Identification
Prerequisites
Language
Compulsory/Elective
Required textbooks
and course materials
Course website
Course outline
Course objectives
Learning outcomes
Teaching methods
Subject
(code, title,
credits)
Department
Program
(undergraduate,
graduate)
Term
Instructor
E-mail:
Phone:
Physical CHEMISTRY (3 credits)
Chemical Engineering
Undergraduate
FALL 2015
Dr. Jestin Mandumpal
jmandumpal@khazar.org or dejesman@gmail.com
+994 514142095
This course is a prerequisite for the Chemical Engineering course studied
further
English
compulsory
Core textbooks
1. Physical Chemistry, Gilbert Castellan
This course is based on traditional face-to-face classes
Alcohols, Ethers and Phenols/ Aldehydes and Ketones/Carboxylic acids &
their derivatives/ Amines/Carbohydrates/Amino acids, Peptides, and
Proteins/Lipids/Nucleic acids
This course is a prerequisite for the Course Biochemistry  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 the Thermodynamic equations.
-To solve problems related to Thermodynamics
Lecture
Group discussion
Experimental exercise
Case analysis
Simulation
Course paper
Others
x
x
x
Evaluation
Policy
Methods
Date/deadlines
Percentage (%)
November, 2015
30
Midterm Exam
20
Assignment and
quizzes
10
Presentation/Group
Discussion
February, 2016
40
Final Exam
100
Total
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
Tentative Schedule
Topics
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
2
2
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
3
[1]
[1]
Real gases (33 – 50)
3
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
4
Some Fundamental Chemical concepts
(1-8)
Introduction(1)
The kinds of matter (1)
The kinds of substances (1)
Atomic and Molar Masses (2)
Symbols and Formulae (3)
The mole (4)
Chemical equations (4)
The international system of Units, SI (6)
Empirical Properties of Gases (9-32)
Boyles’ law and Charles law (9)
Molar mass of a gas. Avogadro’s law;
The ideal gas law (11)
The equation of state; Extensive and
Intensive properties (14)
The properties of the ideal gas (15)
Determination of the molar masses of
gases and of volatile substances (17)
Mixtures; Composition variables (18)
Equation of state for a gas mixture:
Dalton’s law (19)
The partial pressure concept (20)
The barometric distribution law (22)
Textbook/Assignment
s
4
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.
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)
[1]
vii.
5
5
Calculation of average values using
Maxwell distribution(68)
viii. Maxwell
distribution
as
energy
distribution (69)
ix.
Equipartition
of
energy
and
Quantisation (71-74)
x.
The Maxwell_Boltzmann distribution
law(80-82)
Some properties of liquids & solids ( 85
-92)
i.
ii.
iii.
iv.
v.
vi.
6
6
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
7
7
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
Condensed Phases (85)
Coefficients of thermal expansion and
compressibility (86)
Heats of fusion, thermal expansion, &
sublimation (88)
Vapour Pressure ( 88)
Other properties of liquids (90)
Review of structural differences
between solids, liquids and gases (90)
Spontaneity and Equilibrium (203220)
The general conditions of equilibrium
and for spontaneity (203)
Conditions for equilibrium and
spontaneity under constraints (204)
Driving forces for natural changes (208)
The fundamental equations of
thermodynamics (208)
The thermodynamic equation of
state(210)
The properties of A (212)
The properties of G (213)
The Gibbs energy of real gases (215)
Temperature dependence of Gibbs
energy (216)
Systems of variable composition;
Chemical Equilibrium(221−258)
The fundamental equation (221)
The properties of μ (222)
The Gibbs energy of a mixture (223)
The Chemical potential of a pure ideal
gas (224)
Chemical potential of an ideal gas in a
mixture of ideal gases (224)
Gibbs energy and entropy of mixing
(226)
Chemical equilibrium in a mixture (229)
The general behavior of Gas function of
ξ (230)
Chemical equilibrium in a mixture of
ideal gases (232)
[1]
[1]
[1]
8
9
7
x.
xi.
The equilibrium constants (234)
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)
xxii. Differential heat of solution(251)
Midterm exam :: topics 1 − 7
8
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
10
9
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
ix.
[1]
Phase equilibrium in simple
systems : The Phase rule (259276 )
The equilibrium condition (259)
Stability of the Phases of a pure
substance (259)
Pressure dependence of μ versus T
curves (261)
The Clapeyron equation (262)
The Phase diagram (266)
The integration of Clapeyron equation
(268)
Effect of pressure on vapour pressure
(270)
The phase rule(271)
The problem of components(276)
[1]
Solutions (277-318)
Kinds of solutions (277)
Definition of the ideal solution (278)
Analytical form of the chemical
potential in ideal liquid solutions(280)
Chemical potential of the solute in a
binary ideal solution; Application of
Gibbs-Duhem equation(280)
Colligative properties (281)
The freezing point of Depression (282)
Solubility (285)
Elevation of boiling point(287)
Osmotic pressure(288)
[1]
11
9
12
10
x.
General characteristics of ideal
solutions(295)
xi.
The chemical potential in Ideal
solutions(296)
xii.
Binary solutions(297)
xiii. The lever rule(299)
xiv. Changes in state as the pressure is
reduced isothermally (300)
xv.
Temperature-Composition
diagrams(301)
xvi. Change in state with increase in
pressure(302)
xvii. Fractional distillation(302)
xviii. Azeotropes (305)
xix. The ideal dilute solution(307)
xx.
The chemical potentials in the ideal
dilute solutions(309)
xxi. Henry’s law and solubility of
gases(311)
xxii. Distribution of a solute between two
solvents(313)
xxiii. Chemical equilibrium in the ideal
solutions(313)
[1]
Equilibria between condensed phases
(319-344)
[1]
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
13
10
ix.
[1]
xiii.
xiv.
xv.
Gas-solid equilibria; vapour pressure of
salt hydrates(336)
Systems of three components(337)
Liquid-liquid equilibria(338)
Solubility of salts; common ion
effect(339)
Double salt formation(340)
The method of wet residues(342)
Salting out (346)
[1]
i.
Equilibria in non ideal systems (347370)
The concept of activity (347)
x.
xi.
xii.
14
Liquid - Liquid equilibria (319)
Distillation of partially miscible and
immiscible liquids (322)
Solid-Liquid Equilibria The simple
Eutectic diagram(324)
Freezing point diagram with compound
formation(329)
Compounds having incongruent melting
points(330)
Miscibility in the solid state(332)
Freezing point elevation(333)
Partial miscibility in the solid state(334)
11
ii.
iii.
iv.
v.
viii.
The rational system of activities (348)
Colligative properties (350)
The practical system (351)
Activities and reaction Equilibrium
(353)
Activities in Electrolytic solutions (354)
The Debye Huckel theory of the
structure of dilute ionic solutions (358)
Equilibria in ionic solutions (365)
i.
Review of the topics ( 5-9)
vi.
vii.
15
February
2016
Final exam :: topics 5-9
This syllabus is a guide for the course and any modifications to it will be announced in advance.