Physical Chemistry II: Chemical Thermodynamics & Its Applications

Paper Code: 
24CCHY 212
Credits: 
4
Contact Hours: 
60.00
Max. Marks: 
100.00
Objective: 

This course will enable the students to

get acquainted with the laws of thermodynamics and their applications in chemical equilibria.

 

Course outcomes (COs):

Course

Learning Outcome

(at course level)

Learning and Teaching Strategies

Assessment Strategies

Course Code

Course

title

 

 

 

 

24CCHY 212

 

Physical Chemistry II: Chemical Thermodynamics & Its Applications

(Theory)

 

 

 

CO30: Describe the concept of first law of thermodynamics and apply it to calculate thermodynamic properties.

CO31: Explain the concept of second and third law of thermodynamics and apply it to derive different thermodynamic parameters.

CO32: Explain the thermodynamic properties of an open system.

CO33: Describe the concept of chemical equilibrium and apply it for the quantitative treatment of Le Chatelier’s principle.

CO34: Discuss the concepts of  colligative properties and apply these  properties to calculate molecular weight of solute.

CO35: Contribute effectively in course-specific interaction.

Approach in teaching:

Interactive lectures, tutorials, group discussions and e-learning.

 

 

Learning activities for the students:

Peer learning, e-learning, problem solving through tutorials and group discussions.

 

Written examinations, assignments and quiz.

 

 

13.00
Unit I: 
Chemical Thermodynamics I

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, relation between heat capacities, calculations of q, w, U and H for reversible, irreversible and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions, relation between Joule-Thomson coefficient and other thermodynamic parameters, inversion temperature.

Thermochemistry: Heats of reactions, standard states, enthalpy of formation of molecules and ions and enthalpy of combustion and its applications, calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data, effect of temperature (Kirchhoff’s equations) and pressure on enthalpy of reactions, adiabatic flame temperature, explosion temperature.

13.00
Unit II: 
Chemical Thermodynamics II

Second Law: Concept of entropy, 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 and A with T, V and P, free energy change and spontaneity, Gibbs-Helmholtz equation, Maxwell relations, thermodynamic equation of state.

 

10.00
Unit III: 
Systems of Variable Composition

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.

 

12.00
Unit IV: 
Chemical Equilibrium

Criteria of thermodynamic equilibrium, degree of advancement of reaction, chemical equilibria in ideal gases, concept of fugacity, thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient, coupling of exoergic and endoergic reactions, equilibrium constants and their quantitative dependence on temperature, pressure and concentration, free energy of mixing and spontaneity, 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.

 

12.00
Unit V: 
Solutions and Colligative Properties

Dilute solutions, lowering of vapour pressure, Raoult’s and Henry’s Laws and their applications, excess thermodynamic functions, thermodynamic derivation using chemical potential to derive relations between the four colligative properties and amount of solute, applications in calculating molar masses of normal, dissociated and associated solutes in solution.

Essential Readings: 
  1. Principles of Physical Chemistry, Forty Eighth Edition; B. R. Puri, L. R. Sharma, M. S. Pathania; Vishal Publishing Co., Jalandhar, 2020.
  2. An Introduction to Chemical Thermodynamics, Sixth Revised Edition; R.P. Rastogi and R.R. Misra; Vikas Publishing House, 2015.

 

References: 
  1. Atkin’s Physical Chemistry, Eighth Edition; P.W. Atkins, J. Paula; Oxford University Press, International Student Edition, 2017.
  2. Text Book of Physical Chemistry, Second Edition; S. Glasstone, Mac Million India, 1998.
  3. A Textbook of Physical Chemistry, Thermodynamics and Chemical Equilibrium, Vol. II, Sixth Edition; K. L. Kapoor; McGraw Hill Education Private Limited, 2019.
  4. Physical Chemistry, Fifth Edition; G.M. Barrow; McGraw Hill, New Delhi, 2015.
  5. Physical Chemistry Through Problems, Second Edition; S.K. Dogra and S. Dogra; New Age International Pvt. Ltd, New Delhi, 2015.

 

e-Resources:

 

  1. https://nptel.ac.in/courses/112105123 (Unit I & II)
  2. https://www.uou.ac.in/sites/default/files/slm/BSCCH-103.pdf (see Block 4 for Unit I)
  3. https://uou.ac.in/sites/default/files/slm/BSCCH-203.pdf (see Block 1 for Unit I, II and IV)
  4. https://chem.libretexts.org/Bookshelves/General_Chemistry/Book%3A_Genera...(Averill)/13%3A_Solutions/13.05%3A_Colligative_Properties_of_Solutions (Unit V)

 

Academic Year: