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IIS Univ
  • Admissions

    It is a University which is committed to excellence and overall development of the student...

  • Placements

    Excellent education not only imparts knowledge, but also paves the way for...

  • Life@IIS Univ

    Life @ IISU is nothing less than a kaleidoscope of myriad hues; complete with...

  • Academics

    Taking the age-old tradition of enlightenment through education forward,...

  • Research

    To stimulate curiosity and cater to the global needs of a dynamic education,...

  • About Us

    The IIS University, with its perfect amalgamation of innovation, inspiration...

IIS (Deemed to be University)

Gurukul Marg, SFS, Mansarovar, Jaipur 302020, (Raj.) India

Phone:- +91-141-2400160-61, 2397906-07,

Fax: 2395494,2781158, Toll Free No.: 1800 180 7750

Applications of Thermodynamics | Chemistry

Applications of Thermodynamics

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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. be acquainted 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 

 

The students will be able to –

 

CO46: describe concept of Gibbs function, Helmholtz function and discuss their variation with pressure, volume and temperature.

CO47: deduce the thermodynamic relations of equilibrium constant with other thermodynamic properties.

CO48: explain heterogeneous equilibrium having one component and two component systems.

CO49: predict the notation of a single electrode, cell and measure its cell potential using the Nernst equation.

CO50: deduce the expression for EMF of concentration cell.

CO51: calculate valency of ions, solubility product, activity coefficient, thermodynamic properties and  pH of the given solution from EMF measurement.

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.

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; 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: 
2021-2022
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