Sathyabama Institute of Science and Technology B.Sc - Chemistry SCY1316 Physical Chemistry-II Syllabus

[Arvind Kumar]

Sathyabama Institute of Science and Technology B.Sc - Chemistry SCY1316 Physical Chemistry-II Syllabus

SATHYABAMA INSTITUTE OF SCIENCE AND TECHNOLOGY DEPT. OF CHEMISTRY

SCY 1316 PHYSICAL CHEMISTRY-II
L T P C Max. Marks
3 1 0 4 100

UNIT 1 THERMODYNAMICS-II 12 Hrs.
Need for the II law – Statements of the second law – Spontaneous process – Carnot’s cycle – Efficiency – Carnot's theorem (statement only) – Concept of
entropy – Definition – Entropy of an ideal gas – Entropy changes in cyclic, reversible and irreversible processes and physical transformations –
Calculation of entropy changes with changes in T, V, P and entropy of mixing – Gibbs free energy – Helmholtz free energy: their variations with
temperature, pressure and volume – Criteria for spontaneity – Gibbs-Helmholtz equations – derivation and applications – Chemical potential – Gibbs-
Duhem equation - Effect of temperature and pressure on chemical potential – Chemical potential in system of ideal gases – Duhem-Margules equation –
Clausius-Clapeyron equation - Derivation and uses – Nernst heat theorem - Third law of thermodynamics (statement only) – Fugacity (Definition), activity
and activity coefficient.

UNIT 2 ELECTROCHEMISTRY-II 12 Hrs.
Galvanic cells – Reversible and irreversible cells – Western Cadmium Standard cell – Emf and its measurements – Relation between free energy and EMF:
Gibbs-Helmholtz equation – Thermodynamics of a cell reaction – Nernst equation of electrode reaction – Types of reversible electrodes – Single and
standard electrode potential – Reference electrode – SHE – Electrochemical series and its significance – Concentration cell with and without transference –
Liquid junction potential – Applications of EMF measurements – Determination of i) Valency of ions, ii) Solubility product, iii) pH using hydrogen,
quinhydrone and glass electrodes – Potentimetric titration.

UNIT 3 CHEMICAL KINETICS-II 12 Hrs.
Effect of temperature on the rate of reactions – Concept of activation energy: Arrhenius equation – Collision theory of bimolecular and unimolecular
reactions: Lindemann hypothesis – Theory of absolute reaction rates (ARRT) – Parallel, Consecutive, opposing (No derivation) – Chain reactions: H2 – Br2
reaction (steps only. No kinetics required).

UNIT 4 SURFACE CHEMISTRY AND CATALYSIS 12 Hrs.
Adsorption – Physisorption and chemisorption – Adsorption of gases by solids – Freundlich adsorption isotherm – Langmuir adsorption isotherm –
Limitation of Langmuir theory – BET equation (no derivation) – Applications of adsorption – Homogeneous catalysis – Acid-base catalysis – Enzyme
catalysis – Michaelis-Menten equation – Heterogeneous catalysis – Mechanism of unimolecular reactions.

UNIT 5 PHYSICAL PHOTOCHEMISTRY 12 Hrs.
Photochemical reactions – Lambert’s law – Beer’s law – Grotthus-Draper law – Quantum efficiency – Quantum yield – Primary and secondary process –
Dissociation of HI – Kinetics of Hydrogen-bromine reaction – photosensitization – Chemiluminescence – Phosphorescence.
Max. 60 Hrs.

COURSE OUTCOMES
On completion of the course, student will be able to:
CO1:Understand the spontaneity and learn the derivations of various thermodynamic functions.
CO2:Explain the applications of electrode potential and electromotive force.
CO3:Interpret theories of reaction rates.
CO4:Understand and relate unimolecular and multimoecular layer adsorption.
CO5evelop the knowledge of the different types of catalysis.
CO6:Learn the laws of kinetics in photochemical reactions and importance of photochemical processes.

TEXT/REFERENCE BOOKS
1. B. R. Puri and L.R. Sharma, Principles of Physical Chemistry, Shoban Lal Nagin Chand and Co. 23rd edition, 1993.
2. ArunBahl, B. S. Bahl and G. D. Tuli, Essentials of Physical Chemistry, S. Chand publishing, 2012.
3. P.W. Atkins, Physical Chemistry, 7th Ed.,Oxford university press, 2001.
4. Glasston& Lewis, Physical Chemistry, 2nd Edition, McMillan publishers, 1973.
5. A.S. Negi and S. C. Anand, A Textbook of Physical Chemistry, New Age International, 2004.

END SEMESTER EXAM QUESTION PAPER PATTERN
Max. Marks: 100 Exam Duration: 3 Hrs.
PART A: 10 Questions of 2 Marks each-No choice 20 Marks
PART B: 2 Questions from each unit of internal choice, each carrying 16 Marks. 80 Marks
(Out of 100 Marks, maximum of 10% problems may be asked.)