Download CHM314 COURSE COMPACT Course CHM 314 Experimental

CHM314 COURSE COMPACT
Course
Course code: CHM 314
Course title: Experimental Physical Chemistry
Credit unit: 1
Course status: Compulsory
Course Duration
Three hours per week for 15 weeks (45 hours)
Time of Lecture: Monday (2pm – 5pm)
Lecture Location:
Chemistry Laboratory
Time of Lecture:
Monday (2 – 5pm)
Lecturer’s Data:
1. Name of the Lecturer: DADA, Oluwasogo Adewumi
Qualifications obtained: B.Sc (Hons), M.Sc (Chemistry), MCSN, MSAN
College: College of Science and Engineering
Department: Physical Sciences
Unit: Industrial Chemistry
E-mail: [email protected]
Office Location: 1st College Building, 1st Floor, A132.
Consultation Hours: Monday – Wednesday: 2 – 4pm
Thursday – Friday: 12 – 2pm
 Course Content:
CHM 314: Experimental Physical Chemistry II (1 Unit)
Determination of rate, rate constant and activation energy of a reaction.
Determination of standard thermodynamic quantities of a reaction, phase rule.
Application of electrochemical principles in titration reactions. Conductance
measurements. Viscosity measurements.
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 Course Justification:
This course will provide strong foundation in Experimental Physical Chemistry that
can be built upon later and it will also prepare students for relevant approaches to
some aspects of production in the industries through the knowledge of
thermodynamics. Therefore, the course becomes highly imperatives for students
who will finds relevance in Production arm of the Industry.
 Course objectives
The course objectives and goals are:
i.
It is to provide strong practical foundation in Physical Chemistry that would be a basic
tool for their relevance in the industries.
ii.
It will give students opportunity to learn the techniques involved in physical chemistry,
and make them develop a careful, painstaking and a critical analytical attitude to
practical work.
iii.
Also, it will prepare students for relevant approaches to some aspects of data analyses
and some laboratory techniques which will later be useful in their final year research
and career in future.
 Course Requirement:
You are strongly advised to read the manual carefully before you come to the
laboratory. An attempt has been made to explain the theory of basic principle behind each
experiment to enable you understand what is going on. To be able to perform an
experiment successfully and enjoyably it is imperative that you should read the script for
the experiment thoroughly before doing the experiment. It should be borne in mind that in
general it is of little value to carry out a set of instruction without understanding what the
experiment is really about. One way of ensuring that you have read thoroughly the script of
an experiment is to prepare a table of reading to be taken before you proceed to do the
experiment. The table of results should be such that you can record directly the results of
your measurements.
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1. Students should work in pairs, but laying out the table of results, calculations and
writing up should be done individually. However, laying - out of table of results and
calculations may be crossed – checked with the partners. Each experiment must be
written up in the laboratory and submitted for marking at the end of the period.
Remember that the experiments in this manual are designed to be finished and
reported in one 6 hour laboratory period. However, in order to be able to finish you
must organize your time and plan your work carefully.
2. Marks will be awarded for good lay – out of results, precision, accuracy and
understanding. A precise result is one in which successive values are close to each
other and an accurate result is one in which the experiment value is very close to the
true value. If there are no systematic or instrumental errors then precision and
accuracy are equivalent but an incorrectly calibrated instrument for example could
be read to high level of precision and still give inaccurate results.
 THE LABORATORY NOTEBOOK AND FORMAT OF LABORATORY REPORT
An essential part of any laboratory experience is the keeping of full and accurate records. The
laboratory report book is one of the most valuable pieces of equipment the chemist uses. A
properly prepared notebook can be examined at any time to determine what actions were
performed, what transpired during the experiment, what results and conclusions were
obtained, and even what was done incorrectly or improperly. Another chemist should be able
to use a laboratory notebook to repeat an experiment to obtain results identical to those of the
original investigator.
When scientists perform experiments, they make observations, collect and analyze data, and
formulate generalizations about the data. When you work in the laboratory, you should record
all your data in a laboratory report. An analysis of data is easier if all data are recorded in an
organized, logical manner. Tables and graphs are often used for this purpose.
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The format of your laboratory exercise is given below:
i.
Title: The title should clearly describe the topic of the report.
ii. Objectives: Write a statement to express your expectations of the results and as an answer
to the problem statement.
iii. Materials: List all laboratory equipment and other materials needed to perform the
experiment.
iv. Procedure: Describe each step of the procedure so that someone else could perform the
experiment following your directions.
v. Results: Include in your report all data, tables, graphs, and sketches used to arrive at your
conclusions.
vi. Conclusions: Record your conclusions in a paragraph at the end of your report. Your
conclusions should be an analysis of your collected data. Essential conclusions of
calculations and results in a clear and systematic manner and where possible, these should
include accepted literature values. All symbols must be defined and units indicated. For
instance an account which concludes with the statement “X = 20” where X has not been
defined and its unit has not been stated is meaningless. The conclusion should include brief
discussion on major sources of errors and how to improve the experiments.
Note: No information should be written on scraps of paper, however temporary in plan.
According to good laboratory practice (GLP), all entries should be recorded directly into the
laboratory report. All entries should be documented in terms of name of material, units, etc., in
blue or black ink, never in pencil. No entry should be erased or heavily marked over; one neat
line should be drawn through and initialed for each incorrect or undesired entry to signify that
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it is discarded. Each page should be numbered in the upper right corner, the numbers running
consecutively throughout the laboratory report. The first two pages should be reserved for a
Table of Contents. Pages should never be torn out of the laboratory report, and pages should
not be skipped or left blank.
 Alignment with Goals and Vision of Landmark University: To build a total man and
intelligent student who will break a new ground in the field of Science and Engineering.
 Contemporary Issues/ Industry Relevance:
Most of the topics covered under the course would provide strong foundation for the
students in areas of Science and Engineering.
It will provide knowledge on the Chemistry of clay and the technology behind
Composite Materials.
 STRUCTURE OF PROGRAMME/METHOD OF GRADING:
This course has been structured such that the student will compulsorily visit the
laboratory for his/her practical laboratory per week. Pre-laboratory test will be
attempted before coming to the laboratory. Students will be divided into groups for
presentation before Alpha semester examination will be done. The weekly practical
exercises together with the presentation will be graded 50% while the Alpha semester
examination will also be graded 50% following the NUC standard.
 Course Delivery Strategies:
Provision of detailed explanation on different experiments that will be carried out for
proper understanding of the subject matter. Solving of pre-laboratory exercises.
Practical Manual will be provided for proper guidelines
Recommended Readings:
1. Findlay, Practical Physical Chemistry
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2. Glasstone, Textbook of Physical Chemistry, p. 745 – 9
3. Moore, Physical Chemistry p.145 – 147
4. Vogel, Quantitative Inorganic Chemistry
 Brief Overview of Course
These experiments are practical aspects of what will be done in CHM 311. It will cut
across Determination of rate, rate constants and activation energy of a reaction.
Determination of standard thermodynamic quantities of a reaction , Phase Rule.
Application of electrochemical principles in titration reactions. Conductance
measurements. Viscosity measurement. Note: The experimental work will be done for
three hours within which students are required carry out the practical by following the
procedures in the practical manual provided and gather their data after which they
will attempt questions base on the practical.
Course Outline:
 Week 1: Experiment 1: Phase Rule
 Objectives:
- To determine the phase rule: two component solid-liquid system
- To draw phase diagram of naphthalene and naphthol
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Questions:
i.
Define Phase Rule
ii.
State the Phase Rule equation and define the meaning of each parameter in
the equation.
iii.
From the data collected, draw a labeled Phase diagram
 Week 2: Experiment 2: Distribution Co-efficient of Iodine Between Carbon Tetra
Chloride and Water
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 Objective:
- To determine the distribution coefficient of the Iodine Between Carbon Tetra
Chloride and Water
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Question : Give a vivid report of the experiment
 Week 3: Experiment 3: pH – Its Measure and Applications
 Objective:
- To carry out Measurement of The pH of Typically Salt Solution
- To Determine The Dissociation Constant of Weak Acid
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
1.
2.
3.
4.
5.
 Study Questions:
Simple define a buffer solution and explain how to prepare both acidic and alkaline
buffer solutions
From the experimental data, determine the dissociation constant of the weak acid
Calculate the pH of a 0.25moldm-3 solution of phenylamine Kb for phenylamineis
4.8x10-4 moldm-3
Find the pH of a solution of 0.06M ethanoic acid if Ka = 1.8x10-5moldm-3
Find the degree of dissociation of a 0.2moldm-3 solution ethanoic acid if the pH is 5
 Week 4: Experiment 4: Spectrophotometer Determination of the Acid
Dissociation Constant
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 Objectives:
1. To determine the absorption spectrum of each from of methyl red.
2. To Verify the Beer-Lambert’s law
3. To Determine the values of pK from the experimental data obtained
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Question
1. Determine the pH value of each solution and measure the absorbance of each
solution at two wavelengths chosen to enable you to calculate the concentration of
both the acid and basic form of the indictor in the solution.
 Week 5: Experiment 5: Thermodynamics: Determination of Heat of Neutralization
 Objective: To determine the heat of neutralization for the acid-base reaction
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Questions:
1. Define the Heat of Neutralization
2. Plot the graph of time against temperature and explain what can be deduced from
the graph.
 Week 6: Experiment 6: Thermodynamics: Determination of Heat of Solution
 Objective: To Determination of Heat of Solution
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 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions

1.
2.

Study Question
Define the Heat of Solution, Lattice Energy and Hydration energy
From the experimental data, plot the graph time against the temperature.
Week 7: Experiment 7: Thermodynamics: Simultaneous Determination of Several
Thermodynamics Quantities (K, ∆Go, ∆Ho, ∆So)
 Objectives:
1. To standardize hydrochloric acid solution
2. To determine the solubility product of Borax as a function of temperature
3. To determine the standard free energy, standard enthalpy and standard entropy
change for the dissolution of borax in an aqueous solution (∆Go, ∆Ho, ∆So)
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Questions:
1. Calculate values for the solubility product constant (Ksp) for borax at the various
temperatures.
2. Plot ln Ksp vs. 1/T for all ten samples. Determine ∆H (kJ/mol) and ∆S (J/mol K) from this
graph.
3. Calculate the values for ∆G for each sample from the experimental data collected:
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 Week 8: Experiment 8: Using Beer Lambert’s Principle for the Determination of
Manganese in a Steel Sample
 Objective: Determination of Manganese in a Steel Sample using Beer Lambert’s
Principle
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Question:
1. Measure the optical density of the solution. Using the calibration curve
obtained,
2. Calculate the concentration of potassium permanganate from the steel and
hence calculate the percentage of manganese in the steel sample.
 Week 9: Experiment 9: Chemical Kinetics I: Investigation of Effect of Temperature on
the Reaction between Oxalic Acid and Potassium Permanganate System
 Objective:
To investigate the effect of Temperature on the reaction betewwen H2C2O4(aq) and
KMnO4(aq)
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Questions:
1. State the effect of temperature on the kinetics of the reaction between
H2C2O4(aq) and KMnO4(aq)
2. From the experimental data collected, plot an appropriate graph.
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 Week 10: Experiment 10: Chemical Kinetics II: Determination of the Reaction Time,
Order of Reaction and the Specific Rate Constant
 Objectives:
1. To determine the rate law for a chemical reaction
2. To utilize a graphical analysis of experimental data to determine the order of each
reactant in the reaction.
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Question:
1. Calculate the rate of reaction using:

 (mol I 3 )
rate 
and compute the logarithm of the reaction rate.
t
2. Calculate the initial molar concentration of [I-]o and logarithm of initial molar
concentration of the iodide ion, log [I-]o for each kinetic trial.
3. Calculate the initial molar concentration of [H2O2]o and the logarithm of initial
molar concentration , Log [H2O2]o for each kinetic trial

4. Plot the graph of
rate 
 (mol I 3 )
versus Log [I-]o at constant hydrogen
t
peroxide concentration and determine the order of reaction p
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
 (mol I 3 )
5. Plot the graph of rate 
versus Log [H2O2]o at constant Iodide ion
t
concentration and determine the order of reaction q using the kinetic trial 1, 5,
6,and 7
6. Determine the specific rate constant k’ for the seven solutions using the rate law:
rate 
(mol I 2 )
 k ' [ I  ] P [ H 2 O2 ] q . Calculate the average value of k’ with proper units. Also
t
determine the standard deviation and the relative standard deviation (%RSD) of k’ from
your data.
 Week 11: Experiment 11: Chemical Kinetics III: Determination of Energy of Activation
 Objective:
To determine the activation energy of reaction.
 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Question
1. Plot the graph of lnk’ versus 1/T(K) for at least three trials at which the experiment was
performed. Take R= 8.314J/mol/K. From the appropriate plot, determine the Activation
energy
 Week: Experiment 12: Chemical Kinetics II: Determination of the Order of Reaction
and the Specific Rate Constant of a Reaction without using a Buffer Solution
 Objective: To determination of the order of reaction and the specific rate constant of a
reaction without using a buffer solution
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 Description:
First Hour: General Class briefing and demonstration of the practical.
Second and Third hours: Data Collections; Treatment of data and Solving of other
practical questions
 Study Question:
From your data:
1. Calculation the rate and logarithm of the rate which each relation occurs by taking
the reciprocal of the time (seconds) required for the blue colour to appear for each
of solutions.
2. Calculate initial normality of the hydrogen peroxide for each solution and its
logarithm. Remember the total volume of the solution is 250cm3
Week 13 and 14: Thorough Revision and Tutorial
 Objectives:
1. To fully equip the students for the examination
2. To get the student familiar with the experiment
3. To examine different technical questions.
4. To build more confidence in the mind of the students
Week 15
Topic: Examination
Objectives:
To examine the students on some selected practical that have been covered during the
semester.
NOTE: Download your practical Manual on the Intranet Site (Landmark University base)
The Practical Manual has been uploaded on the E-learning platform on the intranet site of the
University.
Recommended Readings:
-
Quantitative Chemical Analytical Chemistry by Vogel
Physical Chemistry by K.K. Sharma Sharma
Physical Chemistry by Thomas Engel
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