CENTRAL INSTITUTE OF PLASTICS ENGINEERING & TECHNOLOGY
Question Bank
2 MARK ---QUESTION
COURSE : DPMT
SEMESTER: II
SUBJECT : Engineering Chemistry
1 MARK—QUESTION(MCQ)
-------
1. Modern Periodic table is based on ……………….
Answer:atomic number
2. The idea of stationary orbits was first given
by
a)Rutherfordb)J.J.Thomsonc)Niels Bohr d)
Max Plank
Answer: c) Niels Bohr
3. If A the number of nucleons and Z is the
number of neutrons and, then the number of protons in an atom is
givenby……………………
a) A+Z b)A-Z c)Z-A d)
none ofthese
Answer: b) A-Z
4. What does ‘AM’ stands for?
Answer:Atomic Mass
5. Electronic configuration of N (7)
is………………
Answer:1S22S22P3
6. The maximum
number of electrons that can be accommodated in an orbitis…………………..
a)2n b) n2c) 2n2d) 2n+1
Answer: c) 2n2
7. The mass number and atomic number of sulphur
atom are 32 and 16 respectively. Thenumber of neutrons in the nucleus is……………….
Answer: 16
8. The particle
with neutral charge in the nucleus is………..
a)proton b)electron c) neutron d)nucleus
Answer: c)neutron
9. Bohr’s model
can successfully explain the structure of hydrogen containing……….electron.
a) 1 b)
2 c) 3 d) 4
Answer: a) 1
10. What does
“VBT” stands for?
Answer: Valance Bond Theory
11. MOT stands
for……..?
Answer:Molecular orbital theory
12. d- Block
elements are also called ………. Metals.
a) alkali b)
alkaline c)transition d)alkaline earth
Answer:c) transition
13. f- Block
elements are also called ………. Metals.
a) alkali b)
inner transition c)transition d)alkaline earth
Answer:b) inner transition
14. …….have same
atomic number but different mass number.
Answer:Isotopes
15. Accordingto……….itisimpossibletodeterminesimultaneouslythe position
and velocity with accuracy of a small particle like electron.
a)Heisenberg’suncertaintyprinciple b) Bohr’s atomic model
c) Pauli’s exclusion principle d)Aufbau Rule
Answer:a) Heisenberg’suncertaintyprinciple
16. Out of the
following pairs of elements which has the same number of electrons in the
outermostenergy level…………………….
a) heliumand lithium
b) boronandcarbon c) carbon and
nitrogen d) lithium andhydrogen
Answer: d) lithium and hydrogen
17. The maximum
number of electrons that can be accommodated in d-subshellis………………
Answer: 10
18. Isobars have
same atomic number but different mass number (Say True orFalse)
Answer: False
19. The most
electronegative element in the periodic tableis…………………..
Answer: Fluorine
20. ………………..is
an electronic configuration of chromium(Cr-atomic number24).
a)1s22s22p63s23p64s23d4
b)1s22s22p63s23p64s13d5
c)1s22s22p63s23p54s23d5
d)1s22s22p63s23p54s23d4
Answer: b)1s22s22p63s23p64s13d5
21. Which one of the following is the most polar
…......
a)H-F b)H-Cl c)H-Br d)H-I
Answer: a) H-F
22. Covalent or
non-polar bond is formed by …………..of electron.
a) Accepting b) donating c) mutual sharing d) none of these
Answer: c)
mutual sharing
23. In a N2 molecule there are one sigma and two pi bonds
(Say True orFalse)
Answer: True
24.. .................... is
formed by sidewise overlapping of atomicorbitals.
Answer: Pi bond
25. The high boiling point of alcohol is due to………………….
a)Covalent bonding b)Ionicbonding c)Hydrogenbonding d) Coordinatebonding
Answer: c) Hydrogen bonding
26. An ionic
bond is formed between.
a) Two metals atoms b) Two
non-metals atoms
c) One metal atom and one non-metal atom d) One metal atom and and one non-metalloid
atom
Answer: c) One metal atom and one non-metal atom
27. In a
chemical bonding the atom attains …………configuration.
a) Partially filled
b) half-filled c) vacant d) octet or inert gas
Answer:d) octet or inert gas
28. Bonding
between a metal ion and a ligand is known as …………bond.
a)Covalent bonding b)Ionicbonding c)Hydrogenbonding d) Coordinatebonding
Answer: d) Coordinate bonding
29. ……… &
…………. are the two types of hydrogen bonding.
a)Inter and intramolecularb)Ionic and covalent c) ionic and coordinate d) None of the above
Answer: a)) Inter and Intramolecular
30. Hydrogen
bond is strongest in …………..
a) O-H…H
b)F-H…F c)O-H…O d) O-H…F
Answer: b)F-H…F
31. According to Lowry-Bronsted concept, an acid is a
substancethat…………………..
a) acceptsa proton
b)releasesaproton
c) acceptsaelectron
d) releases
aelectron
Answer: a) accepts a proton
32. Lewis base is a substance that accepts ………
Answer:lone pair of electron
33. Molecules or
ions that can behave both as Bronsted acid and base arecalled……………….
a)Monoprotic acids
b)polyprotic Acid
c)amphiproticsubstances
d) polyproticbases
Answer: c) amphiprotic substances
34. Nitric acid is a strong acid because ithas………………………
a) highmolecularmass
b)highlyunstable
c)high ionization
d) lowionization
Answer: c) high ionization
35. A weak base has ………..conjugate acid and a weak
acid has a ………..conjugate base.
Answer:strong, strong
36. Solution is a heterogeneous mixture of solute and solvent (Say True
orFalse)
Answer: false
37. The ionic product of water is……………………
Answer: 1 x 10-14
38. ………..of a
solution is the number of equivalents of solute per liter of the solution.
Answer: Normality
39.. Molarity of a solution is the number of
gram moles of solute per liter of thesolution.(Say True orFalse)
Answer: True
40. In a …………., the amount of solute is more in comparison to
saturatedsolution.
a) Saturated solution
b)unsaturated solution
c)super saturated solution
d) all of these
Answer: c) super saturated solution
41. Solution of pH = 9 is ________.
a) Acidic b) Buffer c) Neutral d) None of these
Answer: d) None of these
42. For the preparation of 1000 ml of 0.1 N solution of sulphuric acid,
the amount of H2SO4 needed is……………
a)4.9 g b)9.8
g c) 14.7g d) 19.6 g
Answer: a) 4.9 g
43. For the preparation of 1000 ml of 1 M solution of sodium carbonate,
the amount of Na2CO3 needed is……………
a)53 g b)106
g c) 10.6g d) 5.3 g
Answer: b) 106 g
44. Polar compounds are soluble in ………..solvents.
Answer:polar
45. Non-Polar compounds are soluble in non-polar solvents (Say True
orFalse)
Answer: True
46. pH<7, is generally calledas…………………….
Answer: acid
47. The taste of an acidis………………..
Answer: Sour taste
48.. Blue litmus Paper turns ………..colour,
ifitis acidic solution.
Answer: Red
49.. Red litmus paper turns blue colour,
ifitis............. solution.
Answer: Alkaline
50. The Major quantity of the solution is called as solvent. (Say True
orFalse)
Answer: True
51. Buffer solution is used to………………………
a) Increasethe pH
b) keep the pH remains same
c) decreasethe pH
d) None of these
Answer: b) Keep the pH remains same
52. Buffer
solution is a mixture of weak acid and its…………
Answer: conjugate base
53. Mixture of
NH4OH and NH4Cl solution is a…………buffer.
a) basic
b) acidic
c) neutral
d) salt
Answer: a) basic
54. pH + pOH
=………
a) 7 b) 14 c) 10 d) 12
Answer: b) 14
55. Sigma Bond
is weaker than pi bond .(Say True orFalse)
Answer: False
56. ……….. Water
produces lather with soap solution.
a) Hard b) soft
c) hot d) none of the above
Answer: b) soft
57. Temporary
hardness of water can also be called as ………….
a) Carbonate
b) non carbonate
c) alkaline
d) total
Answer: a) carbonate
58. ……………of Ca andMgcreate temporaryhardness of
water.
a) Carbonates
b) Bicarbonates
c) Carbonates and Bicarbonates
d) None of these
Answer: c) Carbonates and Bicarbonates
59. Hard water can be used for washing purposes (Say True orFalse)
Answer:False
60. Temporary Hardness of water can be removed by ………. the water.
Answer:Boiling
61. Full form of
ppb…..?
Answer: Parts per billion
62.. Magnesiumsulphate& chloridescreates........ hardness inwater.
a)Carbonate
b) Total
c) Temporary
d) Permanent
Answer: d) permanent
63. ………….waterhasH+andOH-ions.
a)Deionized
b)ionized
c) mineral
d) impure
Answer: a) Deionized
64. The degree of hardness of water is usually expressedas………………
Answer: parts per million(ppm)
65. pH stands
for…………..
Answer: Power of Hydrogen
66. Full form of
ppm……..
Answer: parts per million
67. Calgon, Na2[Na4(PO3)6]
is used as a………………………
a)water purifier
b)water hardener
c)watersoftener
d) none ofthese
Answer: c) water softener
68.. Soap is the ………….. of higher fattyacid.
Answer:sodium salt
69. Use of hard
water in boilers causes……………
a)Boiler corrosion b) scales &sludges c) caustic
embrittlement d) all the above
Answer: d) All the above
70. The general
formula of cationexchange resins is…………
a)RH+
b) ROH-
c) RH2O
d) All
the above
Answer: a) RH+
71. Anion
exchange resinscan be regenerated using……….
a) DiluteNaOH
b) HCl c) KMnO4 d) NH3
Answer: a)Dilute NaOH
72. Permanent hardness can be removedby………………………
a) Limesoda process
b)Permutit process
c)Ion-exchangeprocess
d) All of these
Answer: d) All of these
73. .Ground water contains appreciable amount of calcium and magnesium
salts(Say True orFalse)
Answer: True
74. Full form of
EDTA is……..
Answer: Ethylene diamine tetra acetic acid.
75. Full form of
EBT is……..
Answer:Eriochrome Black T
76. Hardness of
water is due to the presence of salts of……….
a)Potassium
b)chlorine c)Magnesium d)boron
Answer:c)Magnesium
77. The functional group of acidis……………….
a)RCOOH
b)RCOOR c)RCHO d)RCOR
Answer :a)RCOOH
78. Ester has
pleasant fruity smell. (say true or false)
Answer: True
79. Which one of following represents ketone
group.
(a) R-COOH (b)
R-CO-R (c) R-OH (d) R-COOR’
Answer: (b) R-CO-R
80. Acid
derivatives are…….
(a) Ester (b)
Amide (c) Anhydride (d) All of these
Answer: (d) All of these
81. What does
“TAN” stands for?
Answer: (d) Total acidity Number
82. Catenation is the property of carbon atom -
Saytrue or false.
Answer: True
83. What does
“VC” stands for?
Answer: Vinyl Chloride
84. Alkyl groups has one hydrogen shortage of Alkane compounds (Say
True orFalse)
Answer:
True
85. Catenation property of carbon is responsible for the large number of
carbon compounds due to its.
a)small size
b)tetrahedral structure
c)moderate electronegativity d)All
of these
Answer: d)All of these
86. All Organic compounds mainly consist
of…………………..
Answer: Carbon and Hydrogen
87. Cyclic Compounds Contain one atom(Sulphur,
Oxygen, Nitrogen) other than carbonis called………………………………
Answer: Heterocyclic Compounds
88. The general formula for alkaneis………………………….
a)CnH2n+2
b)CnH2n
c)CnH2n-2
d)CnH2n+4
Answer: a) CnH2n+2
89. The first synthesized organic compound from an
ammonium cyanate is…………..
Answer: Urea
90. The general formula for alkeneis………………………….
a)CnH2n+2
b)CnH2n
c)CnH2n-2
d)CnH2n+4
Answer: b) CnH2n
91. The general formula for alkyneis………………………….
a)CnH2n+2 b)CnH2n c)CnH2n-2 d)CnH2n+4
Answer: c) CnH2n-2
92. Methane is a major constituent of …………..
Answer :natural gas
93. 74. LPG ismixed with to detect leakage.
a)hydrogen b)oxygen c)mercaptans d)nitrogen
Answer: c) mercaptans
94. The antiknock property of the fuel depends
onits
a)Self-ignitiontemperature
b)
Molecularstructure
c)Chemicalcomposition
d) All of
theabove
Answer: d) All of the above
95. Decomposition
of higher hydrocarbon molecules into lower hydrocarbons having lower
boiling temperatures is known as Hydrogenation (say true or
false)
Answer: false
96. The heat energy released is measured with the
help of …………
Answer: Calorimeter
97.. Bomb calorimeter is used
to determine the calorific value of the…............ fuels
a)Solid fuels
b) Liquid fuels
c) both a& b
d) None of the abov
Answer: c) both a & b
98.. KJ/mol is the unit of………….
a)Calorific value b)Work
c)Specific Heat d)Thermal
conductivity
Answer:a) Calorific value
99. Coal is a …………..fuel, whereas coke is a
……….fuel.
Answer:
primary& secondary
100.Full form of LPG………
Answer:Liquified
Petroleum Gas.
101.Full
form of TEL………
Answer: Tetra
Ethyl Lead
102.Octane
number of isooctane is ……………
a) 50 b) 1
c) 100 d) 5
Answer: c)
100
103.Knocking
…….. the efficiency of petrol engine.
a)
increases b) decreases c) will not affect d) none of these
Answer:b)
decreases
104.Diesel
can be obtained by the fractional distillation of ………….
Answer: crude
oil
105.A
mixture of ……………..is known as water gas.
Answer:
carbon monoxide and hydrogen
106.Coke
is a secondary solid fuel. (Say true or false)
Answer: True
107.The
liquefied petroleum gas (LPG) marketed by Indian oil corporation is
called………………..
Answer:Indane
108.A
petroleum fraction obtained between 180-2500Cis……………..
a) Petrol b) diesel c) Kerosene d) none of these
Answer: c) Kerosene
109.The
fermentation process of cattle dung in the absence of air produces……….
Answer: Gobar
gas
110.The
combustion rate of solid fuels is slow because of the difficulty of thorough
contact betweenthe solid fuel and oxygen. (Say True or False)
Answer: True
111.Burning
of coal and dieselreleases………………….
a)NO2 b)CO2 c) SO2 d)CO
Answer: c) SO2
112.The
antiknock property of gasoline can be increased by adding……….
Answer: TEL
113.Flow
of electrons across the electrodes is known as …………
Answer: Electric Current
114.The
conductance of a solution of an electrolyte generally increases with rise in
temperature(Say True or False)
Answer: True
115.The units
of specific conductanceare………………….
Answer: ohm-1cm-1
116.The
conductivity of an electrolyte is due tothe………………………..
a) presence of ions intheelectrolyte
b) free movement of ions in thesolution
c) reunion of ions inthesolution
d) release of heat energy due toionization
Answer: b) free movement of ions in the solution
117.On passing
electrical current through an electrolyte solution…………………
a) cations movetowardsanode b)
cations move towards cathode and anions towardsanode
c) anions movetowardscathode d) both
cations and anions move in samedirection
Answer: b) cations move towards cathode and anions towards
anode
118.The
fraction of total current carried by the cation and anion is termedas……………….
Answer: Transport number
119.The sum of
the transport number of cation and anion is equalto…………….
a)1 b)0 c)0.5 d)Infinity
Answer: a) 1
120.The ionic
mobility of Li+ is small as compared to that of K+. It is
because Li+ ion is heavily hydrated (Say True orFalse)
Answer: True
121.One faraday is
equalto………………..
a)96.500coulombs
b)9650coulombs
c)965.00coupons
d)96500coulombs
Answer: d) 96500 coulombs
121. Corrosion isa(an)............... process.
a)oxidation
b)reduction
c)electrolysis
d)erosi
Answer: a) oxidation
122.………..metal is used as a coating
on steel to limitcorrosion.
Answer: Zinc
123.Corrosion startsat the …………. of
the metal.
a) surface b)middle c)bottom d)side
Answer: a) Surface
124.The
electrode where reduction occursiscalled…………….
Answer: b) cathode
125.Positive
electrode is known as……….
a)Terminal b) Anode
c) Cathode d) None of these
Answer: b) Anode
126.Rust
is………………….
a) Hydratedcoppersulphate
b)
Hydrated ferroussulphate
c) Hydratedferricoxide
D) Hydrated ferrousoxide.
Answer: c) Hydrated ferric oxide
127.Among
lead, iron, chromium, and copper, the least easily oxidized metalis…………..
Answer: copper
128.Series
connection of a number a number of cells is known as……………
Answer:
battery.
129.Lead
acid battery is a……………..battery.
a)Primary
b) secondary
c) quaternary
d) None of these
Answer: b)
secondary
130.The
anode used in lead storage battery is……………
a)Pb b)PbO2on Pb c)only PbO2d)Zn
Answer: a)Pb
131.In
Daniel cell ……… are used as anode and
cathode respectively.
a)Zn &
Cu b) Cu & Zn c)Cu &Pb
d) Zn &Pb
Answer: a) Zn
& Cu
132.In
the electrolytic refining of metal,the pure metal is used as………..
Answer:
cathode
133.In
electrochemical cell electrical energy in converted in to chemical energy. (say
true or false)
Answer: False
134.A
beaker containing hot water, it is the example of ………..thermodynamic system.
Answer: open
135.The
process in which the volume of the system is remains constant is called as
……….
a) Isobaricb)
Isochoricc) Adiabatic d) Isothermal
Answer: b)
Isochoric
136.In
endothermic process heat is _________.
a) Evolved
b) absorbed c) increased d)
decreased
Answer:b)
absorbed
137.In
exothermic process heat is _________.
(a) Evolved
(b) absorbed (c) increased (d)
decreased
Answer: a)
evolved
138.The
process in which the temperature of the system is remains constant is called
asIsochoric.
(Say true or
false)
Answer:False
139.The study
of the flow of heat or any other form of energy into or out of a system
undergoing
physicalor chemical change
iscalled………………….
Answer: Thermodynamics
140.Thermodynamics
is applicable to macroscopic systems only (Say True orFalse)
Answer: True
141.In an
exothermic reaction the heat energy is……………..while in endothermic reaction
itis…………
a)released,released b)
released, absorbed
c)absorbed,released d)
absorbed,absorbed
Answer: b) released, absorbed
142.The
mathematical relation for the first law of thermodynamicsis……………
a)ΔE=q-w b) ΔE=0 for
acyclicprocess
c) ΔE=q for anisochoricprocess d) all ofthese.
Answer: d) all of these
143.In an
adiabatic process no heat can flow into or out of the system (Say True orFalse)
Answer: True
144.A
thermoflask is an example of…………………
Answer: Isolated system
145.For an
idealgas……………
Answer: PV = nRT
146.A
process which proceeds of its own accord, without any outside assistance
iscalled…………..
a) Non-spontaneousprocess b)
spontaneousprocess
c) Reversibleprocess d)
irreversibleprocess
Answer: b) Spontaneous process
147.Entropy
is ameasureof of the molecules of
thesystem.
a)Concentration b)Velocity c)zig-zagmotion d) randomness ordisorder
Answer: d) randomness or disorder
148.A
machine that can do work by using heat which flows out spontaneously from a
high-temperature source to a low temperature sink iscalled…………………
a) Carnot machine
b) Cyclicmachine c)
Heatmachine d) Heat engine
Answer: d) Heat engine
149.Mixing of
two or more gases is a spontaneous process (Say True orFalse)
Answer: True
150.∆G is stands for……
Answer: Change in Gibbs free energy.
151.∆H is stands for……
Answer: Change in Enthalpy
152.∆S is stands for……
Answer: Change in Entropy
153.The
mathematical reaction for the first law of thermodynamics is…..
a) ∆E=q-W
b) ∆E=0 for a cyclic process
c) ∆E=q for an isochoric processes
d) all of these
Answer: d)
all of these
154.A
closed system is one which cannot transfer matter but transfer…………….to and from
its surrounding.
a)Heat b)work
c)radiation d)all of these
Answer: d)
all of these
155.Enthalpy
is an example for………….. property.
a) Isothermal b)
adiabatic c) intensive d) extensive
Answer: d)
extensive
156.An
intensive property does not depend upon the………
a)Nature of the substance
b) quantity of matter
c) External temperature
d) atmospheric pressure
Answer: a)
Nature of the substance
157.Precipitation
of silver chloride from silver nitrate & sodium chloride is an example
for………reaction
a)reversible b)
irreversible c) neutral d) none of the above
Answer: b)
irreversible
158.For
an endothermic reaction………
a) (∆S > 0) & (+∆H)
b) (∆S < 0) & (+∆H)
c)(∆S< 0)&(-∆H)
d) (∆S
> 0)&(-∆H)
Answer:b) (∆S < 0) & (+∆H)
159.When…………….,
heat is transferred into the system.
a) q>0 b) q<0
c) q=0 d) all the above
Answer
a)q>0
160.w<0
shows that, work is done ……the system.
a) on b) by
c) through d) all the above
Answer: b) by
161………….is
not an intensive property.
a)Volume b)Pressure
c)Density d)Concentration
Answer: a) Volume
162.∆E is stands for……
Answer: Change in Internal energy
163.The
entropy of the system increases in the order…………………….
a) gas< liquid<solid
b) solid < liquid<gas c)
gas < solid<liquid d) none
ofthese
Answer: b) solid < liquid < gas
164.............. ……
is the unit for entropy.
a)KJ mol-1 b)JK-1mol c)JK-1mol-1 d) KJmol
Answer: c)JK-1mol-1
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