COURSE OUTLINE
Course Code: SCH 204
Course Name: Introduction to Reaction Kinetics and Electrochemistry
Introduction
This unit course is made up of two distinct parts: Introduction to Chemical Kinetics and Introduction to
Electrochemistry. In part one, students learn the basics of the subject of chemical kinetics: What it is; what is it
concerned with; what are the relevant concepts and terminologies of chemical kinetics; how do we express rates of
reactions in terms of the concentration of the participating species; how to determine rate laws for chemical
reactions; what factors affect rates of chemical reactions and how changes in temperature affect rates of reactions
and why. Under Introduction to electrochemistry, students learn about the chemical generation of electricity and the
use of electricity to cause chemical reactions to occur. In addition, students will be expected to understand the
practical importance of electrochemical processes in chemistry and in our everyday life.
Programme
B.Sc (Chemistry), Year 2
Lecture Time
Second semester
Venue
Second semester
Pre-requisite
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SCH 103 (General Physical Chemistry)
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SMA 103 (Calculus I)
Office Location
Chiromo Campus, Chemistry Department, Prefab Room 3
Consultation Hours
Second semester
Course Objectives
(i)
Introduction to Chemical Kinetics
At the end of this section, students should be able to:
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Know what chemical kinetics is with respect to the subject of chemistry.
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Define terms: Rate of reaction; Rate laws; Reaction order; Rate constant; Molecularity of a reaction;
Elementary reaction steps; Half-life; Activation energy and Arrhenius equation.
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Determine units of rate constant for a reaction of any order.
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Know what factors affect reaction rate constant, k and how.
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Know the different ways of expressing rates of reactions.
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Distinguish between the various methods of determining reaction rate laws.
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Distinguish between zero-, first-, second-, third- and nth-order reactions through their corresponding
integrated rate equations and half-life expressions.
(ii)
Know how temperature affects rates of chemical reactions and why.
Introduction to Electochemistry
At the end of this section, students should be able to:
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Define electrochemistry.
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Set-up electrochemical cells.
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Distinguish between primary cells and secondary cells.
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Determine the standard electrode (Reduction/Oxidation) potentials.
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Write electrochemical series; oxidation/reduction reactions and overall cell reactions.
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Define electrolysis.
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Relate the cell potential with the concentrations or pressures of the reagents and the products of a cell
reaction (Nernst Equation).
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Recite and apply the Faraday’s laws of electrolysis in terms of moles of electrons and substances.
-
Apply the principles of electroplating.
Detailed Course Content
Reaction rate processes and rate laws; order and molecularity of a reaction; first, second, third and pseudo order
reactions; determination of an order of a reaction; differential and integral rate equations; effect of temperature on
reaction rate; energy of activation; Arrhenius equation. Electrolysis; electrical units; electrolytic conductance; molar
conductance; conductance of solutions of strong and weak electrolytes; ionic conductance at infinite dilution.
Applications of conductance measurements - conductometric titrations and solubility of sparingly soluble salt.
Transference numbers and the methods of their determinations. Electrochemical cells: Electromotive force (emf) of
cells, the hydrogen electrode, the emf series and its uses, Nernst equation, concentration cells, the standard cell, the
principle of measurement of the emf of a cell. Applications (electrolysis of NaCl, electroplating).
Instructional Methods
1.
3 hours of lectures per week
2.
1 tutorial
3.
Homeworks
4.
Class discussions
Course Materials
The following reference materials (books, etc) are relevant for this course:
1.
Principles of general chemistry by Martin S. Silberberg. McGraw Hill, Inc, N.Y. 2007.
2.
Chemistry by Raymond Chang. MacGraw Hill, Inc, N.Y. 1991.
3.
Physical Chemistry by Peter Atkins; Juliode Paula, 7th Ed. Oxford University Press, Oxford, 2003.
4.
A textbook of Physical Chemistry by Negi A. S.; Anand S. C. New Age International (P) Limited,
Publishers, New Delhi, 2001.
5.
Physical Chemistry by Barrow G. M. McGraw Hill, Inc. New Delhi, 5 th Ed, 1992.
6.
Any other physical chemistry textboob(s) and any relevant website(s).
Evaluation
At the end of this course, students will be evaluated as follows:
1.
1 C.A.T = 30%
2.
1 Exam = 70%
Contact
The following are my contacts:
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Address: Dept. of Chem., Univ. of Nairobi, P.O. Box 30197, Nairobi.
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E-mail: Peterson.guto@uonbi.ac.ke
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Mobile: 0713 887854