SYLLABUS BS CHEMISTRY
Course Title
Environmental Chemistry
Course Code:
Credit Hours:
Objectives:
CHEM21113(3+0)
The students will be able to acquire:
The knowledge and develop understanding about the fundamental principles of
environmental chemistry and different types of pollutions.Such information will be useful in
studying and solving pollution related issues and experiments in the laboratory.
Course Outlines:
Atmospheric Pollution: The atmosphere, Composition, Temperature and pressure profile, Role
of free radicals in the atmosphere, Temperature inversion and photochemical smog, Particulate
matter in the atmosphere, Industrial pollutants, Atmospheric aerosols, Acid-rain major sources,
Mechanism, Control measures and effects on buildings and vegetation, Global warming, Major
greenhouse gases, Mechanism, Control measures and global impact, The stratospheric ozone–the
ozone hole, CFCs, Ozone protection, Biological consequences of ozone depletion.
Water Pollution: Water pollution and waste water treatment, Municipal, Industrial and
agricultural sources of pollution, Heavy metals contamination of water, Eutrophication,
Detergents and phosphates in water, Water quality criteria, Water purification: Primary,
Secondary and advanced treatment, Removal of nitrogen and phosphorous compounds from
polluted water, Organic matter in water and its decomposition.
Land pollution: Soil and mineral resources, General principles of metal extraction, Heavymetals
contamination of soil, Toxicity of heavy metals, Bio-accumulation of heavy metals, Organic
matter in soil, Macro and micro-nutrients in soil, Ion-exchange in soil, Soil pH and nutrients
availability.
Green Chemistry: Atom economy, Integrated pests management control (IPMC), Ionic liquids,
Super critical extraction technology, Green synthesis, Recycling, Carbon dioxide sequestering,
Water based paints.
Recommended Books:
Baird, C; Cann, M. Environmental Chemistry. W.H. Freeman& Company,Page 65 of 154
2012; 5thed.
Dara, S.S; Mihsra, D.D. A Text Book of Environmental Chemistry and Pollution Control.
S. Chand & Co, 2004;9thEd.
Singhi, R; Singh, V. Green Chemistry for Environmental Remediation. John-Wiley &
Sons, 2011.Page 66 of 154
Course Title:
Fundamentals of Physical Chemistry
Course Code:
CHEM1112
Credit Hours:4(3+1)
Objectives:
The students will acquire knowledge:
To understand the fundamental principles and laws of thermodynamics and chemical
equilibria.To investigate the physical properties of ideal/non-ideal binary solutions.About the
rates of reactions and perform related calculations.
Course Outlines:
Gaseous State: Equation of states, Ideal and real gases, Virial equation and the vander Waal‟s
equation for real gases, Critical phenomena and critical constants,
Chemical Thermodynamics: Four laws of thermodynamics and their applications, Thermo
chemistry, Calorimetry, Heat capacities and their dependence on temperature, pressure and
volume, Reversible and non-reversible processes, Spontaneous and non-spontaneous processes,
Relations of entropy and Gibbs free energy with equilibrium constant, Gibbs Helmholtz
equation, Fugacity and activity.
Chemical Equilibrium: General equilibrium expressions, Reaction quotients, Examples of
equilibrium reactions in solid, Liquid and gas phases, Extent of reactions and equilibrium
constants, Gibbs energies of formation and calculations of equilibrium constants, Le-Chatelier‟s
principle. Effect of temperature and pressure on the equilibrium constants/compositions, Van‟t
Hoff equation,
Liquid State: Physical properties of liquids, Surface tension, Viscosity, Refractive index, Dipole
moment and their applications, Brief account of interactions among the molecules in liquids
Solution Chemistry:, Ideal and non-ideal solutions, Raoult‟s law and its applications, Lowering
of vapor pressure, Elevation of boiling point, Depression of freezing point, Osmotic pressure,
Vapor pressure of non-ideal solutions and Henry‟s law, Abnormal colligative properties,
Degrees of association and dissociation of solutes, Osmotic pressure and its measurement,
Fractional distillation and concept of azeotropic mixtures.
Chemical Kinetics: The rates of reactions zero, First, Second and third order reactions with
same and different initial concentrations, Half-lives of reactions, Experimental techniques for
rate determination and methods for determination of order of reaction, Arrhenius equation.
Practicals:
Determination of viscosity of liquids.
Determination of refractive index of liquids.
Determination of percent composition of liquid solutions viscometrically.
Determination of refractive index and molar refractivity.
Determination of percent composition of liquid solutions by refractive index
measurements.
Determination of molecular weight of a compound by elevation of boiling point
(ebullioscopic method).
Determination of molecular weight of a compound by lowering of freezing point
(cryoscopic method).
Determination of heat of solution by solubility method.
Determination of heat of neutralization of an acid with a base.
Kinetic study of acid catalyzed hydrolysis of ethyl acetate.
Determination of partition coefficient of a substance between two immiscible liquids.
Recommended Books:
Atkins, P; Paula,J.D. Atkin‟s Physical Chemistry. Oxford University Press, 2010;9thEd.
Shoemaker, D. Experiments in Physical Chemistry.McGraw Hill, 2003; 8thEd.
Silbey, R; Alberty, R; Bawendi, M. Physical Chemistry.2005,4thEd.
Glasstone, S. Textbook of Physical Chemistry. Macmillan London, 1960.
James, A.M; Prichard, F.E. Practical Physical Chemistry. Longman Group Limited: New
York, 1974;3rdEd.
Chaudhary, S.U. Ilmi Textbook of Physical Chemistry, Ilmi Kitab Khana: Lahore,
2013;2ndEd.
Atkins, P; Jones, L. Chemical Principles: The Quest for Insight. W.H.
Freeman: New York, 2010;5thEd.
