the mixing of ideal gases, determination of partial molar quantities, fugacity and fugacity coefficient.

 

9.00
Unit V: 
Chemical Equilibrium

Chemical Equilibrium: Criteria of thermodynamic equilibrium, degree of advancement of reaction, Equilibrium constant and relationship between KP, KC and Kx , standard Gibbs free energy change in a chemical reaction: Van't Hoff's reaction isotherm, van't Hoff's reaction isobar and isochore, chemical equilibria in ideal gases, thermodynamic derivation of relation between Gibbs free energy of a reaction and reaction quotient, equilibrium constants and their dependence on temperature, pressure and concentration, Le Chatelier’s principle (quantitative treatment), free energy of mixing and spontaneity, equilibrium between ideal gases and a pure condensed phase.

 

Essential Readings: 
  • A Textbook of Physical Chemistry, Third edition; A.S. Negi, S.C. Anand; New Age International (P) Ltd. Publishers, New Delhi, 2022.
  • Principles of Physical Chemistry, Forty Eighth Edition; B. R. Puri, L. R. Sharma, M. S. Pathania; Vishal Publishing Co., Jalandhar, 2020.

 

References: 

SUGGESTED READINGS:

  • Atkin’s Physical Chemistry, Tenth Edition; P.W. Atkins, J. Paula; Oxford University Press, South Asia Edition, 2017.
  • Physical Chemistry Through Problems, Second Edition; S.K. Dogra and S. Dogra; New Age International Pvt. Ltd, New Delhi, 2015.
  • Thermodynamics for Chemist; Samuel Glasstone; East West Press, Private Limited, 2015.
  • A Textbook of Physical Chemistry, Thermodynamics and Chemical Equilibrium, Volume II, Sixth Edition; K. L. Kapoor; McGraw Hill Education Private Limited, 2019.
  • A Textbook of Physical Chemistry, Applications of Thermodynamics, Volume III, Fifth Edition; K. L. Kapoor; McGraw Hill Education (India) Private Limited, 2019.

e-RESOURCES :

 

 

Academic Year: 
2022-2023
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