Applications of Thermodynamics

Paper Code: 
CHY-303
Credits: 
2
Contact Hours: 
30.00
Max. Marks: 
100.00
Objective: 

Course Objectives:

This course will enable the students to –

  1. Acquaint the students with the laws of thermodynamics in understanding homogenous and heterogenous equilibria.
  2. Provide an in-depth knowledge of the concepts of electrochemistry in redox system.

Course Outcomes (COs):

Course

Learning outcomes

(at course level)

Learning and teaching strategies

Assessment Strategies

Paper Code

Paper Title

CHY

303

Applications of Thermodynamics (Theory)

 

The students will be able to –

CO49: describe concept of Gibbs function, Helmholtz function and discuss their variation with pressure, volume and temperature.

CO50: deduce the thermodynamic relations of equilibrium constant with other thermodynamic properties.

CO51: explain heterogeneous equilibrium having one component and two component systems.

CO52: predict the notation of a single electrode, cell and measure its cell potential using the Nernst equation.

CO53: measure the thermodynamic properties of a cell using EMF.

CO54: explain the operations of a concentration cell and predict the concentration in the cell based on the cell potential.

CO55: measuring the pH of the given solution using various types of electrodes.

Interactive Lectures

Discussion

Tutorials

Multimedia Presentations

Demonstration

Learning activities for the students:

Self learning Assignments

Power Point Presentation

Handouts

The oral and written examinations (Scheduled and surprise tests)

Closed book and open book tests

Quiz

Problem solving exercises

Assignments

Presentation

Semester End Examinations
 

 

5.00
Unit I: 
Thermodynamics: Free energy functions

Gibbs and Helmholtz functions, Gibbs function (G) and Helmholtz function (A) as thermodynamic quantities, A & G as criteria for thermodynamic equilibrium and spontaneity, their advantages over entropy change, variation of G & A with pressure, volume and temperature.

6.00
Unit II: 
Thermodynamics: Chemical equilibrium

Equilibrium constant and free energy, thermodynamic derivation of law of mass action. Le Chatelier’s principle, reaction isotherm and reaction isochore, Clapeyron equation, Clausius-Clapeyron equation and its applications.

7.00
Unit III: 
Heterogeneous equilibria – Phase rule

Introduction to phase, components and degree of freedom, derivation of Gibbs phase rule; phase equilibria of one component system-water, CO2 and sulphur system.

Phase equilibria of two component system: Simple eutectic – Bi-Cd and Pb-Ag systems, desilverisation of lead.

Solid solutions: Compound formation with congruent melting point (Mg-Zn), (FeCl3 – H2O) and incongruent melting point (NaCl-H2O)and (CuSO4 – H2O) system, freezing mixtures (acetone – dry ice).

5.00
Unit IV: 
Electrochemistry I: Equilibrium in Redox System

Types of reversible electrodes: Gas-metal ion, metal-metal ion, metal-insoluble salt-anion and redox electrodes, electrode reactions, Nernst equation, EMF of a cell and its measurement, computation of cell EMF, calculation of thermodynamic quantities of cell reactions (∆G, ∆H & K), derivation of cell EMF and single electrode potential; Standard hydrogen electrode- reference electrodes, standard electrode potential, sign conventions, electrochemical series and its significance.

7.00
Unit V: 
Electrochemistry II: Electromotive Force

Electrolytic and galvanic cells: Reversible and irreversible cells, conventional representation of electrochemical cells.

Concentration cell with and without transport, liquid junction potential, applications of concentration cell- valency of ions, solubility product, activity coefficient, potentiometric titrations.

Definition of pH and pKa, determination of pH using hydrogen, quinhydrone, glass electrodes and by potentiometric method.

Essential Readings: 
  • 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; G.M. Barrow; International Students Edition; McGraw Hill, New Delhi, 1994.
  • Physical Chemistry; G.M. Barrow; Sixth Edition; McGraw Hill, New Delhi, 1994.

 

Academic Year: 
2020-2021
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