11th Public Exam March 2019 Important One Marks Questions

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Questions:

Multiple Choice Question

95 x 1 = 95

The First ionisation potential of Na, Mg and Si are 496, 737 and 786 kJ mol^-1 respectively. The ionisation potential of Al will be closer to ___________

(a)

760 kJ mol^-1

(b)

575 kJ mol^-1

(c)

801 kJ mol^-1

(d)

419 kJ mol^-1

IE₁ and IE₂ of Mg are 179 and 348 kcal mol^-1 respectively. The energy required for the reaction Mg⟶ Mg²⁺ + 2e^- is ___________

(a)

+169 kcal mol^-1

(b)

- 169 kcal mol^-1

(c)

+ 527 kcal mol^-1

(d)

- 527 kcal mol^-1

The correct order of decreasing electronegativity values among the elements X, Y, Z and A with atomic numbers 4, 8, 7 and 12 respectively __________

(a)

Y > Z > X > A

(b)

Z > A > Y > X

(c)

X > Y > Z > A

(d)

X > Y > A > Z

Which one of the following arrangements represent the correct order of least negative to most negative electron gain enthalpy _______________.

(a)

Al < O < C < Ca < F

(b)

Al < Ca < O < C < F

(c)

C < F < O < Al < Ca

(d)

Ca < Al < C < O < F

In the third period the first ionization potential is of the order.

(a)

Na > Al > Mg > Si > P

(b)

Na < Al < Mg < Si < P

(c)

Mg > Na > Si > P > Al

(d)

Na< Al < Mg < Si < P

Van't Hoff equation is ___________

(a)

\(\triangle G^0=-\triangle H^0-T\triangle S^0\)

(b)

G - H - TS

(c)

\(\triangle G^0\) = -2.303 RT log K_eq

(d)

\(\triangle S-\triangle H/T\)

Assertion: Permanent hardness of water is removed by treatment with washing soda.
Reason: Washing soda reacts with soluble calcium and magnesium chlorides and sulphates in hard water to form insoluble carbonates

(a)

Both assertion and reason are true and reason is the correct explanation of assertion.

(b)

Both assertion and reason are true but reason is not the correct explanation of assertion.

(c)

Assertion is true but reason is false

(d)

Both assertion and reason are false

Which one of the following is not an extensive property?

(a)

Density

(b)

Molarity

(c)

Molality

(d)

Mole

The most electro negative element possess the electronic configuration______.

(a)

ns² np²

(b)

ns² np⁴

(c)

ns² np⁵

(d)

ns² np³

10.

Match the list-I and list-Il using the correct code given below the list.

List-I		List-II
A	Manufacture of soap	1	Na₂CO₃.10H₂O
B	Mild antiseptic	2	Liquid Na metal
C	Softening of hard water	3	NaOH
D	Coolant in nuclear reactor	4	NaHCO₃

(a)

A	B	C	D
4	3	2	1

(b)

A	B	C	D
3	4	1	2

(c)

A	B	C	D
2	1	3	4

(d)

A	B	C	D
1	2	4	3

11.

How many grams are contained in 1 gram atom of Na?

(a)

13g

(b)

1 g

(c)

23 g

(d)

1/23g

12.

The ideal gas equation is ____________.

(a)

PV = RT for 1 mole

(b)

P₁V₁ = P₂V₂

(c)

\(\frac{P}{T}=R\)

(d)

P = P₁ + P₂ + P₃

13.

The oxidation number of Cr in K₂Cr₂O₇ is ___________.

(a)

(b)

(c)

(d)

14.

Correctly match the list-I and list-II using the code given below the list

List-I		List-I
A	Beryllium	1	Sacrificial anode
B	Calcium	2	X-ray tube radiation window
C	Magnesium	3	Scavenger to remove oxygen in TV
D	Barium	4	Getter in vacuum tubes

(a)

A	B	C	D
4	2	3	1

(b)

A	B	C	D
2	4	1	3

(c)

A	B	C	D
3	1	4	2

(d)

A	B	C	D
1	3	2	4

15.

Which one of the following is not a redox reaction?

(a)

Rusting of iron

(b)

Extraction of metal Na

(c)

Electroplating

(d)

Aluminothermic process

16.

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

17.

How many H₂O molecules are there in a snowflake weighing 1 mg?

(a)

3.35 x 10¹⁹

(b)

6.023 x 10²³

(c)

3.35 x 10^-19

(d)

100

18.

Copper chloride produces __________ colour in fire works

(a)

red

(b)

green

(c)

blue

(d)

yellow

19.

Consider the following statements.
(i) Superoxides of alkali metals are diamagnetic.
(ii) Superoxides of alkali metals are blue in colour.
(iii) Superoxides of alkali metals are paramagnetic.
Which of the above statements is/are not correct?

(a)

(i) only

(b)

(ii) only

(c)

(iii) only

(d)

(i) and (ii)

20.

Match the list-I and list-II correctly using the code given below the list.

List-I	List-II
A. Principal quantum number	1.represents the directional orientation of orbital
B. Azimuthal quantum number	2.represents the spin of the electron
C. Magnetic quantum number	3.represents the main shell
D. Spin quantum number	4.represents the sub shell

(a)

A	B	C	D
3	4	1	2

(b)

A	B	C	D
4	2	3	1

(c)

A	B	C	D
2	1	4	3

(d)

A	B	C	D
1	3	2	4

21.

Consider the following statements.
(i) H₂O₂is a powerful oxidising agent.
(ii) H₂O₂ is stored in dark coloured bottles.
(iii) H₂O₂is used as moderator in nuclear reactors.
Which of the above statements is/are not correct

(a)

(i) only

(b)

(i) and (ii)

(c)

(iii) only

(d)

(i), (ii) and (iii)

22.

Match the List-I and List-II using the correct code given below the list.

List-I	List-II
A. Hydrogenation of unsaturated vegetable oils	1. Rocket fuel
B. Calcium hydride	2. Welding of metals
C. Liquid hydrogen	3. Desiccant
D. Atomic hydrogen	4. Margarine

(a)

A	B	C	D
4	3	1	2

(b)

A	B	C	D
3	4	2	1

(c)

A	B	C	D
1	3	4	2

(d)

A	B	C	D
2	1	4	3

23.

Which one of the metal is used to convert para hydrogen into ortho hydrogen?

(a)

Copper

(b)

Aluminium

(c)

Sodium

(d)

Platinum

24.

The mass of one molecule of HI in grams is ____________.

(a)

2.125\(\times\)10^-22

(b)

128

(c)

127

(d)

6.02\(\times\)10^-23

25.

The pressure-volume work for an ideal gas can be calculated by using the expression.
\(w=-\int _{ { v }_{ i } }^{ { v }_{ f } }{ { P }_{ ext }.{ dV }_{ t } } \)
The work can also be calculated from the PV plot by using the area. Under the curve within the specified limits. When an ideal gas is compressed
(a) reversibly or
(b) irreversibly from volume V_i to V_f, choose the correct option _____

(a)

w (reversible) = W (irreversible)

(b)

w (reversible) < W (irreversible)

(c)

W (reversible) > W (irreversible)

(d)

W (reversible) = W (irreversible)

26.

In general, for an exothermic reaction to be spontaneous:

(a)

temp should be high

(b)

temp should be zero

(c)

temp should be low

(d)

temp has no effect

27.

The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated is __________

(a)

(b)

(c)

(d)

28.

If system moves from ordered state to disordered state, its entropy ___________

(a)

Decreases

(b)

Increases

(c)

Become zero

(d)

Increases then decreases

29.

The unit of entropy is ____________

(a)

J K^-1 mol^-1

(b)

J mol^-1

(c)

J K mol^-1

(d)

J^-1K^-1

30.

The final temperature of an engine whose initial temperature is 400K and having efficiency 25%

(a)

200K

(b)

400K

(c)

300K

(d)

450K

31.

The temperature at which the volume of the gas becomes zero is ________

(a)

0^oC

(b)

0 K

(c)

0 F

(d)

none of these

32.

The equivalent mass of potassium permanganate in alkaline medium is:
MnO₄^- + 2H₂O + 3e^-\(\rightarrow\) MnO₂ + 4OH^-

(a)

31.6

(b)

52.7

(c)

(d)

None of these

33.

Assertion: Number of radial and angular nodes for 3p orbital are 1, 1 respectively.
Reason: Number of radial and angular nodes depends only on principal quantum number.

(a)

both assertion and reason are true and reason is the correct explanation of assertion.

(b)

both assertion and reason are true but reason is not the correct explanation of assertion.

(c)

assertion is true but reason is false

(d)

both assertion and reason are false

34.

Which is true about cyclic process?

(a)

ΔU=0; ΔH=0

(b)

ΔU>0; ΔH<0

(c)

ΔH=0; ΔU<0

(d)

ΔU=0; ΔH<0

35.

In an exothermic reaction, heat is evolved and system loses heat to the surroundings. For such system
(i) q_p will be negative
(ii) Δ_rH will be positive
(iii) q_p will be positive
(iv) Δ_rH will be negative

(a)

(i), (ii)

(b)

(iii), (iv)

(c)

(i) & (iv)

(d)

(ii) & (iii)

36.

Thermodynamics does not deal with ____

(a)

the feasibility of a chemical reaction

(b)

energy changes involved in chemical reaction

(c)

the extent to which a chemical reaction process

(d)

the rate at which a reaction occurs

37.

Which is insoluble in water?

(a)

CaF₂

(b)

CaCl2

(c)

HgCl₂

(d)

Ca(NO₃)₂

38.

Match the list-I with list-II and select the correct answer using the code given below the lists.

List-I		List-II
A	Molecular formula	1	Completely consumed
B	Stoichiometric Equation	2	Left unreacted
C	Limiting reactant	3	n x Empirical formula
D	Excess reagent	4	Balanced equation

(a)

A	B	C	D
3	4	2	1

(b)

A	B	C	D
3	4	1	2

(c)

A	B	C	D
4	3	1	2

(d)

A	B	C	D
4	3	1	2

39.

Which set of elements shows positive electron gain enthalpy?

(a)

He,N,O

(b)

Ne,N,Cl

(c)

O,Cl,F

(d)

N,He,Ne

40.

Which of the following property has no unit?

(a)

ionisation energy

(b)

electronegativity

(c)

electron affinity

(d)

atomic radius

41.

With respect to chlorine, hydrogen will be __________

(a)

Electropositive

(b)

Electronegative

(c)

Neutral

(d)

None of these

42.

A example of covalent hydride is ____________

(a)

CaH₂

(b)

CH₄

(c)

TiH

(d)

all the above

43.

Which mixture of gases at room temperature does not obey Dalton's law of partial pressure?

(a)

NO₂ and O₂

(b)

SO₂ and SO₃

(c)

CO and CO₂

(d)

NH₃ and HCI

44.

In a closed room of 1000 m³ a perfume bottle is opened up. The room develops smell. This is due to which property of gases _____________

(a)

Viscosity

(b)

Density

(c)

Diffusion

(d)

None

45.

Which hydroxide decomposes on heating?

(a)

NaOH

(b)

RbOH

(c)

KOH

(d)

LiOH.

46.

If E_n = -313.6/n2,If the value of E_i = -34.84 to which value 'n' corresponds __________

(a)

(b)

(c)

(d)

47.

Match the list I with List II and select the correct answer using. the code given below the lists.

List I		List II
A	Metalloid	1	Cerium
B	Noble gas	2	Nobelium
C	Trans uranium element	3	Arsenic
D	Lanthanide	4	Argon

(a)

A	B	C	D
1	3	2	4

(b)

A	B	C	D
4	2	1	3

(c)

A	B	C	D
3	4	2	1

(d)

A	B	C	D
2	1	4	3

48.

The number of elements in the first period of the modern periodic table is _____

(a)

(b)

(c)

(d)

49.

J. J. Thomson's cathode ray experiment revealed that atoms consist of _____________

(a)

electrons

(b)

protons

(c)

neutrons

(d)

photons

50.

The law that relates the pressure and volume of gases is ________

(a)

Boyle's

(b)

Charles

(c)

Dalton

(d)

none of the above

51.

There are _____ periods in the periodic table.

(a)

(b)

(c)

(d)

52.

Consider the following statements according to modern periodic table.
(i) Modern periodic table contains 18 vertical columns and 7 horizontal rows.
(ii) The elements after uranium are called transuranium elements
(iii) The 17th group elements are called chalcogens
(iv) The elements of Groups 13 to 18 are called p-block elements.
which of the following statement(s) given above is/are correct.

(a)

(i), (iii) & (iv)

(b)

(i), (ii) & (iii)

(c)

(i), (ii) & (iv)

(d)

all the 4 statements

53.

In which of the following compounds does hydrogen has an oxidation state of -1?

(a)

CH₄

(b)

NH₃

(c)

HCl

(d)

CaH₂

54.

Molar heat of vaporization of a liquid is 4.8 kJ mol^-1. If the entropy change is 16 J mol^-1 K^-1, the boiling point of the liquid is ____________

(a)

323 K

(b)

27° C

(c)

164 K

(d)

0.3 K

55.

In an isothermal reversible compression of an ideal gas the sign of q, ΔS and w are respectively _______________

(a)

+, -, -

(b)

-, +, -

(c)

+, -, +

(d)

-, -, +

56.

Match the list I with List II and select the correct answer using. the code given below the lists.

List I		List II
A	Chancourtois	1	Addition of synthetic elements
B	Rang	2	Families and periods Long form
C	Glenn Seaborg	3	Modern periodic law
D	Moseley	4	First periodic law

(a)

A	B	C	D
1	3	2	4

(b)

A	B	C	D
4	2	1	3

(c)

A	B	C	D
3	4	1	2

(d)

A	B	C	D
2	1	4	3

57.

Given that C_(g)+ O_2(g)⟶ CO_2(g)ΔH^o =-akJ; 2CO_(g)+O_2(g) ⟶ 2CO_2(g)ΔH^o= -bkJ; Calculate the AHo for the reaction C_(g)+ 1/2O_2(g)⟶ CO_(g) ______________

(a)

\(\frac{b+2a}{2}\)

(b)

2a-b

(c)

\(\frac{2a-b}{2}\)

(d)

\(\frac{b-2a}{2}\)

58.

The enthalpies of formation of Al₂O₃ and Cr₂O₃are -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2Al + Cr₂O₃ ⟶ 2Cr + Al₂O₃ is _______________

(a)

- 1365 kJ

(b)

2730 kJ

(c)

- 2730 kJ

(d)

- 462 kJ

59.

Hydrogen is used in _________

(a)

hydrogenation of oils

(b)

fuel cells

(c)

gas bags for air ships

(d)

all the above

60.

C(diamond) ) ⟶ C(graphite), ΔH = -ve, this indicates that ___________

(a)

graphite is more stable than diamond

(b)

graphite has more energy than diamond

(c)

both are equally stable

(d)

stability cannot be predicted

61.

In an adiabatic process, which of the following is true ?

(a)

q = w

(b)

q = 0

(c)

ΔE = q

(d)

PΔV= 0

62.

Among the following the least thermally stable is ___________

(a)

K₂CO₃

(b)

Na₂CO₃

(c)

BaCO₃

(d)

Li₂CO₃

63.

The ratio of de Broglie wavelengths of a deuterium atom to that of an \(\alpha\) - particle, when the velocity of the former is five times greater than that of later, is ____________

(a)

(b)

0.2

(c)

2.5

(d)

0.4

64.

The product obtained as a result of a reaction of nitrogen with CaC₂ is ___________

(a)

Ca(CN)₃

(b)

CaN₂

(c)

CaCN₂

(d)

Ca₃N₂

65.

In which process, fused sodium hydroxide is electrolysed for extraction of sodium ?

(a)

Castner's process

(b)

Cyanide process

(c)

Down process

(d)

All of these

66.

Find the wrong statement

(a)

sodium metal is used in organic qualitative analysis

(b)

sodium carbonate is soluble in water and it is used in inorganic qualitative analysis

(c)

potassium carbonate can be prepared by solvay process

(d)

potassium bicarbonate is acidic salt

67.

RbO₂ is _____________

(a)

superoxide and paramagnetic

(b)

peroxide and diamagnetic

(c)

superoxide and diamagnetic

(d)

peroxide and paramagnetic

68.

If temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes _________

(a)

(b)

(c)

(d)

69.

Consider the following statements
i) Atmospheric pressure is less at the top of a mountain than at sea level
ii) Gases are much more compressible than solids or liquids
iii) When the atmospheric pressure increases the height of the mercury column rises.
Select the correct statement

(a)

I and II

(b)

II and III

(c)

I and III

(d)

I, II and III

70.

Use of hot air balloon in sports at meteorological observation is an application of __________________

(a)

Boyle's law

(b)

Newton's law

(c)

Kelvin's law

(d)

Brown's law

71.

Which one of the following is used as a standard for atomic mass?

(a)

₆C¹²

(b)

₇C¹²

(c)

₆C¹³

(d)

₆C¹⁴

72.

Which of the following compound(s) has /have a percentage of carbon same as that in ethylene (C₂H₄)?

(a)

propene

(b)

ethyne

(c)

benzene

(d)

ethane

73.

Two 22.4 litre containers A and B contains 8 g of O₂ and 8 g of SO₂ respectively at 273 K and 1 atm pressure, then ______.

(a)

Number of molecules in A and B are same

(b)

Number of molecules in B is more than that in A.

(c)

The ratio between the number of molecules in A= to number of molecules in B is 2:1

(d)

Number of molecules in B is three times greater than the number of molecules in A

74.

The equivalent mass of ferrous oxalate is __________.

(a)

\(\frac { molar\ mass\ of\ ferrous \ oxalate }{ 1 } \)

(b)

\(\frac { molar\ mass\ of\ ferrous \ oxalate }{ 2 } \)

(c)

\(\frac { molar\ mass\ of\ ferrous \ oxalate }{ 3 } \)

(d)

None of these

75.

If uncertainty in position and momentum are equal, then minimum uncertainty in velocity is _________

(a)

\(\frac { 1 }{ m } \sqrt { \frac { h }{ \pi } } \)

(b)

\( \sqrt { \frac { h }{ \pi } } \)

(c)

\(\frac { 1 }{ 2m } \sqrt { \frac { h }{ \pi } } \)

(d)

\( { \frac { h }{4\pi } } \)

76.

Electron density in the yz plane of 3d_xy orbital is ___________

(a)

zero

(b)

0.50

(c)

0.75

(d)

0.90

77.

How many electrons in an atom with atomic number 105 can have (n + 1) = 8 ?

(a)

(b)

(c)

(d)

unpredictable

78.

Consider the following sets of quantum numbers:

	n	l	m	s
(i)	3	0	0	+\(\frac { 1 }{ 2 } \)
(ii)	2	2	1	-\(\frac { 1 }{ 2 } \)
(iii)	4	3	-2	+\(\frac { 1 }{ 2 } \)
(iv)	1	0	-1	+\(\frac { 1 }{ 2 } \)
(v)	3	4	3	-\(\frac { 1 }{ 2 } \)

Which of the following sets of quantum number is not possible?

(a)

(i), (ii), (iii) and (iv)

(b)

(ii), (iv) and (v)

(c)

(i) and (iii) .

(d)

(ii), (iii) and (iv)

79.

The value of universal gas constant depends upon __________

(a)

Temperature of the gas

(b)

Volume of the gas

(c)

Number of moles of the gas

(d)

units of Pressure and volume.

80.

Which of the following is the correct expression for the equation of state of van der Waals gas?

(a)

\(\left( P+\frac { a }{ { n }^{ 2 }{ V }^{ 2 } } \right) (V-nb)=nRT\)

(b)

\(\left( P+\frac { na }{ { n }^{ 2 }{ V }^{ 2 } } \right) (V-nb)=nRT\)

(c)

\(\left( P+\frac { { an }^{ 2 } }{ { V }^{ 2 } } \right) (V-nb)=nRT\)

(d)

\(\left( \frac { P+{ n }^{ 2 }{ a }^{ 2 } }{ { V }^{ 2 } } \right) (V-ab)=nRT\)

81.

Rate of diffusion of a gas is ________

(a)

directly proportional to its density

(b)

directly proportional to its molecular weight

(c)

directly proportional to its square root of its molecular weight

(d)

inversely proportional to the square root of its molecular weight

82.

7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is ________.

(a)

(b)

N₂O

(c)

(d)

CO₂

83.

When 22.4 litres of H₂(g) is mixed with 11.2 litres of Cl₂(g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to ______.

(a)

2 moles of HCl (g)

(b)

0.5 moles of HCl (g)

(c)

1.5 moles of HCl (g)

(d)

1 moles of HCl (g)

84.

The maximum number of electrons in a sub shell is given by the expression _____________

(a)

2n²

(b)

2l + 1

(c)

4l + 2

(d)

none of these

85.

Two electrons occupying the same orbital are distinguished by ___________

(a)

azimuthal quantum number

(b)

spin quantum number

(c)

magnetic quantum number

(d)

orbital quantum number

86.

Based on equation E = \(-2.178\times { 10 }^{ -18 }J\left( \frac { { Z }^{ 2 } }{ { n }^{ 2 } } \right) \)certain conclusions are written. Which of them is not correct?

(a)

Equation can be used to calculate the change in energy when the electron changes orbit

(b)

For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit

(c)

The negative sign in equation simply means that the energy of electron bound to the nucleus is lower than it would be if the electrons were at the infinite distance from the nucleus.

(d)

Larger the value of n, the larger is the orbit radius.

87.

The hybridisation of oxygen atom is H₂O and H₂O₂ are, respectively __________

(a)

sp and Sp³

(b)

sp and sp

(c)

Sp and Sp²

(d)

Sp³and Sp³

88.

Volume strength of 1.5 N H₂O₂ is _____________

(a)

1.5

(b)

4.5

(c)

16.8

(d)

8.4

89.

For decolorisation of 1 mole of acidified KMnO₄, the moles of H₂O₂ required is ___________

(a)

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

(b)

\(\frac{3}{2}\)

(c)

\(\frac{5}{2}\)

(d)

\(\frac{7}{2}\)

90.

When hydrogen peroxide is shaken with an acidified solution of potassium dichromate in presence of ether, the ethereal layer turns blue due to the formation of _____________

(a)

Cr₂O₃

(b)

\({ CrO }_{ 4 }^{ 2- }\)

(c)

CrO(O₂)₂

(d)

none of these

91.

Zeolite used to soften hardness of water is hydrated _____________

(a)

Sodium aluminium silicate

(b)

Calcium aluminium silicate

(c)

Zinc aluminium borate

(d)

Lithium aluminium hydride

92.

Tritium nucleus contains _____________

(a)

1 p+0 n

(b)

2 p+1 n

(c)

1 p + 2 n

(d)

none of these

93.

Ionic hydrides are formed by _____________

(a)

halogens

(b)

halogens

(c)

inert gases

(d)

group one elements

94.

Which one of the following statements is incorrect with regard to ortho and para dihydrogen ?

(a)

They are nuclear spin isomers

(b)

Ortho isomer has zero nuclear spin whereas the para isomer has one nuclear spin

(c)

The para isomer is favoured at low temperatures

(d)

The thermal conductivity of the para isomer is 50% greater than that of the ortho isomer

95.

The energies E₁and E₂ of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths ie \(\lambda \)₁ and\(\lambda \)₂ will be ___________

(a)

\(\frac { { \lambda }_{ 1 } }{ { \lambda }_{ 2 } } =1\)

(b)

\({ \lambda }_{ 1 }=2{ \lambda }_{ 2 }\)

(c)

\({ \lambda }_{ 1 }=\sqrt { 25\times 50{ \lambda }_{ 2 } } \)

(d)

\(2{ \lambda }_{ 1 }={ \lambda }_{ 2 }\)

Assertion and reason

4 x 2 = 8

96.

Assertion (A): The orbitals having equal energy are known as degenerate orbitals.
Reason (R): The three 2p orbitals are degenerate is the presence of external magnetic field.
Codes:
(a) Both A and R are true and R is the correct explanation of A
(b) Both A and R are true but R is not the correct explanation of A
(c) A is true but R is false
(d) Both A and R are false

(a)

Both A and R are true and R is the correct explanation of A

(b)

Both A and R are true but R is not the correct explanation of A

(c)

A is true but R is false

(d)

Both A and R are false

97.

Assertion : Alkaline earth metals are harder than alkali metals
Reason : Atomic radii of alkaline earth metals are smaller than corresponding alkali metals "in the same periods of periodic table
Codes:
a) both assertion and reason are true and reason is the correct explanation of assertion
b) both assertion and reason are true but reason is not the correct explanation of assertion
c) assertion is true but reason is false
d) both assertion and reason are false

(a)

Both assertion and reason are true and reason is the correct explanation for assertion.

(b)

Both assertion and reason are true but reason is not the correct explanation for assertion

(c)

Assertion is true but reason is false

(d)

Both assertion and reason are false

98.

Assertion : BeSO₄ is soluble in water while BaSO₄ is not
Reason : Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.
(a) both assertion and reason are true and reason is the correct explanation of assertion
(b) both assertion and reason are true but reason is not the correct explanation of assertion
(c) both assertion and reason are false.
(d) Both assertion and reason are false

(a)

both assertion and reason are true and reason is the correct explanation of assertion

(b)

both assertion and reason are true but reason is not the correct explanation of assertion

(c)

assertion is true but reason is false

(d)

both assertion and reason are false.

99.

Assertion: Two mole of glucose contains 12.044 x 10²³ molecules of glucose
Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 10²²
(a) both assertion and reason are true and the reason is the correct explanation of assertion
(b) both assertion and reason are true but reason is not the correct explanation of assertion
(c) assertion is true but reason is false
(d) both assertion and reason are false

(a)

both assertion and reason are true and the reason is the correct explanation of assertion

(b)

both assertion and reason are true but the reason is not the correct explanation of assertion

(c)

an assertion is true but reason is false

(d)

both assertion and reason are false

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Answers Key:

Multiple Choice Question

95 x 1 = 95

(b)
575 kJ mol^-1

(a)
Y > Z > X > A

(d)
Ca < Al < C < O < F

(b)
Na < Al < Mg < Si < P

(a)
Both assertion and reason are true and reason is the correct explanation of assertion.

(d)
Mole

10.

(b)

A B C D

3 4 1 2

11.

12.

(a)
PV = RT for 1 mole

13.

(b)
+6

14.

(b)

A B C D

2 4 1 3

15.

(a)
Rusting of iron

16.

(b)
directly proportional to its absolute temperature

17.

(a)
3.35 x 10¹⁹

18.

19.

(a)
(i) only

20.

(a)

A B C D

3 4 1 2

21.

22.

(a)

A B C D

4 3 1 2

23.

(d)
Platinum

24.

(a)
2.125\(\times\)10^-22

25.

(b)
w (reversible) < W (irreversible)

26.

27.

28.

(b)
Increases

29.

(a)
J K^-1 mol^-1

30.

31.

(b)
0 K

32.

(b)
52.7

33.

34.

(a)
ΔU=0; ΔH=0

35.

36.

(d)
the rate at which a reaction occurs

37.

(a)
CaF₂

38.

(b)

A B C D

3 4 1 2

39.

(d)
N,He,Ne

40.

(b)
electronegativity

41.

(a)
Electropositive

42.

(b)
CH₄

43.

(d)
NH₃ and HCI

44.

45.

(d)
LiOH.

46.

(b)
3

47.

48.

(a)
2

49.

(a)
electrons

50.

(a)
Boyle's

51.

(b)
7

52.

53.

(d)
CaH₂

54.

(b)
27° C

55.

(d)
-, -, +

56.

(b)

A B C D

4 2 1 3

57.

(d)
\(\frac{b-2a}{2}\)

58.

(d)
- 462 kJ

59.

(d)
all the above

60.

(a)
graphite is more stable than diamond

61.

(b)
q = 0

62.

(d)
Li₂CO₃

63.

(d)
0.4

64.

65.

(a)
Castner's process

66.

67.

(a)
superoxide and paramagnetic

68.

69.

(d)
I, II and III

70.

(a)
Boyle's law

71.

(a)
₆C¹²

72.

(a)
propene

73.

74.

75.

76.

(a)
zero

77.

(b)
17

78.

(b)
(ii), (iv) and (v)

79.

(d)
units of Pressure and volume.

80.

81.

(d)
inversely proportional to the square root of its molecular weight

82.

(a)
NO

83.

(d)
1 moles of HCl (g)

84.

85.

(b)
spin quantum number

86.

(b)
For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit

87.