Engineering
Chemistry I
EG 1105 SH
Total: 6 hour /week
Year:
I Lecture: 3
hours/week
Semester:
I Tutorial:
1 hours/week
Practical: hours/week
Lab: 2 hours/week Course Description:
This subject consists of three units related to general
chemistry, language of chemistry, and system of classification necessary to
develop background in chemistry that supports for the understanding and
practicing related engineering works.
Course
Objectives:
After the completion of this subject, students will be able
to explain the basic concepts related to the followings and apply them in the
field of related engineering works:
1. General
chemistry
2. Language
of chemistry 3. System of
classification
Course
Content:
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Unit 1:
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Language of chemistry: [4]
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1.1
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Symbol:
§ Definition
§ Significance
(qualitative and quantitative)
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1.2
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Formula:
§ Definition
§ Significance
(qualitative and quantitative)
§ Concept
of valency in terms of combining capacity with H2, O2,
and Cl2
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§
Variable valency (ref. Fe, Sn, Pb, Cu, Hg, S and N)
§ Radicals
(electro- positive and electro - negative)
§ Writing a formula
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1.3
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Chemical
equation: § Definition
§ Types
requisites
§ Significance
and limitation
§ Balancing
of chemical equation by hit and trial method and Partial equation method
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Unit 2:
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General chemistry:
2.1
Atom and molecule:
§
Definition
§
Dalton's atomic theory and modern position of
the theory
2.2
Atomic weight:
§
Definition
§ Determination
of atomic weight by Dulong and Petit's method and Related
numerical problems
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[8]
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2.3
Molecular Weight:
§ Definition
§ Avogadro's
hypothesis
§ Application
of Avogadro's hypotheses ( Mol. Wt=2×V.D., in the deduction of atomicity
of elementary gases H2 , Cl2,
O2, and N2)
§ Molecular
weight determination by Victor Meyer's method and Related
numerical problems
2.4
Equivalent weight:
§ Definition
§ Equivalent
weight of element, acid, base and salt
§ Equivalent
weight determination by hydrogen displacement method and oxide method.
§ Numerical
relation between equivalent weight, atomic weight and valency
§ Some
related problems of equivalent wt. (From Hydrogen displacement method and oxide
method)
2.5
Simple mole concept: § Mole
of an atom
§ Mole
of a molecule
§ Molar
volume and
§ Simple
calculation on mole concept
Unit 3:
System of classification: [33]
3.1 Acid,
Base and Salt:
§ Arrhenius
concept of acid and base
§ Lowry
and Bronsted concept of acid and base
§ Conjugate
acid and base
§ Amphoteric
nature of water
§ Lewis
concept of acid and base § Properties of acid
and base.
§ Definition
of Salt
§ Types
of salt (normal, acidic and basic)
§ Concept
of hydrogen ion concentration, pH value and pH Scale § Buffer solution.
3.2
Volumetric analysis:
§ Definition
of titration (acidimetry and alkalimetry),
§ Indicator
§ End-point
(neutralization point)
§ Standard
solution (primary and secondary standard solution), Normal, Decinormal, Molar,
Molal solution
§ Requisites
of primary standard substance
§ Volumetric
equation,
§ Express
the strength of solution Normality, Molarity,
Molality, gram per litre and percentage and related numerical problems
3.3
Periodic table:
§ Mendeleef's
periodic law
§ Mendeleef's
periodic table
§ Characteristics
of groups and periods in the table
§ Advantages
and anomalies of the periodic table
§ Modern
periodic law 3.4 Electronic theory valency:
§ Assumptions
§ Types
§ Electrovalency
eg. NaCl, MgO, CaS
§ Covalency
eg. H2, O2, N2, CH4, H2O,
NH3, C2H2
§ Coordinate
co-valency eg.H2O2, SO2, O3, SO3)
§ Electronic
dot structure of some compounds eg.H2SO4, CaCO3,
K2SO3
3.5
Electrolysis:
§ Definition
of electrolyte, non-electrolyte and electrolysis
§ Faraday
laws of electrolysis,
§ Application
of electrolysis (electroplating and electro refining)
§ Electrolysis
of acidulated water
3.6 Oxidation
and reduction: § Classical
definition
§ Electronic
interpretation
§ Oxidizing
agent: Definition and eg O2, O3, oxyacids, halogens, K2Cr2O7,
KMnO4
§ Reducing
agent: Definition and eg. H2, H2S with some
examples,
§ auto-oxidation
eg.H2O2, HNO2, SO2
§ Idea
of oxidation number
§ Balancing
chemical equation by oxidation number method
3.7
Atomic structure:
§ Subatomic
particles (electron, proton and neutron)
§ Classical
α - rays scattering experiment
§ Rutherford's
atomic model and its drawbacks
§ Bohr's
atomic model (postulates only)
§ Composition
of nucleus
§ Mass
number and atomic number
§ Isotopes
and isobar
§ Arrangement
of electron (Bohr - Bury Scheme)
§ Concept
of shell and sub shell,
§ Electronic
Configuration and atomic structure of Some elements (Atomic no. 1 to 30) § Hund's
rule
§ General
idea of quantum number and Pauli's exclusion principle
3.8
Corrosion:
§ Definition
§ Types
§ Direct
and indirect method and prevention against corrosion
3.9
Activity and electrochemical
series:
§ Definition
§ Action
of water, acid and oxygen on metals.
Engineering Chemistry Practical I [30]
1.
Simple Glass Working [6]
a. to
cut the glass tube into three equal parts and round up their shape edges
b. to
bore a hole through a cork
c. to
bend the glass tubing into acute, obtuse and right angle
d. to
draw a jet and capillary tube
e. to
fit up a wash bottle
2.
To separate sand and copper sulphate crystals in
pure and dry state from the mixture of
sand
and copper sulphate [2]
3.
To separate sand and calcium carbonate in pure
and dry state from the mixture of sand and calcium carbonate
[2]
4.
To prepare pure water from supplied impure water
by distillation and o test the purity of the sample prepared
[2] 5. To neutralize dilute sulphuric acid with
sodium carbonate solution, and to recover crystals
of
sodium sulphate [2]
6.
To obtain pure and dry precipitate of barium
sulphate by treating excess of dilute
sulphuric
acid with barium chloride solution [2]
7.
To investigate the composition of water by
electrolysis by using Hofmann's apparatus
[2]
8.
To determine the equivalent weight of reactive
metal by hydrogen displacement method. [2]
9.
To determine the pH of different unknown
solution and using pH paper and universal
indicator
[2]
10.
To prepare primary standard solution of sodium
carbonate and to use it to standardize an
approximate
decinormal acid solution [2]
11.
To standardize given unknown acid (Approx N/10)
solution by preparing standard alkali
solution.
(Expression of strength in different ways) [2]
12.
To standardize given unknown alkali
(approximately N/10) solution with the help of by preparing standard acid
solution. (Expression of strength in different ways) [2]
13.
To carry out conductivity experiments on solids
and liquids (CuSO4, Zn, Mg, Al, Fe,
CCl4,
C6H6, C2H5OH) [2]
Text books:
1.
A Text book of Chemistry, Jha and Guglani
2.
Foundations of Chemistry, Vol. 1, M.K. Sthpit
and R.R. Pradhananga
Reference books:
1.
Fundamentals of Chemistry, K.R. Palak
2.
Inorganic Chemistry, Bahl and Tuli
3.
A Text book of Engineering Chemistry, R.S.
Sharma
4.
A Textbook of Inorganic Chemistry, L.M. Mitra
5.
Elementary practical chemistry, M.K Sthapit
6.
Engineering Chemistry, M.L. Sharma, K. M.
Shrestha, PN, Choudhary
7.
A Textbook of Engineering Chemistry, Prakash
Poudel
Other learning materials:
1. Other
references to be selected by the related lecturer(s) from among the texts
available in the market that meet the content needs of this subject
2. Note:
The related institute may develop its own textbook and approve from
the related authority so as to have a prescribed textbook of this subject.
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