Thermodynamics

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

Course Objectives:

This course will enable the students to –

  1. make the students learn various laws of thermodynamics and their applications.
  2. learn about thermodynamic functions and thermodynamic conditions for equilibrium.
  3. make students aware about thermodynamic conditions for equilibrium and the concept of solubility and common ion effect.

Course Outcomes (COs):

Course

Learning outcomes

(at course level)

Learning and teaching strategies

Assessment

Strategies

Paper Code

Paper Title

CHY-213

 

Thermody namics

 

 

The students will be able to –

CO41:  describe the concept of thermal equilibrium and Zeroth-law of thermodynamics.

CO42:  state and apply the first law of thermodynamics for COsed and open systems undergoing different thermodynamic processes to calculate change in internal energy.

CO43:  describe Hess's law of constant heat summation and Kirchoff's relations and can apply them.

 CO44:  describe the need of second law of thermodynamics and know various thermodynamic relations.

CO45: understand the concept of thermodynamic state functions and their variation with temperature and pressure.

 CO46: apply various laws of chemical equilibrium and know the concept of common ion effect.

 

Interactive Lectures

 

Discussions

 

Tutorials

 

Problem solving

Presentati ons by individua l student/ group of three Students

 

Class Tests at Periodic intervals.

 

Written assignment(s)

 

Semester End Examination

 

12.00
Unit I: 
First Law of Thermodynamics

Importance and scope, definitions of system and surroundings; type of systems (isolated, closed and open). Extensive and intensive properties. Steady state and equilibrium state. Concept of thermal equilibrium and the zeroth-law of thermodynamics. Thermodynamic coordinates, state of a system, equation of state, state functions and path functions. Partial derivatives and cyclic rule. Concept of heat and work (IUPAC convention). Graphical explanation of work done during expansion and compression of an ideal gas. Reversible and irreversible processes and work done. First law of thermodynamics, internal energy (U) as a state function. Enthalpy as a state function. Heat changes at constant volume and constant pressure; relation between CP and CV using ideal gas and vander Waals equations. Joule's experiment and its consequence. Explanation of term (δU/δV)T. Isothermal and adiabatic processes. Joule-Thomson experiment and its consequences; inversion temperature. Joule-Thomson coefficient for a van der Waals gas, General heat capacity relations.

6.00
Unit II: 
Thermochemistry

Thermochemistry: heat changes during physicochemical processes at constant pressure/volume. Hess's law of constant heat summation and applications, Kirchoff's relations. Bond dissociation energies. Changes of thermodynamic properties in different chemical changes.

8.00
Unit III: 
Second Law of Thermodynamics
Second law of thermodynamics – need for a Second law. Concept of heat reservoirs and heat engines. Kelvin – Planck and Clausius statements and equivalence of the two statements with entropic formulation. Carnot cycle and refrigerator. Carnot's theorem; thermodynamic scale of temperature.
Physical concept of entropy. Entropy as a measure of the microscopic but not macroscopic disorder. Entropy change of systems and surroundings for various processes and transformations. Entropy change during the isothermal mixing of ideal gases. Nernst Heat Theorem, Third law of thermodynamics (elementary idea) Entropy and unavailable work. 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.
 
7.00
Unit IV: 
Thermodynamic Functions

Open system, chemical potential and activity, partial molar quantities, chemical potential in terms of Gibb's free energy and other thermodynamic state functions and its variation with temperature and pressure. Gibbs-Duhem equation; fugacity of gases and fugacity coefficient.

12.00
Unit V: 
Chemical Equilibrium

Thermodynamic conditions for equilibrium, degree of advancement. Van't Hoff's reaction isotherm (deduction from chemical potential). Explanation of the free energy versus degree of advancement plot. Equilibrium constant and standard Gibbs free energy change. Definitions of KP, KC and Kx ; van't Hoff's reaction isobar and isochore from different standard states. Shifting of equilibrium due to change in external parameters e.g. temperature and pressure. Le Chatelier's principle and degree of advancement. Activity and activity coefficients of electrolyte / ion in solution. Debye-Huckel limiting law (statement and applications only). Solubility equilibrium and common ion effect.

References: 
  • A Textbook of Physical Chemistry; A.S. Negi, S.C. Anand; New Age International (P) Limited, New Delhi, 2007.
  • Elements of Physical Chemistry; Seventh International Edition. P.W. Atkins, J. Paula; Oxford, India 2017.
  • Elements of Physical Chemistry; Seventh Edition. P.W. Atkins, J. Paula; Oxford University Press, New York, 2016.
  • Physical Chemistry; Fourth Edition; R.A. Alberty; Wiley Eastern Ltd., Singapore, 2004.
  • Physical Chemistry Through Problems; S.K. Dogra and S.Dogra; Second Edition;New Age International Pvt. Ltd, New Delhi, 2001.
  • Physical Chemistry;Sixth Edition ; G.M. Barrow; McGraw Hill, New Delhi, 1996.
Academic Year: 
2020-2021
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