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Questions:

Multiple Choice Question

99 x 1 = 99

If in a mixture where Q = k is combined, then what happens?

(a)

the reaction shift towards products

(b)

the reaction shift towards reactants

(c)

nothing appears to happen, but forward and reverse are continuing at the same rate

(d)

nothing happens

What effect does a catalyst have on the equilibrium position of a reaction?

(a)

a catalyst favours the formation of products

(b)

a catalyst favours the formation of reactants

(c)

a catalyst does not change the equilibrium position of a reaction

(d)

a catalyst may favour reactants or product formation, depending upon the direction in which the reaction is written.

H₂ + S ⇌ H₂S + energy.
In this reversible reaction, select the factor which will shift the equilibrium to the right.

(a)

adding heat

(b)

adding H₂S

(c)

blocking hydrogen gas reaction

(d)

removing hydrogen sulphide gas

In a closed system
A(S) ⇌ 4 B(g) + 3 C(g)
If partial pressure of C is doubled, then partial pressure of B will be _____.

(a)

\(2\sqrt { 2 } \)times the original value

(b)

\(\frac { 1 }{ 2 } \)times the original value

(c)

2 times of the original value

(d)

\(\frac { 1 }{ 2\sqrt { 2 } } \)times of the original value

A catalyst will increase the rate of a chemical reaction by ______.

(a)

shifting the equilibrium to the right

(b)

shifting the equilibrium to the left

(c)

lowering the activation energy

(d)

increasing the activation energy

The equilibrium expression, K_c= [CO₂] represents the reaction.

(a)

C(s) + O₂(g) ⇌ CO₂(g)

(b)

CaCO₃(s) ⇌ CaO(s) + CO₂(g)

(c)

CO(g) + \(\frac { 1 }{ 2 } \) O₂(g) ⇌ CO₂(g)

(d)

CaO(s) + CO₂(g) ⇌ CaCO₃(s)

For an endothermic reaction ______.

(a)

\(\Delta\)H is-ve

(b)

\(\Delta\)H is+ve

(c)

\(\Delta\)H is zero

(d)

none of these

Which of the following always has a negative value?

(a)

heat of reaction

(b)

heat of solution

(c)

heat of combustion

(d)

heat of formation

Which of the following properties is not a function of state?

(a)

concentration

(b)

internal energy

(c)

enthalpy

(d)

entropy

10.

For a cyclic process, the change in internal energy of the system is ______.

(a)

always +ve

(b)

equal to zero

(c)

always -ve

(d)

none of the above

11.

An isochoric process takes place at constant ______.

(a)

temperature

(b)

pressure

(c)

volume

(d)

concentration

12.

Thermodynamics is applicable to ______.

(a)

macroscopic system only

(b)

microsopic system only

(c)

homogeneous system only

(d)

heterogeneous system only

13.

Tolueue reacts with chlorine in the presence of light to give ______.

(a)

benzyl choride

(b)

benzoyl chloride

(c)

p-chlorotoluene

(d)

o-chlorotoluene

14.

Benzene reacts with acetyl chloride in the presence of AlCl₃ to give ______.

(a)

acetophenone

(b)

toluene

(c)

benzophenone

(d)

ethyl benzene

15.

Baeyer's reagent is ______.

(a)

aqueous KMnO₄

(b)

neutral KMnO₄

(c)

alkaline KMnO₄

(d)

aqueous bromine water

16.

The catalyst required for the given reaction is ______.
\(HC\equiv CH+dil{ \quad H }_{ 2 }{ SO }_{ 4 }\overset { Catalyst }{ \longrightarrow } { CH }_{ 3 }CHO\)

(a)

HgSO₄

(b)

(c)

A1CI₃

(d)

17.

A liquid hydrocarbon is converted to a mixture of gaseous hydrocarbon by ______.

(a)

hydrolysis

(b)

oxidation

(c)

distillation

(d)

cracking

18.

The IUPAC name of this compound is

(a)

3-ethyl-4-chloro-1, 4-pentadiene

(b)

2-chloro-3-ethyl-1, 4-pentadiene

(c)

4-chloro ethyl-1-pentene

(d)

3-ethyl-4-chloro-4-pentene

19.

The hybridization state of a carbocation is ______.

(a)

Sp⁴

(b)

sp³

(c)

sp²

(d)

20.

The reaction

(a)

carbocation formation

(b)

free-radical mechanism

(c)

carbanion formation

(d)

none of these

21.

The bond that undergoes heterolytic cleavage most readily is ______.

(a)

C-C

(b)

C-O

(c)

C-H

(d)

O-H

22.

The IUPAC name of ______.

(a)

1, 2-dichloropropane

(b)

3, 3-dichloropropane

(c)

1, 1-dichloropropane

(d)

dichloropropane

23.

The maximum number of electrons in a sub-shell is given by the equation _______.

(a)

n²

(b)

2n²

(c)

21-1

(d)

21 + 1

24.

The outermost electronic configuration of manganese (at. no. = 25) is _______.

(a)

3d⁵4s²

(b)

3d⁶4s¹

(c)

3d⁷4s^o

(d)

3d⁶ 4s²

25.

The orbital with n = 3 and 1 = 2 is _______.

(a)

(b)

(c)

(d)

26.

The Balmer series in the spectrum of hydrogen atom falls in _______.

(a)

ultraviolet region

(b)

visible region

(c)

infrared region

(d)

none of these

27.

Cathode rays are deflected by _______.

(a)

electric field only

(b)

electric and magnetic field

(c)

magnetic field only

(d)

none of these

28.

Which of the following is used in photoelectric cells?

(a)

(b)

(c)

(d)

29.

Hydrides as well as halides of alkaline earth metals tend to polymerize

(a)

(b)

(c)

(d)

30.

Which of the following is not a peroxide?

(a)

KO₂

(b)

CrO₅

(c)

Na₂O₂

(d)

BaO₂

31.

The oxide of which of the following metals is amphoteric?

(a)

(b)

(c)

(d)

32.

In the Solvay process

(a)

an ammoniacal brine solution is carbonated with CO₂, forming NaHCO3 which on decomposition at 150^oC produces Na₂CO₃

(b)

a sodium amalgum reacts with water to produce NaOH which gives Na₂CO₃ on reacting with CO₂

(c)

A brine solution is made to react with BaCO₃ to produce Na₂CO₃

(d)

all of the above

33.

Lithium shows a diagonal relationship with

(a)

sodium

(b)

silicon

(c)

nitrogen

(d)

magnesium

34.

When heated to 800^oC, NaNO₃ gives

(a)

Na+N₂+O₂

(b)

NaNO₂+O₂

(c)

Na₂O+O₂+N₂

(d)

NaN₃+O₂

35.

Which of the following is the least thermally stable?

(a)

MgCO₃

(b)

CaCO₃

(c)

SrCO₃

(d)

BeCO₃

36.

Which of the following gases will have the lowest rate of diffusion?

(a)

H₂

(b)

N₂

(c)

F₂

(d)

O₂

37.

The compressibility factor, z for an ideal gas is

(a)

zero

(b)

less than one

(c)

greater than one

(d)

equal to one

38.

In van der Waals equation of state for a non-ideal gas the net force of attaction among the molecules is given by

(a)

\(\frac{an^2}{V^2}\)

(b)

P+\(\frac{an^2}{V^2}\)

(c)

P-\(\frac{an^2}{V^2}\)

(d)

-\(\frac{an^2}{V^2}\)

39.

The cleansing action of soaps and detergents is due to

(a)

internal friction

(b)

high hydrogen bonding

(c)

viscosity

(d)

surface tensions

40.

Viscosity of a liquid is a measure of

(a)

repulsive forces between the liquid molecules

(b)

frictional resistance

(c)

intermolecular forces between the molecules

(d)

none of the above

41.

With rise in temperature, the surface tension of a liquid

(a)

decreases

(b)

increases

(c)

remaining the same

(d)

none of the above

42.

At constant temperature, the pressure of the gas is reduced to one-third, the volume

(a)

reduce to one-third

(b)

increases by three times

(c)

remaining the same

(d)

cannot be predicted

43.

Which of the following is the correct mathematical relation for Charles law at constant pressure?

(a)

V\(\alpha\)T

(b)

V\(\alpha\)t

(c)

V\(\alpha\)\(\frac{1}{2}\)

(d)

all of above

44.

The average kinetic energy of the gas molecule is

(a)

inversely proportional to its absolute temperature

(b)

directly proportional to its absolute temperature

(c)

equal to the square of its absolute temperature

(d)

All of the above

45.

For one mole of a gas, the ideal gas equation is

(a)

PV =\(\frac{1}{2}\)RT

(b)

PV=RT

(c)

PV =\(\frac{3}{2}\)RT

(d)

PV =\(\frac{5}{2}\)RT

46.

Silicon shows a diagonal relation with

(a)

magnesium

(b)

phosphorous

(c)

carbon

(d)

boron

47.

Which of the following molecules have zero dipole moment?

(a)

CS₂

(b)

CO₂

(c)

CCl₂

(d)

CH₂Cl₂

48.

Silicones are a group of organosilicon polymers containing

(a)

Si - O - Si linkages

(b)

0 - Si - 0 linkages

(c)

Si - C - Si linkages

(d)

Si - Si - 0 linkages

49.

Which of the following is a purely acidic oxide?

(a)

Si0₂

(b)

Sn0₂

(c)

PbO

(d)

Mn0₂

50.

Silicon carbide (SiC) is known as

(a)

quartz

(b)

tridynite

(c)

corundum

(d)

carborundum

51.

Carbon-60 contains

(a)

20 pentagons and 12 hexagons

(b)

12 pentagons and 20 hexagons

(c)

30 pentagons and 30 hexagons

(d)

24 pentagons and 36 hexagons

52.

Which of the following compound is an important catalyst as well as a Lewis acid?

(a)

Al₂S₂

(b)

BF₃

(c)

S₄N₄

(d)

N₂H₄

53.

Boron has an extremely high melting point because of

(a)

its ionic crystal structure

(b)

the strong binding forces in the covalent polymer

(c)

atomic size

(d)

allotropy

54.

In the ethylene molecule the two carbon atoms have the oxidation numbers.

(a)

-1, -1

(b)

-2, -2

(c)

-1, -2

(d)

+2,-2

55.

Which one among the following is not example of autoredox reaction?

(a)

\({ P }_{ 4 }+{ OH }^{ - }\longrightarrow { H }_{ 2 }{ PO }_{ 4 }^{ - }+{ PH }_{ 3 }\)

(b)

\({ H }_{ 2 }{ O }_{ 2 }\longrightarrow { H }_{ 2 }{ O+O }_{ 2 }\)

(c)

\({ S }_{ 2 }{ O }_{ 3 }^{ 2- }\longrightarrow S{ O }_{ 4 }^{ 2- }+S\)

(d)

\(AgCl+{ NH }_{ 3 }\longrightarrow [Ag({ NH }_{ 3 })_{ 2 }]Cl\)

56.

Which of the following are not redox reactions?

(a)

Mg + N₂ \(\rightarrow\) Mg₃N₂

(b)

K4[Fe (CN)₆] + H₂S0₄ + H₂0 \(\rightarrow\) K₂S0₄ + CO + FeS0₄ + (NH₄)₂S0₄

(c)

\({ S }_{ 2 }{ O }_{ 3 }^{ 2- }\longrightarrow S{ O }_{ 4 }^{ 2- }+S\)

(d)

\(AgCl+{ NH }_{ 3 }\longrightarrow [Ag\left( { NH }_{ 3 } \right) 2]Cl\)

57.

The oxidation number of carbon 'is zero in ______.

(a)

HCHO

(b)

CH₂Cl₂

(c)

C₁₂H₂₂O₁₁

(d)

All the above

58.

When methane is burnt in oxygen to produce CO₂ and H₂0 the oxidation number of carbon changes by ______.

(a)

-8

(b)

Zero

(c)

(d)

59.

The reaction: CH₃CH₂I + KOH_(aq) \(\rightarrow\)CH₃CH₂OH + KI is classified as :________.

(a)

electrophilic substitution

(b)

nucleophilic substitution

(c)

elimination

(d)

addition

60.

In the Lassaigne’s test for nitrogen in an organic compound, the Prussian blue colour is obtained due to the formation of: ______.

(a)

Na₄[Fe(CN)₆]

(b)

Fe₄[Fe(CN)₆]₃

(c)

Fe₂[Fe(CN)₆]

(d)

Fe₃[Fe(CN)₆]₄

61.

Which of the following will increase the BOD of water supply?

(a)

O₃

(b)

C₂H₅OH

(c)

H₂O

(d)

CO₂

62.

Besides CO₂, the other greenhouse gas is

(a)

(b)

N₂

(c)

O₂

(d)

CH₄

63.

Which of the following causes less pollution?

(a)

NO_x

(b)

SO_x

(c)

CO₂

(d)

C_xH_y

64.

Which of the following acid is most abundant in acid rain?

(a)

HCl

(b)

HNO₃

(c)

H₂SO₄

(d)

Organic acid

65.

The oxidation number of the carboxylic carbon atom in CH₃COOH is ______.

(a)

(b)

(c)

(d)

66.

On the reaction 2Ag + 2H₂SO₄ \(\rightarrow\) Ag₂So₄ + 2H₂O+S_O2 sulphuric acid acts as ______.

(a)

an oxidizing agent

(b)

a reducing agent

(c)

a catalyst

(d)

an acid as well as an oxidant

67.

Which of the following is most powerful oxidizing agent in the following

(a)

O₃

(b)

KMnO₄

(c)

H₂O₂

(d)

K₂Cr₂O₇

68.

Which of the following halogens do not exhibit a positive oxidation number in their compounds?

(a)

(b)

(c)

(d)

69.

Among the following molecules, in which does bromine show the maximum oxidation number?

(a)

Hg₂ (Br0₃)₂

(b)

Br - Cl

(c)

KBrO₄

(d)

Br₂

70.

Out of the following, intramolecular hydrogen bonding exists in ______.

(a)

water

(b)

H₂S

(c)

4-nitrophenol

(d)

2-nitrophenol

71.

sp³, sp² and sp hybridized carbon atom, the p character is maximum in:______.

(a)

sp³

(b)

sp²

(c)

(d)

all of the above have same p-character

72.

Which one is diamagnetic among NO⁺, NO and NO^-?

(a)

NO⁺

(b)

(c)

NO^-

(d)

None of these

73.

In SO₂ molecule, S atom is: ______.

(a)

sp³ hybridized

(b)

sp hybridized

(c)

sp² hybridized

(d)

d sp² hybridized

74.

The species CO, CN^- and N₂ are ______.

(a)

isoelectronic

(b)

having coordinated bond

(c)

having polar bond

(d)

having low bond energies

75.

A co-ordinate bond is formed by ______.

(a)

sharing of electrons contributed by both the atoms

(b)

complete transfer of electrons

(c)

sharing of electrons contributed by one atom only

(d)

none of these

76.

Water undergoes self-ionization to a small extent to give

(a)

H⁺ and OH^-

(b)

OH⁺ and H^-

(c)

H₃O⁺ and OH^-

(d)

none of the above

77.

Zeolite is

(a)

hydrated sodium aluminium silicate - Na₂Al₂Si₂O₈.xH₂O

(b)

hydrated ferric oxide

(c)

sodium hexametaphosphate

(d)

sodium tetraborate

78.

Hydrogen is obtained as a by-product in the

(a)

electrolysis of water

(b)

manufacture of caustic soda

(c)

Bosch process

(d)

Lane process

79.

The higher density of water than that of ice is due to

(a)

dipole-dipole interaction

(b)

dipole-induced dipole interaction

(c)

hydrogen bonding

(d)

all of these

80.

Calgon, which is used as a water softener, has the formula

(a)

Na₄ [Na₂ (PO₃)₆]

(b)

Na₂ [Na₄(PO₃)₆]

(c)

Na₂[Na₄(PO₄)₅]

(d)

Na₂ [Na₂ (PO₄)₆]

81.

On treatment of hard water with zeolite, sodium ions get exchanged with

(a)

Ca²⁺ ions

(b)

Mg²⁺ ions

(c)

H⁺ ions

(d)

OH^-

82.

Water may be softened using

(a)

sodium aluminium silicate

(b)

Graham's salt

(c)

an ion exchange resin

(d)

trisodium phosphate

83.

Hydrogen gas is generally prepared by the

(a)

reaction of granulated zinc with dilute H₂SO₄

(b)

reaction of zinc with conc. H₂SO₄

(c)

reaction of pure zinc with dil. H₂SO₄

(d)

action of steam on red hot coke.

84.

Which one of the following alkaline earth metal carbonates is thermally most stable

(a)

MgCO₃

(b)

CaCO₃

(c)

SrCO₃

(d)

BaCO₃

85.

Which one of the following alkali metals give hydrated salts?

(a)

(b)

(c)

(d)

86.

Which element has smallest size?

(a)

(b)

(c)

(d)

87.

Which one of the following is isoelectronic with Ne?

(a)

N3^-

(b)

Mg²⁺

(c)

AI³⁺

(d)

all of the above

88.

Which of the following species are not known?

(a)

AgOH

(b)

PbI₄

(c)

PI₅

(d)

SH₆

89.

What is the electronic configuration of the elements of group 14?

(a)

ns² np⁴

(b)

ns²np⁶

(c)

ns² np²

(d)

ns²

90.

The highest ionization energy is exhibited by _____.

(a)

halogens

(b)

alkaline earth metals

(c)

transition metals

(d)

noble gases

91.

As per the available data: ______.

(a)

CH₄(g) + 2O₂(g) \(\rightarrow \) CO₂(g) + 2H₂O(l); \(\triangle \)_C\(H^{ \ominus }\) = -890.3 KJ mol^-1

(b)

C(s) + O₂(g) \(\rightarrow \) CO₂(g) \(\triangle \)_C\(H^{ \ominus }\)=-393.5 KJ mol^-1

(c)

H2(g) + 1/2O2(g) \(\rightarrow \) H2O (l); \(\triangle \)_C\(H^{ \ominus }\)= -285.8 KJ mol^-1

92.

A reaction, A + B → C + D + q is found to have a positive entropy change. The reaction will be _______.

(a)

possible at high temperature

(b)

possible only at low temperature

(c)

not possible at any temperature

(d)

possible at any temperature

93.

\(\triangle U^{ \ominus }\)of combustion of methane is – X kJ mol^–1. The value of \(\triangle H^{ \ominus }\) is _______.

(a)

\(=\triangle U^{ \ominus }\)

(b)

\(>\triangle U^{ \ominus }\)

(c)

\(<\triangle U^{ \ominus }\)

(d)

94.

The enthalpies of all elements in their standard states are: _______.

(a)

unity

(b)

zero

(c)

(d)

different for each element

95.

The mass of an atom of nitrogen is _______.

(a)

\(\frac { 14 }{ { { 6.023\times 10 }^{ 23 } } } \)

(b)

\(\frac { 28 }{ { { 6.023\times 10 }^{ 23 } } } \)g

(c)

\(\frac { 1 }{ { { 6.023\times 10 }^{ 23 } } } \)g

(d)

14 amu

96.

The number of significant figures in 0.0101 is _______.

(a)

(b)

(c)

(d)

97.

Which of the following has the highest mass?

(a)

1 g atom of C

(b)

\(\frac { 1 }{ 2 } \)mole of CH₄

(c)

10 mL of water

(d)

3.011 x 10²³atoms of oxygen

98.

5.6 litres of oxygen at NTP is equivalent to _______.

(a)

1 mole

(b)

\(\frac { 1 }{ 4 } \)mole

(c)

\(\frac { 1 }{ 8 } \)mole

(d)

\(\frac { 1 }{ 2 } \)mole

99.

One mole of CO₂ contains _______.

(a)

6.02 x 10²³atoms of C

(b)

3 g of CO₂

(c)

6.02 x 10²³atoms of O

(d)

18.1 x 10²³ molecules of CO₂

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Answers Key:

Multiple Choice Question

99 x 1 = 99

(a)
adding heat

(d)
\(\frac { 1 }{ 2\sqrt { 2 } } \)times of the original value

(b)
CaCO₃(s) ⇌ CaO(s) + CO₂(g)

(b)
\(\Delta\)H is+ve

(a)
concentration

10.

(b)
equal to zero

11.

12.

(a)
macroscopic system only

13.

(a)
benzyl choride

14.

(a)
acetophenone

15.

16.

(a)
HgSO₄

17.

(d)
cracking

18.

(b)
2-chloro-3-ethyl-1, 4-pentadiene

19.

20.

(b)
free-radical mechanism

21.

(d)
O-H

22.

23.

(d)
21 + 1

24.

(a)
3d⁵4s²

25.

26.

(b)
visible region

27.

(b)
electric and magnetic field

28.

(d)
Cs

29.

30.

(a)
KO₂

31.

(a)
Pb

32.

33.

(d)
magnesium

34.

35.

(d)
BeCO₃

36.

37.

(d)
equal to one

38.

(a)
\(\frac{an^2}{V^2}\)

39.

(d)
surface tensions

40.

(b)
frictional resistance

41.

(a)
decreases

42.

(b)
increases by three times

43.

(a)
V\(\alpha\)T

44.

(b)
directly proportional to its absolute temperature

45.

(b)
PV=RT

46.

(d)
boron

47.

(a)
CS₂

48.

(a)
Si - O - Si linkages

49.

(a)
Si0₂

50.

(d)
carborundum

51.

(b)
12 pentagons and 20 hexagons

52.

(d)
N₂H₄

53.

(b)
the strong binding forces in the covalent polymer

54.

(b)
-2, -2

55.

(d)
\(AgCl+{ NH }_{ 3 }\longrightarrow [Ag({ NH }_{ 3 })_{ 2 }]Cl\)

56.

(d)
\(AgCl+{ NH }_{ 3 }\longrightarrow [Ag\left( { NH }_{ 3 } \right) 2]Cl\)

57.

(d)
All the above

58.

(d)
+4

59.

(b)
nucleophilic substitution

60.

(b)
Fe₄[Fe(CN)₆]₃

61.

62.

63.

64.

65.

(d)
+3

66.

(d)
an acid as well as an oxidant

67.

(a)
O₃

68.

(a)
F

69.

70.

(d)
2-nitrophenol

71.

(a)
sp³

72.

(a)
NO⁺

73.

74.

(a)
isoelectronic

75.

76.

77.

(a)
hydrated sodium aluminium silicate - Na₂Al₂Si₂O₈.xH₂O

78.

(b)
manufacture of caustic soda

79.

80.

(b)
Na₂ [Na₄(PO₃)₆]

81.

(a)
Ca²⁺ ions

82.

83.

(a)
reaction of granulated zinc with dilute H₂SO₄

84.

(d)
BaCO₃

85.

(a)
Li

86.

(b)
N

87.

(d)
all of the above

88.

89.

90.

(b)
alkaline earth metals

91.

(a)
CH₄(g) + 2O₂(g) \(\rightarrow \) CO₂(g) + 2H₂O(l); \(\triangle \)_C\(H^{ \ominus }\) = -890.3 KJ mol^-1

92.

(d)
possible at any temperature

93.

94.

(b)
zero

95.

(b)
\(\frac { 28 }{ { { 6.023\times 10 }^{ 23 } } } \)g

96.

(a)
3

97.

(a)
1 g atom of C

98.

(b)
\(\frac { 1 }{ 4 } \)mole

99.

(a)
6.02 x 10²³atoms of C

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