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A course consisting of about ro lectures, together with three hours' tutorial and discussion work per week during first and second terms, and the completion of the design of a chemical plant to meet a specified production requirement, together with a review of its economics.


The design of a chemical plant to meet a specified requirement. The sequence for investigation of a chemical manufacturing project and the preparation of a report on the work. This includes the preparation of flowsheets, the consideration of the effects of market forecasts, economic evaluation, estimates for and minimization of capital and production costs, the specification of equipment, the selection of appro- priate materials of construction, instrumentation location, the requirements of staff and labour, and safety precautions.



Buchanan, R. H. and Sinclair, C. G., (Eds.) Costs and Economics of the Australian Industries. (West.)

Vilbrandt, F. C. and Dryden, C. E., Chemical Engineering Plant Design. (McGraw-Hill.) EXAMINATION

Students will be assessed on the design project completed during the course.


A course of three lectures per week during Terms I and II, with laboratory work throughout the year.

Pre-requisite Standard. While there is no pre-requisite, it is strongly recommended that the students beginning the course should have a background of descriptive chemistry and basic chemical theory equivalent to Matriculation Chemistry. A knowledge of the subject up to this standard will be assumed as a basis for the course.


The course will consist of a treatment of basic physical, inorganic and organic chemistry, emphasizing aspects of the subject of importance in engineering investigations and practice.

The following syllabus provides a general guide to the topics to be discussed.


Chemical Kinetics. Factors influencing the rates of chemical reactions; collision theory of reaction. Catalysis—homogeneous and heterogeneous, with applications.

Chemical Equilibrium. Acid-base equilibria, calculation of pH, buffer solutions, indicators, titration curves. Complex ion equilibria.

The Properties of Gases, Liquids and Solids. The Kinetic theory of matter. The ideal gas equation; real gases and deviations from ideality; van der Waals' equation; liquefaction of gases and critical phenomena. The liquid state. Crystalline solids—metals, ionic, valence and molecular crystals. Crystal defects. The band theory of solids. Influence of bond type on physical and chemical properties of crystalline solids. Solid-liquid-gas equilibria for one-component systems : the Phase Rule.

Solutions. Two-component systems; solutions; the properties of gas-gas, gas-liquid. liquid- liquid and solid-liquid systems. Fractional distillation. Distribution law. Colligative properties of dilute solutions.

Thermochemistry. The first law of thermodynamics; heat and work; internal energy and enthalpy; calorimetry; heat of combustion; the laws of Hess and Kirchhoff. Combustion of fuels.

Electrochemistry: Conductance of electrolyte solutions and the ionic theory. lxidation reduction equilibria, redox indicators, titration curves; electrode potentials; electrolytic cells•, measurement of hydrogen ion concentration. Electrolysis. Overvoltage. Electro- deposition of metals. Corrosion. Factors influencing corrosion and methods of cопtrоl- ling it.

Surface Chemistry and the Colloidal State. Surface phenomena. The colloidal state:

lyophobic and lyophilic sols. Viscosity of proteins. Gels. Emulsions. Chromatography.

Theory of Chemical Analysis. The theory and procedure involved in volumetric analysis such as is given in the laboratory work. Conductornetric titrations; potentiometriс titra- tions. Spectrophotometry.

Radiochemistry. Measurement of radioactivity; properties of radioactive isotopes and their applications to some typical chemical problems. The Szilard-Chalmers 'recoil effect'.


The properties of homologous series. Aliphatic and aromatic hydrocarbons and their simpler derivatives. The main functional groups. Fuels; Plastics—thermosetting and thermoplastic, polymerization; other organic engineering materials.


Three hours per week throughout the year, covering quantitative analytical chemistry and general inorganic, physical and organic chemistry, the experiments being chosen to illustrate, amplify and extend the theory course.

The practical classes for this subject are taken in the Chemistry Laboratory of the

Redmond Barry Building. The department supplies all the apparatus for which a fee of $iо must be paid to the University Branch of the National Bank, using a specially stamped bank slip obtained from the Laboratory. Evidence of payment must be pro- diced to the Laboratory before practical classes begin. The full fee is retained as no charge will be made for reasonable wear and breakage.


(a) Recommended for preliminary reading:

Stranks, D. R., Heffernan, M. L., Lee Dow, K. C., МcTigue, P. T. and Withers, G. R., Chemistry: A Structural View. (M.U.P.)

Diamant, R. M. E., Applied Chemistry for Engineers. (Pitman.)

Sienko, M. J. and Plane, R. A., Chemistry: Principles and Properties. (McGraw-Hill, 1966.)

(b) Prescribed text-books:

*Glasstone' S. and Lewis,


Elements of Physical Chemistry. (Macmillan.) or *Barrow, G. M.. Physical Chemistry. (znd ed., McGraw-Hill, 1966.)

or Ander, P. and Sonnessa, A.


Principles of Chemistry: An Introduction to Theoretical Concepts. (Collier-Macmillan, 1965.)


B. H., University Chemistry. (Addison-Wesley, 1965.)

or Andrews, D. H. and Kokes, R.


Fundamental Chemistry. (znd ed., Wiley, 1965.)

*Diver, N.


(ed.), Departmental Publications:

Experiments in Inorganic and Physical Chemistry. (1968 edition.) Experiments in Organic Chemistry. (1968 edition.)

(These laboratory handbooks are available only from the Chemistry Laboratory, Red- mond Barry Building.) .

((•) Recommended for reference:

Glasstone, S., Textbook of Physical Chemistry. (nd ed., Macmillan.) Moore, W. J., Physical Chemistry. (4th ed. Longmans.)

Addison, W. E.. Structural Principles in Inorganic Compounds. (Longmans.)

liver, N. H. (ed.), Fundamental Aspects of Chemistry 1963. (Dept. of Chem., U. of M.) Van Vlack, L. H., Elements of Materials Science. (2nd ed., Addison-Wesley.) Mackenzie, C. A., Unified Organic Chemistry. (Harper International Student Reprints

—Harper & Row, 1g6z.)

Bezant, R. J. Basic Organic Chemistry. (McGraw-Hill, 1966.)

Brown, R. D. and O'Donnell, T. A., Manual of Elementary Practical Chemistry. (3гd ed., M.U.P.)

koithoti, I. M. and Sandell, E. B., Textbook of Quantitative Inorganic Analysis. (3rd ed., Macmillan.)

Vogel, A. I., A Text-book of Quantitative Inorganic Analysis including Elementary Instrumental Analyses. (3rd ed., Longmans.)

Findlay, A. and Kitchener, J. A., Practical Physical Chemistr . (8th


Longmans.) Daniels, F., Williams, J. W., Bender, P.. Alberty, R. A. andyCornwell, C. D., Experi-

men tal Physical Chemistry. (6th ed., McGraw-Hill.)

Aylward, G. H. and Findlay, T. J. V., Chemical Data Book. (and


Wiley, 1966.) EXAMINATION

One 3-hour written paper, for Pass and Honours combined. There will be no practical examination, but the standard of the student's laboratory work will be assessed con- tinually throughout the year, and is taken into account in determining the success of the candidates at the Annual Examination.



A course of three lectures, one tutorial per week and laboratory work throughout the year. A preliminary standard equivalent to Matriculation Chemistry will be assumed. The syllabus is basically similar to that of the Chemistry IA course with the restriction that certain subjects arc not developed so fully.



Experimental methods; methods of measurement and analysis including manometry, spectrophotometry, conductance and potential measurements.

Chemical equilibrium: homogeneous and heterogeneous equilibria in gases and solution;

determination of equilibrium constants.

Properties of electrolytes as found from conductance measurements; molar conductance;

law of independent ionic migration; conductometric titrations.

Oxidation—reduction equilibria; reduction potentials; Nernst equation; half cells, cell reactions; equilibrium constants; potentiometric measurements and application to the

determination of pH, pКg, K,, etc. redox indicators; free energy changes during redox reactions, relation to equilibrium constants; standard free energies.

Electrolysis; decomposition and discharge potentials; overpotential; order of discharge.

Solubility equilibria; determination of solubility and solubility products; calculation of solubilities involving simultaneous equilibria, complex ions; precipitation titratioes.

Acid/base equilibria; calculation of pi from fundamental principles; buffer solutions; poly- protics; titration curves, indicators; acids and bases in non aqueous solvents.

Gases: ideal and real gases; kinetic theory of gases,* deviations from ideal gas behaviour and interpretation in terms of modification of kinetic theory postulates; van der Waals' equation; critical state; liquefaction.

Phase Equilibria : one component systems, P-V and P-T diagrams; polymorphism and metastable states. Two component systems; gas-liquid, liquid-liquid and liquid-solid systems; partial miscibility; distribution law; ideal and non ideal solutions; distillation;


Chemical kinetics: measurement of reaction rate; rate laws; factors affecting rate: con- centration (order; rate expressions for first and second order reactions); temperature;

catalysts; radiation. Simple collision theory model for reaction mechanisms; collision frequency; energy distributions; activation energy.

Thermodynamics: thermodynamic properties, heat and work, functions of state U and H; heat absorbed at constant volume and at constant pressure, specific heats, Kirchoff's Law.

*Note: Detailed formulation of the ist Law of Thermodynamics and the Kinetic Theory of Gases will not be presented but will be assumed to be known from coverage in Physics I. Students not taking physics will be supplied with a reading list to cover these topics to a suitable level.


Atomic Structure and the Theory of Valency: electrovalent, covalent, dative, hydrogen, metallic and van der Waals' bonding.

Structure of Solids: influence of bond type on chemical and physical properties and type of structure.

Introduction to Co-ordination Chemistry: Werner's theory of cobalt and platinum ammines, inorganic stereochemistry, isomerism, chelating ligands, aquo, ammino and halide complexes of selected cations, stability constants.

Periodic Classification: comparative chemistry of selected groups and periods of elements with special reference to periodicity and electronic configuration.


The scope of organic chemistry—Bonding, structure, and elementary stereochemistry of carbon compounds. An outline of the chemistry of hydrocarbons and their monotunc- tional derivatives in terms of molecular structure and the electronic mechanisms of reactions.


Three hours per week, throughout the year, illustrating the principles of inorganic, physical and organic chemistry together with exercises in quantitative and qualitative analysis.

The practical classes for this subject are taken in the Chemistry Building. The department supplies all the apparatus for which a fee of $io must be paid to the University Branch of the National Bank, using a specially stamped bank slip obtained from the department.

Evidence of payment must be produced to the department before practical classes begin.


(a) Recommended for preliminary reading:

Pauling, L., General Chemistry. (Freeman.)

Strапks, D. R. et al., Chemistry-A Structural View. (M.U.P.)

The content of lectures in Chemistry I B will be based on the assumption that all students have read the text-book by Stranks et al.

(b) Prescribed text-books:

Glasstone, S. and Lewis, D., Elements of Physical Chemistry. (Macmillan.) or Mahan, B. H., University Chemistry. (Addison-Wesley.)

Bell, C. F., and Lott, K. A. K., Modern Approach to Inorganic Chemistry. (Butterworth.) Allinger, N. L. and Allinger, J., Structures of Organic Molecules. (Prentice-Hall.) Saunders, W. H., Ionic Aliphatic Reactions. (Prentice-Hall.)

Tedder, J. M. and Nechvatal, A., Basic Organic Chemistry. (Wiley.)

*Departmental Publication—Experiments in Chemistry. (1968 ed.) (This laboratory hand- book is available only from the School of Chemistry.)

Aylward, G. H. and Findlay, T.


V. (eds), Chemical Data Book. (2nd ed., Wiley, 1966.) (c) Recommended for reference:

Daniels, F. and Alber ty, R. A., Physical Chemistry. (3rd'ed., Wiley.) Gilreath, E. S., Fundamental Concepts of Inorganic Chemistry. (McGraw-Hill.) Gould, E. S., Inorganic Reactions and Structure. (Holt.)t

Brown, R. D. and O'Donnell, T. A., Manual of Elementary Practical Chemistry. (3rd ed., M.U.P.)

Books marked


are used by students proceeding to Chemistry


and Chemistry III.


One 3-hour paper in Physical Chemistry, one a-hour paper in Inorganic Chemistry and one 2-hour paper in Organic Chemistry.

The practical work of each student is assessed continually throughout the year, and is taken into account in determining the success of candidates at the Annual Examination.