ACADEMIC YEAR 2011-2012
[Paper code: 51005]
Mrs. V. Lakshmi Prasanna, Assistant Professor
Mr. K. Phani Raja, Assistant Professor
1
CONTENTS
Topic
Page No.
1.
2.
3.
4.
5.
Academic calendar
3
Course objective
4
Syllabus
5
Lecture plan
8 to 10
Learning objectives, Essay questions, Objective questions
[Multiple choice & Fill in Blanks]
6. Unit I
11o 14
7. Unit II
14to 17
8. Unit III
18 to 20
9. Unit IV
21 to 23
10. Unit V
23 to 26
11. Unit VI
26 to 29
12. Unit VII
29 to 32
13. Unit VIII
32 to 35
2
ACADEMIC CALENDER
S.NO
1
2
3
EVENT
DATE & DAY
Orientation Programme
24.08.2011 (WED)
1st Spell of Instructions for covering Units 1 25.08.2011 (THUR) to
&2
29.10.2011(SAT)
1st Mid Term Examinations
31.10.2011 (MON) to
Timings: 10.00 am To 12.00 Noon (Forenoon
03.11.2011 (THU)
Duration
01 Day
10 Weeks
04 Days
Session) 2.00 pm To 4.00 pm (Afternoon Session )
4
5
2nd Spell of Instructions for covering Units 04.11.2011 (FRI) to
3, 4 & 5
14.01.2012 (SAT)
nd
2 Mid Term Examinations
18.01.2012 (WED) to
Timings: 10.00 am To 12.00 Noon (Forenoon
21.01.2012 (SAT)
10 Weeks
04 Days
Session) 2.00 pm To 4.00 pm (Afternoon Session )
6
7
3rd Spell of Instructions for covering Units 6, 23.01.2012 (MON) to
7&8
27.03.2012 (TUE)
3rd Mid Term Examinations
14-11-2011 (MON) to
Timings: 10.00 am To 12.00 Noon (Forenoon
26-11-2011(SAT)
10 Weeks
04 Days
Session) 2.00 pm To 4.00 pm (Afternoon Session )
8
9
10
11
Preparation and Practical Examinations
02.04.2012 (MON) to
14.04.2012 (SAT)
End Semester Examinations (Regular)
16.04.2012 (MON) to
28.04.2012 (SAT)
Summer Vacation
30.04.2012 (MON) to
30.06.2012 (SAT)
Commencement of Class work for II Year - I 02.07.2012 (MON)
Semester for the academic year 2012-2013
3
02 Weeks
02 Weeks
2 Months
-----
COURSE OBJECTIVE
Chemistry is the study of matter, its properties, and the changes that it may undergo
and how these properties and changes are affected by its composition. It is important for
engineers to have knowledge chemistry, since they can expect to find problems in fields as
diverse as the design and development of new materials, quality control and environmental
engineering that are basically chemical in nature. The standing and firmness of a structure is
decided by the strength of foundation laid, although it is never expressed to the external
world. Similarly the applied and engineering sciences derive strength from basic sciences and
their growth is decided by inputs given by the basic sciences.
Chemistry is the back bone in designing and understanding the nature of various
engineering materials. Many advances in engineering either produce a new chemical demand
as in the case of polymers or wait upon chemical developments for their application as in the
case of implants and alloys. Currently , the electronics and computer engineers are waiting
for suitable bio-polymers and nano molecules for use in miniature super computers; the
electrical engineers are in search of proper conducting polymers; the mechanical engineers
are on look out for the micro fluids and civil engineers are looking for new materials that are
environment friendly , economical but long lasting.
Engineering chemistry is maze of topics of basic chemistry and applied chemistry.
This course is an attempt which is made to mix both the facets of the subject to reach proper
consequence and meet the demands of engineers. This course aims imparting intensive and
extensive knowledge of the subject, so that the student can understand the role of chemistry
in the field of engineering. This course is also aimed at developing analytical capabilities of
the students so that they characterize, transform and use the materials in engineering; apply
the knowledge gained in solving related engineering problems; to develop fascination
towards engineering chemistry and scientific reasoning in students.
4
ENGINEERING CHEMISTRY SYLLABUS
Branch: I B. Tech. (Common to all Branches)
UNIT-1: ELECTROCHEMISTRY AND BATTERIES
Concept of Electro Chemistry, Conductance-electrolyte in solution, Conductance-Specific,
Equivalent and Molar conductance, Ionic mobilities, Kohlrausch’s Law. Application of
conductance. EMF: Galvanic Cells, types of Electrodes. Reference Electrode (SCE,
Quinhydrone electrode), Ion Selective Electrodes(Glass Electrode) Nernest equation,
concentration Cells, Galvanic series, potentiometric titrations, numerical problems.
Batteries: Primary and Secondary cells,(lead-Acid cell, Ni-Cd cell, Lithium cells).
Applications of batteries, Fuel cells: Hydrogen-Oxygen fuel cells, Advantages of fuel cells.
UNIT –2: CORROSION AND ITS CORROSION CONTROL
Introduction, Causes and different types of corrosion and effects of corrosion, theories of
corrosion-Chemical, Electrochemical corrosion, corrosion reactions, factors affecting
corrosion-Nature of metal-galvanic series, over voltage, purity of metal, nature of oxide film,
nature of corrosion product. Nature of environment –effect of temperature, effect of pH ,
Humidity, effect of oxidant. Corrosion control methods – Cathodic protection, sacrificial
anode, impressed current cathode. Surface coatings-methods of application on metals-hot
dipping, galvanizing, tinning, cladding, electroplating-organic surface coatings- paints
constituents and functions.
UNIT –3: POLYMERS
Types of Polymerization, Mechanism (Chain growth & Step growth). Plastics: Thermoplastic
resins & Thermo set resins. Compounding &fabrication of plastics, preparation, properties,
engineering applications of: polyethylene, PVC, PS, Teflon, Bakelite, Nylon. Conducting
Polymers: Polyacetylene, polyaniline, conduction, doping, and applications. Liquid Crystal
5
polymers: Characteristics and uses Rubber-Natural rubber, vulcanization, Elastomer-Buna-S,
Butyl rubber, Thiokol rubbers, Fibers-polyester, fiber reinforced plastics (FRP), applications.
UNIT –4: WATER
Introduction, Hardness: Causes, expression of hardness-units-types of hardness, estimation of
temporary& permanent hardness of water, numerical problems. Boiler troubles-Scale &
sludge formation, caustic enbsittlement, corrosion, priming & foaming softening of water
(Internal & external treatment-Lime soda, Zeolite, Ion exchange process and Numerical
problems) Reverse osmosis, electro dialysis.
UNIT-5: SURFACE CHEMISTRY
Solid surfaces, types of adsorption, Langmuir adsorption isotherm, BET adsorption equation.
Calculation of surface area of solid &application adsorption, classification of colloids,
Electrical & Optical properties micelles, applications of colloids in industry. Nano materials:
Introduction, preparation and applications of nano materials.
UNIT-6: ENERGY SOURCES
Fuels, classification-conventional fuels (solid, liquid, gaseous). Solid fuels-coal-analysisproximate and ultimate analysis and their significance. Liquid fuels-primary-petroleumrefining of petroleum-cracking knocking synthetic petrol-Bergius and Fiscner Tropsech’s
process; Gaseous fuels-natural gas, analysis of flue gas by Orsat’s method Combustionproblems, Calorific value of fuel-HCV, LCV, determination of calorific value by Junker’s
gas calorie meter.
UNIT-7: PHASE RULE
Definitions-phase, component, degree of freedom, phase rule equitation. Phase diagrams-one
component system: water system. Two component system lead-silver system, heat treatment
based on iron-carbon phase diagram, hardening, annealing.
6
UNIT-8: MATERIAL CHEMISTRY
Cement: composition of Portland cement, manufacture of port land cement & hardening of
cement (reactions). Lubricants: Criteria of a good lubricant, mechanism, properties of
lubricants: Cloud point, pour point, flash & fire point, Viscosity. Refractoriess:
Classification, Characteristics of a good refractory. Insulators & conductors: classification of
insulators, characteristics of thermal & electrical insulators and applications of Super
conductors (Nb-Sn alloy, YBa2Cu3O7-8), applications.
Reference Text Books:
T1: Engineering Chemistry by B. Siva Shanker, Mc. Graw Hill Publishing Company Ltd.,
New Delhi (2006).
T2: Engineering Chemistry by J. C. Kuriacase & J. Rajaram, Tata Mc. Graw Hills Co., New
Delhi (2004).
T3: Engineering Chemistry by P.C Jain & Monica Jain.
T4: Chemistry of Engineering materials by C. V. Agarwal, C.P Murthy and A. Naidu, B. S
Publications.
T5: Chemistry of Engineering Materials by R.P Mani and K.N. Murthi.
T6: Applied chemistry: A text book for Engineering & Technology Springer (2005).
T7: Text book of Engineering Chemistry – Shasi Chawla, Dhara, Rai Publications
T8 : Engineering chemistry R. Gopalan – Vikas Publishiers (2008).
7
LECTURE PLAN
S.No.
Name of the topic
No. of
Periods
Teaching
Resource
Methodology
Books
UNIT- I: ELECTROCHEMISTRY AND BATTERIES
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
Introduction to concept of Electro Chemistry
Conductance-Electrolyte in solution, ConductanceSpecific, Equivalent and molar conductance and
Ionic motilities
Kolrausch’s Law, Application of Conductance
EMF: Galvanic Cells, types of Electrodes
Reference Electrode
Saturated Calomel Electrode
Quinhydrone electrode
Ion Selective Electrodes-Glass Electrode
Nernest equation, Numerical problems
Concentration Cells, Galvanic series
Potentiometric titrations
Numerical problems
Introduction of Batteries, Primary and secondary
cells
Lead-Acid cell, Ni-Cd cell, Lithium cells,
applications of batteries
Fuel cells – Hydrogen – Oxygen fuel cells,
Advantages of fuel cells.
Total
1
1
Chalk & talk
Chalk & talk
T8
1
1
1
1
1
1
1
1
1
1
1
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
T1 , T6 ,T8
1
Chalk & talk
T1 , T6 ,T8
1
Chalk & talk
T1 , T6 ,T8
T1 , T6 ,T8
15
UNIT- II: CORROSION AND ITS CORROSION CONTROL
16
17
18
19
20
21
Corrosion and its corrosion control: Introduction,
causes and different types of corrosion and effects of
corrosion
Theories of corrosion – Chemical, Electrochemical
corrosion, corrosion reactions, factors affecting
corrosion
Nature of metal – galvanic series, over voltage,
purity of metal, nature of oxide film, nature of
corrosion product. Nature of environment-effect of
temperature, effect of pH, Humidity, effect of
oxidant
Corrosion control methods
Cathodic protection, sacrificial anode, impressed
current cathode
Surface coatings – methods of application on
metals- hot dipping, galvanizing, tinning
8
1
Chalk & talk
T1 , T4 ,T8
1
Chalk & talk
T1 ,T4 ,T8
1
Chalk & talk
T1 , T4 ,T8
1
1
Chalk & talk
Chalk & talk
T1 , T4 ,T8
T1 , T4 ,T8
1
Chalk & talk
T1 , T4 ,T8
22
Cladding, electro plating -Organic surface coatings
– paints constituents and functions.
Chalk & talk
T1 , T4 ,T8
1
1
1
1
1
1
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
1
Chalk & talk
T1 , T5 ,T8
1
1
Chalk & talk
Chalk & talk
T1 , T5 ,T8
T1 , T5 ,T8
1
1
1
12
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
1
Chalk & talk
T1 , T5 ,T8
1
Chalk & talk
T1 , T5 ,T8
1
1
Chalk & talk
Chalk & talk
T1 , T5 ,T8
T1 , T5 ,T8
1
1
1
1
8
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
T1 , T5 ,T8
1
Total
7
UNIT III : POLYMERS
23
24
25
26
27
28
29
30
31
32
33
34
Total
Introduction to polymers, types of polymerization
Mechanism of Chain growth
Mechanism of Step growth
Plastics: Thermoplastic resins & Thermo set resins
Compounding & fabrication of plastics
Preparation, properties, engineering applications of:
polyethylene, PVC, PS, Teflon, Bakelite, Nylon
Conducting Polymers: Poly acetylene, polyaniline,
conduction, doping, applications
Liquid Crystal polymers
Characteristics and uses Rubber –Natural rubber,
vulcanization
Elastomers – Buna-s, Butyl rubber, Thiokol rubbers
Fibers – polyester
Fiber reinforced plastics (FRP), applications
UNIT IV : WATER
35
36
37
38
39
40
41
42
Total
Water: Introduction, Hardness: Causes, expression
of hardness – units – types of hardness
Estimation of temporary & permanent hardness of
water
Numerical problems
Boiler troubles – Scale & sludge formation, caustic
enbsittlement, corrosion, priming & foaming
Softening of water Internal
External treatment-Lime soda
Zeolite
Ion exchange process and Numerical problems
Reverse osmosis, electro dialysis
UNIT V : SURFACE CHEMISTRY
43
44
45
46
47
48
49
Surface Chemistry: Solid surfaces, types of
adsorption
Longmuir adsorption isotherm
BET adsorption equation
Calculation of surface area of solid & application
adsorption
Classification of colloids
Electrical & optical properties micelles, applications
of colloids in industry
Nano materials: Introduction, preparation and
9
1
Chalk & talk
T1 , T8
1
1
1
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T8
T1 , T8
T1 , T8
1
1
Chalk & talk
Chalk & talk
T1 , T8
T1 , T8
1
Chalk & talk
T1 , T8
applications of nano materials
Total
7
UNIT VI : ENERGY SOURCES
50
51
52
53
54
55
56
57
58
Energy sources: fuels, classification – conventional
fuels (solid, liquid, gaseous)
Solid fuels – coal –analysis – proximate and
ultimate analysis and their significance
Liquid fuels – primary – petroleum
Refining of petroleum-cracking knocking
Synthetic petrol – Bergius and Fischer Tropsech’s
process
Gaseous fuels – natural gas, analysis of flue gas by
Orsat’s method
Combustion – problems
Calorific value of fuel – HCV, LCV
Determination of calorific value by Junker’s gas
calorie meter
Total
1
Chalk & talk
T1 , T2 ,T8
1
Chalk & talk
T1 , T2 ,T8
1
1
1
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T2 ,T8
T1 , T2 ,T8
T1 , T2 ,T8
1
Chalk & talk
T1 , T2 ,T8
1
1
1
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T2 ,T8
T1 , T2 ,T8
T1 , T2 ,T8
1
Chalk & talk
T1 , T8
1
1
1
1
1
6
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
Chalk & talk
T1 , T8
T1 , T8
T1 , T8
T1 , T8
T1 , T8
9
UNIT VII: PHASE RULE
59
60
61
62
63
64
Total
Phase rule: Definitions – phase, component, degree
of freedom
Phase rule equitation
Diagrams –one component system: water system
Two-component system lead- silver system
Treatment based on iron-carbon phase diagram
Hardening, annealing
UNIT VIII: MATERIAL CHEMISTRY
65
66
67
68
69
70
71
Introduction to Materials Chemistry, Cement:
composition of port land cement, manufacture of
port land Cement
Lubricants: Criteria of a good lubricant
Mechanism, properties of lubricants: Cloud point,
pour point, flash & fire point, Viscocity
Refractories: Classification, characteristics of a good
refractory
Insulators & conductors
Classification of insulators characteristics of thermal
& electrical insulators
Applications of superconductors (Nb-Sn alloy,
YBa2-Cu3O7-8), applications
Total
TOTAL NO. OF CLASSES
10
1
Chalk & talk
T1 , T3,T8
1
1
Chalk & talk
Chalk & talk
T1 , T3 ,T8
T1 ,T3 ,T8
1
Chalk & talk
T1 ,T3 ,T8
1
1
Chalk & talk
Chalk & talk
T1 ,T3 ,T8
T1 ,T3 ,T8
1
Chalk & talk
T1 ,T3 ,T8
7
71
LEARNING OBJECTIVES
UNIT-1: ELECTROCHEMISTRY AND BATTERIES: Concept of Electro Chemistry,
Conductance-Electrolyte in solution, Conductance-Specific, Equivalent and Molar
conductance, Ionic mobilities, Kohlrausch’s Law. Application of conductance. EMF:
Galvanic Cells, types of Electrodes. Referenc Electrode (SCE, Quinhydrone electrode), Ion
Selective Electrodes(Glass Electrode) Nernst equation, Concentration Cells, Galvanic series,
Potentiometric titrations, Numerical problems.
Batteries: Primary and Secondary cells, (lead-Acid cell, Ni-Cd cell, Lithium cells).
Applications of batteries, Fuel cells-Hydrogen-Oxygen fuel cells, Advantages of fuel cells.
LEARNING OBJECTIVES
 After completion of this unit the student should be able to:
1. Define the term conductor.
2. Explain the Metallic conductors and Electrolytic conductors.
3. Explain the terms:
 Specific conductance
 Equivalent conductance
 Molar conductance
4. Explain the applications of Kohlrausch’s law.
5. Draw the simple Voltaic(Galvanic)cell
6. Label the Anode and Cathode and their signs.
7. Mention the directions of ion and electron movement and the signs of the electrodes
8. Describe the appropriate electrode potentials.
9. Calculate the Standard cell potential, Eo cell generated by a voltaic cell.
10. Calculate the concentration of an ion by using the Nernst equation.
11. Describe the
 Lead storage battery
 The Dry cell
 The Ni-Cd cell
 Lithium cells
12. Explain the applications of
 Batteries
 Fuel cells
 Advantages of fuel cells.
13. Describe conductometric and potentiometric titrations
14. Describe the types of electrodes present
15. Describe the different types of electrodes.
16. Describe a galvanic series
11
Essay Questions
1. What is conductance of an electrolyte solution?
2. Explain specific, equivalent, and molar conductance?
3. Define Kolrausch’s law? Explain in detail EMF?
4. Explain with a neat diagram the function of Reference and Selective ion electrodes?
5. Explain Nernst equation?
6. What is a fuel cell and what are its advantages?
7. Write about potentiometer titrations?
8. A conductivity cell has two parallel electrodes of 1.25 sq cm area and 1.05 cm apart.
When filled with 0.1N solution of an electrolyte at 25oC, the resistance was found to
be 2,000 Ohms. Calculate the cell constant and electro equivalent conductivity?
9. Explain the primary and secondary cells?
10. The resistance of decinormal solution of a salt occupying a volume between two
platinum electrodes 1.80 cm apart and 5.4 cm2 in area was found to be 32 ohms.
Calculate the equivalent conductance of the solution?
11. A zinc road is placed in 0.1M-znso4 solutions at 298 K. Write the electrode reaction
and calculate the potential of the electrode. Zn = - 0.7 V?
12. Calculate the emf of the following cell?
Zn(s)/Zn+2 (0.1M) // Cu+2 (1.75 M) / (s) at 25oC
Multiple choice Questions
1. Units of specific conductance is?
(a) Ohm-1cm-1
[a]
(b) Ohm-1cm2mol-1
(c) cm-1
(d) Met-1
2. Units of molar conductance is?
(a ) cm-1
(b) ohm-1cm2mol-1
[b]
(c) ohm-1cm-1 (d) met-1
3. Which one of the following is an electrolyte?
(a) Benzene
(b) Chloroform
(c) Benzyl chloride
4. Which one of the following does not conduct electricity
12
[d]
(d) Sodium cyanide
[b]
(a) Molten sodium chloride (b) NaCl crystal (c) Solution of NaCl
(d) None of these
5. The ionization of a weak electrolyte increases, when the solution is diluted. The reaction
is given by:
[b]
(a) Nernst equation (b) Arhenius equation
(c) Oswald law
(d) Law of mass action
6. The degree of dissociation of acetic acid in aqueous solution of the acid is practically
unaffected
[c]
(a) By adding a pinch of NaCl
(b) By adding a drop of HCl
(c) By diluting water
(d) By raising the temperature
7. Conductivity of a solution is directly proportional
(a) Dilution
(b) No.of ions
[b]
(c) Current density
(d) Volume of the solution
8. Pure water does not conduct electricity because
(a) Neutral
(b) Low boiling
[a]
(c) Almost not ionized
(d) Decomposed easily
9. The specific conductance of an electrolyte solution on dilution
(a) Decreases
(b) Increases
(c) Remains unchanged
(d) First increases then decreases
10. The potential of standard hydrogen electrode is taken as
(a) 1 volt
(b) 0 volt
(c) 10 volts
[b]
(d) None of these
11. The electrode with lowest hydrogen over voltage is
(a) Zn
(b) Ni
(c) Hg
[a]
[a]
(d) Pt
12. Calomel is
[c]
(a) Mercuric sulfate (b) Mercurous sulfate (c) Mercurous chloride (d) Mercuric chloride
13. Aqueous solution of which one of the following does not conduct electricity
(a) AgNO3
(b) Acetic acid
(c) NaOH
[a]
(d) HCl
14. A galvanic cell converts
[b]
(a) Electrical Energy in to chemical energy
(b) Chemical energy into electrical energy
(c) Electrical energy into heat energy
(d) Chemical energy into heat energy
15. The relationship between specific conductivity and equivalent conductance is
(a)
 eq 
CX 100
k
 eq 
(b)
k .C
1,000
(c)
13
 eq 
[c]
CX 1,000
kX1,000
 eq 
k
C
(d)
Fill in the blanks
1. Graphite is a good conductor.
2. Specific conductance is expressed in S Cm-1 units.
3. The units of resistivity are Ohm cm.
4. The units of equivalent conductance is Ohm-1 cm2 eq-1.
5. The units of Molar conductivity is Ohm-1 cm2 mol-1.
6. Nernst equation for electrode reaction is E = Eo+ [2.303RT/nF] logC
7. The equivalent conductance increases on dilution.
8. The transport number of an anion is calculated by 1-n = V/u+v.
9. Fuel cells are the cells which do not store the energy.
10. A cell whose reaction is not reversible is called primary cell.
UNIT –2: CORROSION AND ITS COROSSION CONTROL: Introduction, causes and
different types of corrosion and effects of corrosion, theories of corrosion-Chemical,
Electrochemical corrosion, corrosion reactions, factors affecting corrosion-Nature of metalgalvanic series, over voltage, purity of metal, nature of oxide film, nature of corrosion
product. Nature of environment –effect of temperature, effect of pH , Humidity, effect of
oxidant. Corrosion control methods–Cathodic protection, sacrificial anode, impressed current
cathode. Surface coatings-methods of application on metals-hot dipping, galvanizing,
tinning, cladding, electroplating-Organic surface coatings- paints constituents and functions.
LEARNING OBJECTIVES

After completion of this unit the student should be able to:
1. List out the causes and different types of corrosion.
2. Distinguish between chemical and electrochemical corrosion.
3. Describe the factors affecting corrosion.
 Environment factors
 Effect of temperature
14
 Effect of pH
 Humidity
 Effect of Oxidant.
4. Explain the corrosion control methods.
5. Explain the surface coatings and methods of application on metals.
6. Explain the methods
 Electroplating
 Cladding
 Galvanizing
 Tinning & Hot dipping.
 Applying organic surface coatings on metals.
Essay Questions
1. Explain how corrosion control can be brought about by the following methods?
(a) Modifying the environment
(b) Cathodic protection (c) Sacrificial anode
2. Define corrosion and what is its theory explain with chemical reactions?
3. What is chemical and electro chemical corrosion?
4. What are the atmospheric factors affecting corrosion?
5. Explain the following?
(a) Electroplating (b) Galvanizing
(c) Tinning
(d) Metal cladding
6. Write down constituents and functions of paint?
7. Differentiate between Anodic coatings & cathodic coatings?
Multiple choice Questions
1. The rusting of iron is catalyzed by which one of the following:
(a) Fe
(b) O2
[b]
(d) H+
(c) Zn
2. Rusting of iron is
[a]
(a) Enhanced by wet air
(b) Prevented on coating with zinc
15
(c) Retarded in the presence of dissolved salts
(d) Prevented, if the article is connected with a wire of Mg.
3. Corrosion is as example of:
(a) Oxidation
[a]
(b) Reduction
(c) Electrolysis
(d) Erosion
4. For corrosion of iron to take place:
[b]
(a) Presence of moisture is sufficient
(b) Presence of both moisture and oxygen is essential
(c) Hydrogen is required
(d) A strong acid is necessary
5. When a buried pipeline is protected from corrosion by connecting to Mg block, it is
called:
[c]
(a) Impressed voltage protection
(b) Sacrificial cathodic protection
(c) Sacrificial anodic protection
(d) Any of these
6. Corrosion in essence is a process of
(a) Reduction
(b) Oxidation
[b]
(c) Electrolysis
(d) Extraction of metals
7. During wet corrosion:
[a]
(a) The anodic part undergoes oxidation
(b) The cathodic part undergoes oxidation
(c) The anodic part undergoes reduction
(d) Neither anodic nor cathodic part undergo any changes
8. Electrochemical corrosion can occur only if:
[a]
(a) Oxygen in present in contact with metal (b) Air is present in contact with metal
(b) Liquid medium is in contact with metal (d) None of the above are present
9. During galvanic corrosion, the more noble metal acts as:
(a) Anode (b) Cathode
(c) Anode as well as cathode
[a]
(d) Corroding metal
10. During corrosion of iron in aqueous solution:
[c]
(a)Corrosion occurs at cathode
(b) Rust/corrosion product is deposited at anode
(c) Corrosion occurs at anode and rust is also deposited at anode
(d) Corrosion occurs at anode and rust is deposited at cathode
11. During oxygen concentration type corrosion, the corrosion:
16
[b]
(a) Occurs at more-oxygenated part (b) Occurs at less-oxygenated part
(b) Is uniform throughout
(d) Occurs at the cathodic part
12. The process cementation with zinc power is known as:
(a) Galvanizing
(b) Zincing
(c) Sherardizing
[a]
(d) Tinning
13. The rate of corrosion of iron in atmosphere depends upon:
[a]
(a) The humidity of the atmosphere (b) The degree of pollution of the atmosphere
(c) The frequency of rain fall
(d) All of these factors
14. In an electrochemical corrosion:
[a]
(a) Anode undergoes oxidation
(b) Cathode undergoes oxidation
(c) Both undergoes oxidation
(d) None of the above
15. In waterline corrosion the maximum amount of corrosion takes place
[c]
(a) Along a line just above the level of the water meniscus
(b) Along a line at the level of the water meniscus
(c) Along a line just below the level of the water meniscus
(d) At the bottom of the vessel.
Fill in the blanks
1. An example of anodic corrosion inhibitor is chromate.
2. An example of cathodic coating is tinning.
3. Corrosion is a gradual decay of metal by the attack of environment.
4. Soil corrosion is pure electrochemical in character.
5. Drying oils are used as vehicles in paints.
6. Impurities in metal causes corrosion.
7. The rate of corrosion increases with decrease in pH.
8.
The type of corrosion which occurs along rain boundaries is called intergrannular
corrosion.
9. Sand blasting is used for removing oxide scales.
10. Cathodic coatings are obtained by coating a noble metal than the base metal.
17
UNIT–3: POLYMERS: Types of Polymerization, Mechanism (Chain growth &Step
growth).Plastics: Thermoplastic resins &Thermo set resins. Compounding & fabrication of
plastics, preparation, properties, engineering applications of polyethylene, PVC, PS, Teflon,
Bakelite, Nylon. Conducting Polymers: Poly acetylene, polyaniline, conduction, doping, and
applications. Liquid Crystal polymers: Characteristics and uses Rubber-Natural rubber,
vulcanization, Elastomer-Buna-S, Butyl rubber, Thiokol rubbers, Fibers-polyester, fiber
reinforced plastics (FRP), applications.
LEARNING OBJECTIVES

After completion of this unit the student should be able to:
1. Define the term Monomer and Polymer.
2. Describe the molecular structure of polymers.
3. Distinguish between Thermo plastic and Thermosetting plastic.
4. Give examples of Compounding and fabrication of plastics.
5. Explain the engineering applications of
 Poly ethylene
 PVC
 PS
 Teflon
 Bakelite
 Nylon
6. Characterize the uses of Rubber-Natural rubber vulcanization.
7. Describe the Elastomers-Buna-S, Butyl rubber, Thiokol rubbers.
8. Describe the mechanical characteristics of each type of fiber-reinforced composite.
Essay Questions
1. Write down different types of Polymerization and their mechanism?
18
2. Explain thermo plastics and thermosetting resins with examples?
3. Write down preparation, properties and applications of the following?
a) Polyethylene (b) PVC (c) Poly Styrene (d) Teflon (e) Bakelite & Nylon
4. Write down vulcanization of rubber and its advantage?
5. Write down properties and applications of Buna-S, Butyl rubber and Thiokol rubbers?
6. What is FRP and what are its applications?
7. Write down preparation properties and applications of Plastics?
8. What are the characteristics and uses of natural rubber?
Multiple choice Questions
1. Polymerization in which two or more chemically different monomers takes part is called:
(a) Homopolymers
(b) Copolymer
(c) Solids
(d) Fabrics
[b]
2. A thermoplastic is formed by the phenomenon of
[d]
(a) Chlorination
(b) Condensation polymerization
(c) Nitration
(d) Chain polymerization
3. Phenol-formaldehyde resin is commercially known as:
(a) PVC
(b) Elastomer
(c) Bakelite
[c]
(d) Nylon
4. Polymer commonly used for making fiber/cloth is:
(a) Rubber
(b) PVC
(c) Nylon
[c]
(d) Bakelite
5. Bakelite is prepared by the condensation of:
[b]
(a) Benzene and formaldehyde
(b) Phenol and formaldehyde
(c) Phenol and acetaldehyde
(d) Glycerol and phthalic acid
6. A high molecular weight material that can easily be molded in any desired shape is
(a) Graphite
(b) Resin
(c) Jelly
(d) Grease
[b]
7. A plastic which can be softened on heating and hardened on cooling is called
(a) Thermo-elastic
(b) Thermoplastic
(c) Thermosetting
(d) Thermite
8. Phenol-formaldehyde (bakelite) is an example of
(a) Thermo-elastic
(b) Thermoplastic
[c]
(c) Thermosetting
(d) Thermite
9. Natural rubber is basically a polymer of
(a) Propylene
[b]
[b]
(b) Isoprene
(c) Ethylene
19
(d) Propane
10. Which one of the following is an elastomer?
(a) PVC
(b) Bakelite
[d]
(c) Natural rubber
(d) Nylon
11. The raw material used for the manufacture of polyster are
[c]
(a) Vinyl chloride
(b) Urea + formaldehyde
(c) Glycol + terephthalic acid
(d) Phenol + formaldehyde
12. One of the important uses of bakelite is for making:
(a) Cables
(b) Electrical switches
(c) Cloth
[b]
(d) Hose pipe
13. The fiber obtained by the condensation of hexamethylenediamine and adipic acid is
(a) Dacron
(b) Nylon
(c) Rayon
(d) Terylene
14. Nylon is a
[b]
[c]
(a) A polythene derivative
(b) A polyester fiber
(c) A polyimide fiber
(d) None of these
15. Bakelite is a copolymer of
[b]
(a) Urea and formaldehyde
(b) Phenol and formaldehyde
(c) Urea and formaldehyde
(d) Urea and phenol
Fill in the blanks
1. Latex is the dispersion of isoprene molecules.
2. LDPE has less meltinor specific gravity than HDPE.
3. An example of thermosetting homo-polymer is nylon-6.
4. Stereo-specific polymers are obtained by coordination chain polymerization.
5. The plastic used for making optical lenses is PMMA.
6. Buna-S is a co-polymer of butadiene & styrene.
7. Caprolactum is a monomer of nylon-6.
8. Polyacetylene is a conducting polymer.
9. Nylon-6 is a polyamide.
10. Silicones contain alternate Si-O structure.
20
UNIT –4: WATER: Introduction, Hardness: Causes, expression of hardness-units-types of
hardness, estimation of temporary & permanent hardness of water, numerical problems.
Boiler troubles-Scale & sludge formation, caustic ensittlement, corrosion, priming &
foaming softening of water( Internal & external treatment-Lime soda, Zeolite, Ion exchange
process and Numerical problems) Reverse osmosis, electro dialysis.
LEARNING OBJECTIVES
 After completion of this unit the student should be able to:
1. Describe the concepts of Hardness.
2. Mention the types of Hardness.
3. Describe the causes of Hardness.
4. Estimate the Temporary and Permanent hardness of water .
5. Describe the Boiler- troubles –scale and sludge formation.
6. Explain the use the foaming softening of water-internal and external treatment.
7. Explain the use of the methods of
 Lime soda method
 Zeolite
 Ion exchange process.
8. Describe the Reverse Osmosis and electro dialysis.
Essay Questions
1. Define hardness .How to estimate hardness of water using EDTA solution?
2. Explain the following?
(a) Boiler corrosion
(b) Caustic embitterment (c) Scale & Sludge.
3. Explain softening of water using Lime and soda?
4. Define reverse osmosis?
5. Explain electro dialysis?
6. A water sample from Guntur contains the following parameters?
21
Ca(HCO3)2 = 50 ppm, Mg(HCO3)2, CaCl2 =20 ppm,
MgCl2 =80 ppm, CaSO4 =40 ppm.
Find out lime and soda requirement to treat 1 million litres of water (Purity of lime =
80%, Purity of soda = 90%).
7. Explain with a schematic diagram Zeolite process of water treatment?
8. Explain with a schematic diagram softening of water using ion exchange method?
Multiple choice Questions
1. Purest form of natural water is:
(a) River water
[c]
(b) Sea water
(c) Rain water
(d) Lake water
2. Hardness in water is caused by the presence of
(a) Sodium chloride (b) Sodium carbonate
[c]
(c) Calcium chloride (d) Potassium nitrate
3. Permanent hardness in water is caused by the presence of
(a) Calcium chloride
(b) Magnesium sulfate
[c]
(c) Both of them
(d) None of them
4. Temporary hardness in water can be removed by
(a) Filtration
(b) Boiling
[b]
(c) Sedimentation
(d) None of these
5. Scale formation in boilers causes:
(a) No. loss of heat
[b]
(b) Wastage of heat
(c) Increase in efficiency (d) None of these
6. Permanent hardness of water cannot be removed by
(a) Adding soda
(b) Distillation
(c) Boiling
[c]
(d) Adding lime-soda
7. Hard water may be softened by passing it through:
(a) Limestone
(b) Ion-exchange resins
(c) Calgon
[b]
(d) Rock salt
8. EDTA method of determining hardness of water can be used to determine:
(a) All types of hardness
(b) Temporary hardness only
(c) Permanent hardness only
(d) Alkaline hardness only
9. Water is hard when it contains:
[a]
[d]
(a) Acid solution
(b) Precipitate in suspension
(c) Dissolved sodium salts
(d) Dissolved Ca and Mg salts
10. Hard water may be softened by passing it through:
(a) Sodium silicate (Na2SiO3)
(b) Limestone
22
[c]
(c) Ion-exchange resins
(d) Sodiumhexametaphosphate
11. Pure water can be obtained by using
[b]
(a) Permutit process (b) Demineralization method
(c) Lime-soda process
(d) None
12. For maximum efficiency, disinfect ion of water by chlorination should be carried out
(b) At pH above 7
(a) Below break-point
(c) At pH of 5 to 6.5
(d) In cold
13. Coagulants help in the settling of
[d]
(a) Suspended impurities only
(b) Fine suspended matter only
(c) Colloidal particles only
(d) Both (b) & (c)
14. Alkalinity in water cannot be due to the presence of
(a) OH- only
(b) OH– and CO32- (c) Chlorine
[c]
(d) Lime
15. pH of neutral water is
(a) 0
(b) 14
[a]
[a]
(c) 7
(d) 10-7
Fill in the blanks
1. Hardness of water is due to the dissolved salts of Ca & Mg.
2. Hardness of water is expressed in equivalents of CaCO3.
3. Sodium aluminate is used as coagulant during purification of water.
4. Anion exchange resins are regenerated by using NaOH.
5. Best method for removing hardness of water is permuitit process.
6. Cationic exchange resin contains H+ mobile ions.
7. Temporary hardness of water can be removed by boiling.
8. Natrolite is an artificial zeolite.
9. The chemical structure of zeolite is Na2O Al2O3 x SiO2.
10.
Ion free water is known as de-ionized.
UNIT-5: SURFACE CHEMISTRY: Solid surfaces, types of adsorption, Longmuir
adsorption isotherm, BET adsorption equation Calculation of surface area of solid
&application adsorption, classification of colloids, Electrical & Optical properties micelles,
23
applications of colloids in industry. Nano materials: Introduction, preparation and
applications of nano materials.
LEARNING OBJECTIVES
 After completion of this unit the student should be able to:
1. Describe the solid surfaces and concept of adsorption.
2. Distinguish the Physical adsorption and Chemical adsorption.
3. Explain the Longmuir adsorption isotherm.
4. Explain the BET adsorption equip.
5. Calculate the surface area of solid.
6. Explain the usage the applications of adsorption.
7. Classify the colloids.
8. Describe the electrical and optical properties of colloids.
9. Explain the colloids applications in industry.
10. Describe the nano materials.
11. Explain the preparation of nano materials.
12. Explain the applications of nano materials.
Essay Questions
1. What is adsorption write types of adsorption?
2. Explain Longmuir adsorption isotherm, BET adsorption equation?
3. How to calculate the surface area of solid?
4. Explain classification of colloids?
5. Write applications of colloids in industry?
6. Explain preparation and applications of nano materials?
24
Multiple-choice Questions
1. The adsorption is
[a]
(a) Accumulation of a substance on the surface if the solid
(b) Removal of the substance on the surface of the solid
(c) Reaction of the substance with solid
(d) None of these
2. The adsorption isobar between
[b]
(a) Temperature and pressure
(b) Volume and pressure
(c) Temperature and volume
(d) Concentration and temperature
3. When temperature increases chemical adsorption is
(a) Increases
(b) Decreases
(c) First increases then decreases
(d) No effect
[a]
4. The example of physical adsorption is
[c]
(a) Adsorption of hydrogen on Ni metal
(b) Adsorption of hydrogen on charcoal
(c) Both
(d) None
5. A colloidal solution can be purified by the method of
(a) Dialysis
(b) Peptization
[c]
(c) Mechanical dispersion
(d) Oxidation
6. The difference between a lyophilic and lyophobic is in their;
[b]
(a) Particle size
(b) Behavior towards dispersion medium
(c) Filterability
(d) None of these
7. When a beam of light is passed through a colloidal solution
[b]
(a) Is reflected
(b) Is scattered
(c) Passes through undeviated
(d) Is completely absorbed
8. The process of preparation of a colloidal solution from a precipitate is called
(a) Coagulation
(b) Dissolution
(c) Electrophoresis
(d) Peptization
9. Starch dispersed in hot water is an example of:
(a) Emulsion
(b) Hydrophobic sol
(c) Lyphilic sol
10. Which one is an example of gel:
(a) Soap
(b) Cheese
(c) Milk
[d]
[c]
(d) Associated colloid.
[b]
(d) Fog.
11. Emulsion is a colloidal dispersion of
[b]
25
(a) A solid in a liquid
(b) A liquid in liquid
(c) A gas in a liquid
(d) A gas in a gas.
12. Colloidal particles are visible:
[a]
(a) To naked eyes nor under a microscope
(b) Suspended particles from crystalloids
(c) Colloidal particles from crystalloids
(d) Colloidal particles from gel.
13. Tyndall effect is due to:
(a) Absorption of light
[b]
(b) Scattering of light
(c) Both A & B
(d) None of above
14. Alum purifies muddy water by:
(a) Dialysis
(b) Absorption
[c]
(C) Coagulation
(d) Forming a true solution.
15. Optical property of a colloid is studied with the device;
(a) Ultra centrifuge
[c]
(b) Burtons tube (c) Ultra microscope (d) None of the above
Fill in the blanks
1. The absoption involves a very little activation energy.
2. The absorption of H2 or O2 on charcoal is physical.
3. Hydrogenation of oils make the phenomenon of adsorption.
4. Rosin is used as an indicator in argentometric titrations.
5. All gas masks contain activated as adsorbant.
6. The associated collides may be called as miscelles.
7. Soap is an example of associative collide.
8. The elongated micelle are called as cylindrical.
9. Solid-liquid dispersions are known as sols.
10. Alums purify turbid water by coagulation.
UNIT-6: ENERGY SOURCES: Fuels, classification-conventional fuels (solid, liquid,
gaseous).Solid fuels-coal-analysis-proximate and ultimate analysis and their significance.
Liquid fuels-primary-petroleum-refining of petroleum-cracking knocking synthetic petrolBergius and Fiscner Tropsech’s process; Gaseous fuels-natural gas, analysis of flue gas by
Orsat’s method Combustion-problems, Calorific value of fuel-HCV, LCV, determination of
calorific value by Junker’s gas caloriemeter.
26
LEARNING OBJECTIVES
 After completion of this unit the student should be able to:
1. Classify the conventional fuels-solid, liquid, gaseous.
2. Explain the coal analysis-proximate analysis and their significance.
3. Describe the refining of petroleum cracking.
4. Describe the knocking synthetic petrol (liquid fuels).
5. Explain the gaseous fuels-natural gas.
6. Explain the analysis of flue gas by Orsat’s method.
7. Describe the Calorific value of fuel by HCV, LCV.
8. Explain the determination of calorific value by Junker’s gas calorie meter.
Essay Questions
1. Write down Proximate and Ultimate analysis of coal?
2. What is calorific value? Explain solid, liquid, gaseous fuels?
3. Explain Bergius & Fischer Tropsch Process of manufacture of synthetic Petrol?
4. Write refining of petroleum?
5. Explain how to estimate HCV & LCV using Junker’s Gas Calorimeter?
6. How to analyse flue gases using Orsat apparatus?
Multiple Choice Questions
1. Which of the following fuels possesses the maximum calorific value?
[d]
(a) C=84%, H=6%, S=4%, and O=6%
(b) C=84%, H=12%, S=1%, O=1%
(c) C=90%, H=5%, S=2%, O=3%
(d) C=95%, H=2%, S=1%, and O=2%
2. A good fuel should possess:
[d]
(a) High ignition temperature
(b) Moderate ignition temperature
(c) High calorific value
(d) Both B & C
27
3. Which of the following statements is true.
[d]
(a) Coke possesses better strength than coal.
(b) Coke burns with a long flame.
(c) Coke burns with short flame
(d) Sulfur content of cokes is higher than that of coal from which it is obtained.
4. Which of the following fuel gases possess the highest calorific value.
(a) Water gas
(b) Coal gas
[c]
(c) Producer gas
(d) Natural gas
5. Petro chemicals can be used to prepare
(a) PVC plastics
[c]
(b) Polystyrene plastics (c) Terylene fibres
(d) None of the above
6. The maximum temperature reached, when the coal is completely burnt in the theoretical
amount of air is called
[c]
(a) Fusion temperature (b) Calorific intensity (c) Ignition temperature (d)None of above
7. In orat’s apparatus, KOH is used to absorb
(a) Oxygen
(b) Carbondioxide
[b]
(c) Carbonmonoxide
(d) Sulfurdioxide
8. Bomb calorimeter is used for determining the calorific value of
(a) Solid fuel
(b) Liquid fuel
[a]
(c) Gaseous fuel
(d) Both (a) & (b)
9. Bomb calorimeter is used to determine
[b]
(a) HCV at constant pressure
(b) LCV at constant pressure
(c) HCV at constant volume
(d) LCV at constant volume
10. Gas with least calorific value is
(a) Coal gas
(b) Water gas
[b]
(c) Producer gas
(d) Natural gas
11. Main constituent of natural gas is
(a) Carbonmonoxide
(b) Methane
[b]
(c) Hydrogen
(d) Ethane
12. A knocking sound is produced in the internal combustion engine, when the fuel
(a) Burns slowly
[b]
(b) Burns fast
(c) Contains some water (d) Is contaminated with lubricating oil.
13. Cracking is
[b]
(a) Somewhat similar to polymerization
(b) Conversion of long-chain hydrocarbons to shorter ones
(c) The production of unsaturated molecules from saturated ones
(d) Distillation of crude oil to obtain kerosene
28
14. Composing of producer gas is
[b]
(a) CO+Nitrogen (b) CO+Hydrogen (c) CO+Methane (d) Methane+Hydrogen
15. Petrol is a mixture mainly of
(a) Alkenes
(b) Alkanes
[d]
(c) Alkynes
(d) Aromatic hydrocarbons
Fill in the blanks
1. The calorific value of coke is generally higher than coal.
2. The compound with octane number 100 is iso-octane.
3. A good fuel should possess moderate ignition temperature.
4. Petroleum is the only primary liquid fuel in nature.
5. HCV calorific value includes latent heat of steam.
6. A good fuel should possess less moisture content.
7. The fuel which possess highest thermal efficiency is gaseous.
8. The calorific value of a gaseous fuel is determined by junkers gas caloriemeter.
9. One KCal/Kg is equal to 1.8 B.Th.U/lb.
10. Oxygen content decreases the calorific value.
UNIT-7: PHASE RULE: Definitions-phase, component, degree of freedom, phase rule
equitation. Phase diagrams-one component system: water system. Two component system
lead-silver system, heat treatment based on iron-carbon phase diagram, hardening, annealing.
LEARNING OBJECTIVES

After completion of this unit the student should be able to:
1. Define the terms:
 Phase
 Component
 Degree of freedom
 Phase Rule equation
29
2. Explain the phase diagram of one component system-water system.
3. Describe the two component system: Lead-Silver (Pb-Ag)system.
4. Describe the Heat treatment based on iron-carbon phase diagram.
5. Explain the process of Hardening and Annealing.
Essay Questions
1. Define Phase, Component, Degree and Freedom?
2. Explain one component phase diagram with suitable example?
3. Explain two-component phase diagram with suitable example?
4. What is hardening and annealing?
Multiple Choice Questions
1. For water system, the maximum number of degrees of freedom is
(a) 0
(b) 3
(c) 2
[b]
(d) 4
2. The pressure and temperature when all the three phases in water system can coexist in
equilibrium are respectively
[c]
(a) 4.2 mm, 0.00780C
(b) 5.2 mm, 0.00650C
(c) 4.58 mm, 0.00980C
(d) 5.48 mm, 0.00880C
3. In silver-lead system, the composition at the eutectic point is
(a) 2% Ag, 98% Pb
(b) 4% Pb, 96% Ag
(c) 2.6% Ag, 97.4% Pb
(d) 2.4% Pb, 97.6% Ag
4. FALSE about phase is
[d]
[b]
(a) A gaseous mixture constitutes one phase only
(b) Two immiscible liquids form two separate phases
(c) Miscible liquids form one liquid phase only
(d) A mixture of two or more solids constitutes one phase only
5. Dissociation of NH4Cl in a closed vessel is a
(a) Two components system
(b) One component system
(c) Three component system
(d) None of the above
30
[c]
6. A system consists of water in contact with its vapour. The degree of freedom is
(a) Zero
(b) One
(d) Unpredictable
[b]
7. Which of the following is condensed phase rule equation?
[a]
(a) F = C – P + 1
(c) Two
(b) F = C – P + 2
(c) C = F – P + 2
(d) F = C + P – 2
8. Phase rule
[c]
(a) Is of little value in case of very slow equilibrium state attaining system
(b) Cannot predict the behavior of a system under different set of conditions
(c) Requires information regarding molecular micro-structure of system
(d) Takes into congnizence the nature as well as quantities of components present
9. A binary system consisting of two substances, which are miscible in all proportions in
the liquid phase, but which do not react chemically is known as the
(a) Univariant system
(b) Eutectic system
(c) Metastable system
(d) Congruent melting system
[b]
10. Gibbs phase rule is
[b]
(a) F-P=C+2
11.
(b) F+P=C+2
(c) F-C=P+2
(d) P+C=F=2
At triple point of water system, the system is
(a) Invariant
(b) Univariant
[a]
(c) Bivariant
(d) Riparian
12. Eutectic point of a system and triple point are
(a) Identical
(b) Different
[d]
(c) Always same
(d) Both zero variant
13. When lead is progressively added to molten silver, the melting point of the resultant
alloy is
[a]
(a) Raised
(b) Lowered
(c) Unaltered
(d) Unpredictable
14. A system consists of a pure gas in equilibrium with its vapour. The degree of freedom
is
[b]
(a) 1
(b) 2
(c) 3
(d) 0
15. In Ag-Pb system at the eutectic, the number of phases at equilibrium are
(a) 1
(b) 2
(c) 3
(d) None
Fill in the blanks
1. In the expression C = N-E, E is the number of the independent equations.
31
[c]
2. If F = 0, the system is called invariant.
3. The phase rule for a one component system is given as F = 3-P.
4. The M.P of ice can be lowered by an increase of pressure.
5. If the pressure is kept constant, the phase diagram is called isobaric.
6. The solid-liquid system with gas phase absent is called a condensed system
7. A triple point is invariant.
8. The number of degrees of freedom for an invariant system is zero.
9. The main components of solders are Pb & Sn.
10. The curve above which the system consists of liquid only is liquids.
UNIT-8: MATERIAL CHEMISTRY: Cement: composition of Portland cement,
manufacture of port land cement & hardening of cement (reactions). Lubricants: Criteria of a
good lubricant, mechanism, properties of lubricants: Cloud point, pour point, flash & fire
point Viscosity. Refractories: Classification, Characteristics of a good refractory. Insulators
& conductors: classification of insulators, characteristics of thermal & electrical insulators
and applications of Super conductors (Nb-Sn alloy, Yba2Cu3O7-8), applications.
LEARNING OBJECTIVES

After completion of this unit the student should be able to:
1. Describe the composition of Port land cement, manufacture of port land cement.
2. Explain the setting and hardening of cement.
3. Explain the mechanism of lubricants.
4. Classify the Refractories.
5. Explain the characteristics of a good refractory.
6. Distinguish between Insulators and Conductors.
7. Differentiate thermal and electrical insulators.
8. Describe the applications of Super conductors.
9. Describe the applications of conductors.
32
10. Describe the applications of insulators.
Essay Questions
1. Explain with a schematic diagram the manufacture of Portland cement?
2. Define lubricant. What is the criteria of a good lubricant?
3. Define Refractory. Write down their classification and properties?
4. Explain with suitable examples classification of thermal and electrical insulators?
5. What is a superconductor? What are its applications?
6. Explain the following?
(a) Cloud point (b) Pour point (c) Flash & Fire point.
7. Explain how to determine viscosity of a lubricant using Red Wood Viscometer?
Multiple Choice Questions
1. The raw material needed for the manufacture of port land cement
(a) Limestone+clay+sand
(b) Lime stone+sand+gypsum
(c) Limestone+clay+gypsum
(d) Alumina+sand+gypsum
[c]
2. Major component of Portland cement is
(a) Tricalcium silicate
3.
5.
(c) MgO
(d)CaSO4
Cement made from high lime to silica ratio,is known as
(a) Sorel
4.
(b) CaO
[a]
(b) Silicate
(c) high-early
[b]
(d) Rapid-hardening
The function of gypsum is to
[a]
(a) Start the setting of cement
(b) Stop the hydration of cement
(c) Retard the easily initial setting of cement
(d) None of the above
A lubricant is used with the object of
(a) Increasing fractional heat
[c]
(b) Resistance increasing resistance
(c) Decreasing fractional (d) Providing direct contact between rubbing system
6.
A lubricant should possess high
(a) Volatility
7.
(b) Acidity
[c]
(c) Oiliness
A good lubricant should have
(d) None of these
[b]
33
(a) Low viscosity index
(b) High viscosity index
(c) Low fire point
(d) High viscosity
8. An acidic environment, preferably refractory should not be
(a) Acidic
9.
(b) Basic
(c) Neutral
(d) None of these
A good refractory material must
[b]
(a) Be chemically inactive in use
(b) Possess low softening of temperature
(c) Undergo spalling
(d) Possess high dermal expansion
10. A refractory material generally obtained from bauxite is
(a) Fireclay
(b) Dolomite
(c) Chromite
12.
13.
14.
15.
[a]
(b) Basic refractory (c) Neutral refractory (d) None of these
The single most important property of lubricating oil is its
(a) Fire point
(b) Cloud point
(c) Oiliness
[d]
(a) Rail axle boxes
(b) Gears
(c) Bearings working at high temperature
(d) Delicate instruments
A lubricant is used primarily to prevent
[c]
(a) Corrosion of metals
(b) Oxidation of metals
(c) Wearing out of rubbing metallic surfaces
(d) Reduction of metals
Lime contain more than 90%of calcium oxide is called……lime
(b) Hydraulic
[d]
(d) Viscosity index
Greases are not used to lubricant;
(a) Poor
[d]
(d) Alumina
11. Alumina is an example of
(a) Acidic refractory
[c]
(c) Fat
(d) Dolomite
Fill in the blanks
1. Lubricants for refrigeration are naphthalene oils.
2. Delicate instruments exhibit thick film lubrication.
3. Major component of Portland cement is tricalcium silicate.
4. Calcium sterate acts as a water proofing agent in cements.
5. The constituent of cement having least setting time is tricalcium aluminate.
6. Al2O3.2SiO2. 2H2O is the composition of the fire clay refractory.
7. Viscosity Of liquids decreases with increase in temperature.
34
[d]
8. High molecular weight oils possess high viscosity.
9. Graphite and carborrundum are neutral refractories.
10. A lubricant is used primarily to prevent naphthalene oils of rubbing metallic
surface.
35