CHEM-5101                             Physical Chemistry                              4 (3+1)

This course is the first part of this program, introduction to Physical Chemistry. This foundation course of physical chemistry covers basic knowledge and its application for learning chemical principles of physics to chemistry. This offer complementary approaches to the fundamental understanding of chemical systems. Students will acquire knowledge to enable themselves to understand the kinetic theory of gases, collision theory of reactions, fundamental principles and laws of thermodynamics and chemical equilibria and to investigate the physical properties of ideal/non-ideal binary solutions. Students will also be able to study the rates of reactions and perform related calculations. The general goal of learning physical chemistry is to obtain a vision of matter-energy relationship in physical and chemical systems. Learning objectives emphasized in CHEM 5101 involve developing an understanding of basic principles of physical chemistry. Students learned in class to modern physical chemistry techniques which give them opportunities to see how Physical Chemists are solving current, real-world problems.

Contents

1. Elementary Mathematics: Logarithmic, exponential and trigonometric functions, differentiation of elementary functions, methods of differentiation and integration, significance of differentiation and integration.
2. Physical States of Mater: Gases (van der Waal’s equation, critical Phenomena, Critical values of T, P andV., liquification of gases, molecular collisions, collision diameter, mean free path) Liquids (viscosity, Parachor value, Refractive index, molar refraction and its applications. Dipole moment, Solids (Unit cells. Bragg crystal analysis, crystal structure of NaCl, powder method of crystal structure analysis).
3. Atomic Structure: De Brogile equation. Schrodinger wave equation, solution for particle in 1D box, quantization concept, Heisenberg Uncertainty Principle, Pauli Exclusion Principle, Hund’s Rule.
4. Chemical Thermodynamics: First law of thermodynamics, state functions, isothermal and adiabatic processes in ideal gases, heat capacity, reversible and irreversible processes. Spontaneous and non-spontaneous processes, second law of thermodynamics, change of entropy with change in T, P andV.
5. Chemical Equilibrium: Law of Mass Action, equilibrium constant, relationship between Kc, Kp, Kx and Ka and LeChaterlier’s Principle.
6. Solutions: composition, ideal and non-ideal solutions. Raoult’s law. Colligative properties, ebullioscopy, cryoscopy, osmotic pressure, distillation and concept of azeotropes.
7. Chemical Kinetics: Zero, first and second order reaction, Arrhenius equation, activation energy, Lindemann’s mechanism, collision theory and transition state theory.
8. Electrochemistry: Conductance, dependence of conductance on the nature of solvent and temperature, Kohlrausch’s law and its applications, measurement of conductance strong and weak electrolytes, degree of dissociation.

Physical Chemistry Lab

1. Determination of surface tension and Parachor value by stalagmometer.
2. Determination of percent composition of liquid solutions from surface tension measurement.
3. Determination of viscosity and Rhechor value of liquids from viscosity measurement.
4. Determination of percent composition of liquid solutions viscometrically.
5. Determination of refractive index and molar refractivity by refractometer.
6. Determination of percent composition of liquid solutions by refractive index measurements.
7. Determination of heat of solution by solubility method.
8. Determination of heat of neutralization of an acid with a base.
9. A kinetic study of acid hydrolysis of ethyl acetate.
10. Kinetic study of saponification of ethyl acetate.
11. Determination of molecular weight of a compound by elevation in boiling point. (Ebullioscopic method).
12. Determination of molecular weight of a compound by lowering of freezing point (The Cryoscopic methods).
13. Determination of equilibrium constant of KI – I2 Kl3.
14. Conductometric titration of strong acid and strong base.

Recommended Texts

1. Atkins, P., Paula, J., and Keeler, J. (2017). Atkins' Physical Chemistry (11th ed.), Oxford University Press.
2. Kuhn, H. Försterling, H. Waldeck, D.H. (2009). Principles of Physical Chemistry (2nd ed.), Wiley Publisher.

Suggested Readings

1. Akhtar, M.N. and Nabi, G. (2006). Text Book of Physical Chemistry. Ilmi Kitab Khawna, Lahore.
2. Das, R.C., and Behera, B. (2003). Experimental Physical Chemistry. Tata McGraw Hill, Delhi.

Assessment methodology

• Sessional: 15% (Presentations: 10%, Partcipation: 5%)
• Practical: 25% 
• Midterm exam/ Term paper: 15%
• Final exam: 45%

Classes:

BS Chemistry I (R)

Time Table