Identification
Subject
(code, title,
credits)
Department
Program
Term
Instructor
E-mail:
Phone:
Physical CHEMISTRY (3 credits)
Chemical Engineering
Undergraduate
SPRING 2016
Dr. Jestin Mandumpal
jmandumpal@khazar.org or dejesman@gmail.com
+994 514142095
Prerequisites
Language
Compulsory/Elective
Required textbooks
and course materials
Course website
Course outline
Chemistry 2 & Calculus 1
English
Compulsory
Core textbooks: Physical Chemistry, Gilbert Castellan (1983) Third Eds.
Course objectives
This course is a prerequisite for “Chemical Engineering  courses studied
further.
General objective of the course
To meet curriculum requirements of the School of Engineering and Applied
Sciences (SEAS)
Specific objectives of the course
-To support student academically, to improve their chances of realizing their
potential.
-To encourage students participation and interaction as well as fostering
atmosphere of tolerance and respect.
-To develop understanding the fundamentals of chemistry.
-To build background for the students further studying Chemical
Engineering 
By the end of the course the students should be able
-To know and apply main laws of Thermodynamics & Solutions.
-To know properties of Thermodynamic variables & Chemical Equilibrium
-To derive Thermodynamic equations.
-To learn problem solving strategies
x
Lecture
x
Group discussion
Experimental exercise
x
Assignments
x
Simulation
x
Course paper
Others
Methods
Date/deadlines
Percentage (%)
April, 2016
30
Midterm Exam
10 + 10
Assignment and
quizzes
10
Presentation/Group
Discussion
June, 2016
40
Final Exam
100
Total
Learning outcomes
Teaching methods
Evaluation
This course is based on traditional face-to-face classes
Fundamental concepts in chemistry, State of Matter and Thermodynamics,
Spontaneity and Equilibrium, Solutions, Condensed Matter
Policy
Attendance
The students are required to attend all classes as a part of their studies and
those having legitimate reasons for absence (illness, family bereavement, etc.)
are required to inform the instructor.
Tardiness / other disruptions.
If a student is late to the class for more than 10 (ten) minutes, (s)he is not
allowed to enter and disturb the class. However, this student is able to enter
the second double hours without delaying.
Exams
In order to be excused from the exam, the student must contact the dean and
the instructor before the exam. Excuse will not be granted for social activities
such as trips, cruises and sporting events (unless you are participating). The
exams will all be cumulative. Most of the questions on each exam will be
taken from the chapters covered since the last exam.
But some will come from the earlier chapters. In general the coverage will
reflect the amount of the time spend in class on the different chapters.
Withdrawal (pass / fail)
This course strictly follows grading policy of the School of Engineering and
Applied Sciences. Thus, a student is normally expected to achieve a mark of
at least 60% to pass. In this case of failure, he/she will be referred or required
to repeat the course the following term or year.
Cheating / plagiarism
Cheating or other plagiarism during midterm and final examinations will lead
to paper cancellation. In case, the student will automatically get 0 (zero),
without any considerations.
Professional behaviour guidelines
The student shall behave in the way to create favorable academic and
professional environment during the class hours. Unauthorized discussions
and unethical behavior are strictly prohibited.
For successful completion of the course, the students shall take an active part
during the class time, raising questions and involving others to discussions.
Learning and Teaching Methods
This course considers active learning process rather than passive one.
Week
Topic
1
1
2
3
2
3
Tentative Schedule
Topics
Some Fundamental Chemical concepts (1-8)
i.
Introduction(1)
ii.
The kinds of matter (1)
iii.
The kinds of substances (1)
iv.
Atomic and Molar Masses (2)
v.
Symbols and Formulae (3)
vi.
The mole (4)
vii.
Chemical equations (4)
viii. The international system of Units, SI
(6)
Empirical Properties of Gases (9-32)
i.
Boyles’ law and Charles law (9)
ii.
Molar mass of a gas. Avogadro’s law;
The ideal gas law (11)
iii.
The equation of state; Extensive and
Intensive properties (14)
iv.
The properties of the ideal gas (15)
v.
Determination of the molar masses of
gases and of volatile substances (17)
vi.
Mixtures; Composition variables (18)
vii.
Equation of state for a gas mixture:
Dalton’s law (19)
viii. The partial pressure concept (20)
ix.
The barometric distribution law (22)
iii.
iv.
v.
vi.
vii.
viii.
ix.
4
[1]
[1]
Real gases (33 – 50)
i.
ii.
4
Textbook/Assignments
Deviations from ideal behavior (33)
Modifying the ideal gas equation. The
van der Waal’s equation (34)
Implications of Van der Waal’s
equations (36)
The isotherms of real gas (40)
Continuity of states (41)
The isotherms of the van der Waals
equation(42)
The critical state (43)
The law of corresponding states(45)
Other equations of state (46)
[1]
The Structure of Gases (51-84)
i.
ii.
iii.
iv.
v.
vi.
vii.
Introduction (51)
Kinetic theory of Gases (51)
Calculation of the pressure of gas(52)
Dalton’s law of partial pressures (57)
Distributions
and
Distribution
functions (57)
The Maxwell distribution (58)
Calculation of average values using
[1]
viii.
ix.
x.
5
5
Maxwell distribution(68)
Maxwell distribution as energy
distribution (69)
Equipartition
of
energy
and
Quantisation (71-74)
The Maxwell_Boltzmann distribution
law(80-82)
Some properties of liquids & solids ( 85 -92)
i.
ii.
Condensed Phases (85)
Coefficients of thermal expansion and
compressibility (86)
iii.
Heats of fusion, thermal expansion, &
sublimation (88)
iv.
Vapour Pressure ( 88)
v.
Other properties of liquids (90)
Review of structural differences between solids,
liquids and gases (90)
6
6
The laws of thermodynamics: Generalities and the
zeroth law
i.
ii.
iii.
iv.
v.
7
7
v.
vi.
vii.
viii.
ix.
7
The first law of thermodynamics
Conversion of energy from one form
to the other
The second law of thermodynamics
The zeroth law of thermodynamics
Thermometry
[1]
Energy and the first law of thermodynamics
i.
ii.
iii.
iv.
8
[1]
x.
xi.
xii.
xiii.
xiv.
Work and heat
Expansion work
Work of compression
Maximum and Minimum quantities of
work
Reversible and irreversible
tranformations
First law of thermodynamics
Properties of energy
Change in energy and change in
properties in system
Changes in state at constant volume
Joule-Thomson’s experiment
Adiabatic changes in state
First law of thermodynamics and
chemical reactions
The formation reaction
Conventional values of molar
[1]
[1]
enthalpies
xv.
The determination of heat of
formation
xvi. Sequence of reactions: Hess’s law
xvii. Heats of solution and dilution
xviii. Heats of reaction at constant volume
xix. Dependence of heat of reaction on
temperature
xx.
Bond enthalpies
xxi. Calorimetric measurements
Midterm April 2016
9
8
Introduction to the second law of
thermodynamics
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
x.
xi.
xii.
10
9
Carnot cycle
The second law of thermodynamics
Characteristics of a reversible cycle
A perpetual motion of a second kind
The efficiency of heat engines
Another impossible engine
The thermodynamic temperature scale
Carnot cycle with ideal gas
Carnot refrigerator
The heat pump
Definition of entropy
The Clausius inequality
[1]
Entropy and the third law of
thermodynamics
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
x.
Properties of entropy
Conditions of thermal and mechanical
stability of the system
Change of entropy & change in state
variables
Entropy as a function of temperature
and pressure
Entropy as a function of temperarture
and volume
Entropy change in ideal gas
The third law of thermodynamics
Entropy and probability
Energy of distribution
Entropy of mixing
[1]
11
10
Spontaneity and Equilibrium (203-220)
The general conditions of equilibrium
and for spontaneity (203)
ii.
Conditions for equilibrium and
spontaneity under constraints (204)
iii.
Driving forces for natural changes
(208)
iv.
The fundamental equations of
thermodynamics (208)
v.
The thermodynamic equation of
state(210)
vi.
The properties of A (212)
vii.
The properties of G (213)
viii. The Gibbs energy of real gases (215)
ix.
Temperature dependence of Gibbs
energy (216)
Systems of variable composition; Chemical
Equilibrium(221−258)
i.
The fundamental equation (221)
ii.
The properties of μ (222)
iii.
The Gibbs energy of a mixture (223)
iv.
The Chemical potential of a pure
ideal gas (224)
v.
Chemical potential of an ideal gas in a
mixture of ideal gases (224)
vi.
Gibbs energy and entropy of mixing
(226)
vii.
Chemical equilibrium in a mixture
(229)
viii. The general behavior of Gas function
of ξ (230)
ix.
Chemical equilibrium in a mixture of
ideal gases (232)
x.
The equilibrium constants (234)
xi.
Standard Gibbs energies of formation
(235)
xii.
The temperature dependence of the
equilibrium constant (238)
xiii. The equilibrium between ideal gas and
pure condensed phases (240)
xiv. Le Chatelier principle (242)
xv.
Equilibrium
constants
from
Calorimetric measurements (244)
xvi. Chemical reactions and entropy of the
universe (245)
xvii. Coupled reactions (246)
xviii. Dependence of other thermodynamic
constants upon composition(246)
xix. Partial molar quantities and additivity
rules (247)
xx.
Gibbs Duhem equation (249)
xxi. Partial molar quantities in mixtures of
ideal gases (250)
i.
12
13
11
11
[1]
[1]
[1]
xxii.
14
12
15
Differential heat of solution(251)
Phase equilibrium in simple systems : The
Phase rule (259-276 )
i.
The equilibrium condition (259)
ii.
Stability of the Phases of a pure
substance (259)
iii.
Pressure dependence of μ versus T
curves (261)
iv.
The Clapeyron equation (262)
v.
The Phase diagram (266)
vi.
The integration of Clapeyron
equation (268)
vii.
Effect of pressure on vapour pressure
(270)
viii. The phase rule(271)
ix.
The problem of components(276)
[1]
Review (8-12)
June 2016
Final exam :: topics 8-12
This syllabus is a guide for the course and any modifications to it will be announced in advance.