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Questions:

Multiple Choice Question

58 x 1 = 58

Statement-I: The magnetic moment of parahydrogen is zero.
Statement-II: The spins of two hydrogen atoms in para H2 molecule neutralise each other.

(a)

Statements-I and II are correct and Statement-II is the correct explanation of statement-I.

(b)

Statements-I and II are correct but Statement-II is not the correct explanation of statement- I.

(c)

Statement-I is correct but Statement-II is wrong.

(d)

Statement-I is wrong but Statement-II is correct.

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

List-I	List-II
A. Cyclic process	1. ΔU=q-PΔV
B. Adiabatic process	2. ΔU=q_v
C. Isobaric process	3. q=-w
D. Isochoric process	4. ΔU=w

(a)

A	B	C	D
4	2	3	1

(b)

A	B	C	D
3	4	1	2

(c)

A	B	C	D
2	1	4	3

(d)

A	B	C	D
1	3	2	4

Which one is the correct unit for entropy?

(a)

KJ mol

(b)

JK^-1 mol

(c)

JK^-1 mol^-1

(d)

KJ mol^-1

A gas can expand from 100 ml to 250 ml under a constant pressure of 2 atm. The work done by the gas is _________

(a)

-30.39 J

(b)

25 J

(c)

5 kJ

(d)

16 J

The process in which there is no exchange of heat between the system and surrounding is called ______

(a)

Adiabatic process

(b)

Isothermal process

(c)

Isobaric process

(d)

Isochoric process

The most electro negative element possess the electronic configuration______.

(a)

ns² np²

(b)

ns² np⁴

(c)

ns² np⁵

(d)

ns² np³

Which of the following is the most powerful oxidising agent?

(a)

KMnO₄

(b)

K₂Cr₂O₇

(c)

O₃

(d)

H₂O₂

The compressibility factor for an ideal gas is ______________.

(a)

1.5

(b)

(c)

(d)

\(\propto \)

How many moles of Hydrogen atoms are present in 1 mole of C₂H₆?

(a)

18 moles

(b)

6 moles

(c)

3 moles

(d)

1 mole

10.

Which one of the following is used in purification of sugar and as drying agent?

(a)

Ca(OH)₂

(b)

MgSO₄.7H₂O

(c)

CaSO₄.2H₂O

(d)

CaO

11.

Consider the following statements
(i) Empirical formula shows the actual number of atoms of different elements in one molecule of the compound.
(ii) Ozone is a diatomic molecule.
(iii) Gases are easily compressible.
Which of the above statement is/are not correct?

(a)

(i), (ii), (iii)

(b)

(i) & (ii)

(c)

(ii) & (iii)

(d)

(iii) only

12.

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)

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

13.

Among all the elements which one has the highest value of electronegativity?

(a)

Chlorine

(b)

Bromine

(c)

Fluorine

(d)

Iodine

14.

Which of the following metal is not in liquid state?

(a)

Gallium

(b)

Aluminium

(c)

Mercury

(d)

Caesium

15.

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)

16.

Which one of the following is the smallest atom?

(a)

Francium

(b)

Rubidium

(c)

Lithium

(d)

Sodium

17.

Which metal does not liberate H₂ gas from dilute aqueous hydrochloric acid at 298 K?

(a)

(b)

(c)

(d)

18.

Which of the following elements were unknown at that time of Mendeleev?

(a)

Na, Mg

(b)

Fe, CO

(c)

K, Cu

(d)

Ga, Ge

19.

Which of the following is used as desiccants to remove moisture from organic solvents?

(a)

Calcium hydride

(b)

LiAIH₄

(c)

Sodium boro hydride

(d)

Sodium hydride

20.

Which of the following is used in illumination of wrist watches?

(a)

Phosphorous

(b)

Radon

(c)

Tritium

(d)

Deuterium

21.

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

(a)

Copper

(b)

Aluminium

(c)

Sodium

(d)

Platinum

22.

Which one of the following element mostly present in the sun and the stars?

(a)

Hydrogen

(b)

Lithium

(c)

Helium

(d)

Beryllium

23.

Two containers A and B of the equal volume contain 6g of each O₂ and SO₂ at 300K and 1atm. Then ____________

(a)

No. of molecules in A is less than that in B

(b)

No.of molecules inA is more than that inB

(c)

No. of molecules in A and B are same

(d)

none of these

24.

The amount of heat evolved when 500 cm³ of 0.1 M hydrochloric add is mixed with 200 cm³ of 0.2 M sodium hydroxide solution is _________

(a)

-57.1 kJ

(b)

+ 57.1 kJ

(c)

2.284 kJ

(d)

-2.284 kJ

25.

The heat absorbed at constant volume is equal to the system's change in:

(a)

enthalpy

(b)

entropy

(c)

internal energy

(d)

free energy

26.

The number of d- electrons in Fe⁺² (Z = 26) is not equal to the number of electrons in which one of the following?

(a)

d-electron in Fe (Z = 26)

(b)

p-electron in Ne (Z = 10)

(c)

s-electron in Mg (Z = 12)

(d)

p-electron in CI (Z = 17)

27.

If the de Broglie wavelength of a particle of mass (m) is 100 times its velocity, then its value in terms of its mass (m) and Planck's constant (h) is ___________

(a)

\(\frac{1}{10}\sqrt{\frac{m}{h}}\)

(b)

\({10}\sqrt{\frac{h}{m}}\)

(c)

\(\frac{1}{10}\sqrt{\frac{h}{m}}\)

(d)

\({10}\sqrt{\frac{m}{h}}\)

28.

The net work done by the system _____________

(a)

w-P\(\Delta\)V

(b)

w+P\(\Delta\)V

(c)

-w+P\(\Delta\)V

(d)

-w-P\(\Delta\)V

29.

Which of the following process is feasible at all temperatures?

(a)

\(\Delta\)H > 0, \(\Delta\)S > 0

(b)

\(\Delta\)H > 0, \(\Delta\)S < 0

(c)

\(\Delta\)H < 0. \(\Delta\)S>0

(d)

\(\Delta\)H < 0, \(\Delta\)S < 0

30.

Equal volumes of He, O₂ and SO₂ are taken in a closed container. The ratio of the partial pressures of gases He, O₂ and SO₂ would be __________

(a)

1 : 2 : 8

(b)

8 : 16 : 1

(c)

1 : 4 : 16

(d)

16 : 2 :1

31.

The enthalpy and entropy change for a chemical reactions are -5.3 x 10³ cal and 4.7 cal K^-1 respectively. Predict the nature of the reaction at 298 k.

(a)

Non feasible

(b)

Reversible

(c)

Non-spontaneous

(d)

Spontaneous

32.

Change in enthalpy is ___________

(a)

Heat absorbed at constant pressure

(b)

The total energy change at constant pressure and temperature

(c)

Equal to change in internal energy at constant volume

(d)

All the above

33.

In a compression process, P_ext is ___________

(a)

(P_int+ dP)

(b)

(P_int- dP)

(c)

(dP-P_int)

(d)

(-P_int+dP)

34.

The correct statements is / are :
(i) BeCl₂ is a covalent compound
(ii) BeCl₂ can form dimer
(iii) BeCl₂ is an electron deficient molecule
(iv) The hybridisation of Be in BeCl₂ is Sp²

(a)

(i) and (iii)

(b)

(i), (ii) and (iii)

(c)

(i) and (iv)

(d)

(ii), (iii) and (iv)

35.

Which among the following is not a state function?

(a)

Pressure

(b)

Volume

(c)

Temperature

(d)

Work

36.

Gypsum is _________

(a)

CaSO₄.H₂O

(b)

CaSO₄.1/2H₂O

(c)

CaSO₄.1/4H₂O

(d)

CaSO₄.2H₂O

37.

Pick the incorrect statement about the factors affecting ionization energy

(a)

More is the shielding of valence electrons more is the ionization energy

(b)

Ionization enthalpy ∝ effective nuclear charge

(c)

Half filled or fully filled atomic orbitals have high ionization energy

(d)

Larger is the atomic radii lower is ionization energy

38.

The compound in which mass percentage of carbon is 75% and that of hydrogen is 25% is _____________.

(a)

C₂H₆

(b)

C₂H₂

(c)

CH₄

(d)

C₂H₄

39.

Give an example of molecule in which the ratio of the molecular formula is six times the empirical formula.

(a)

C₆H₁₂O₆

(b)

CH₂O

(c)

CH₄

(d)

NA₂CO₃

40.

The polarising power of Mg is almost same as ___________

(a)

(b)

(c)

(d)

41.

The liquefaction behaviour of temporary gases like CO₂ approaches that of N₂, O₂ (permanent gases) as we go _______

(a)

below critical temperature

(b)

above critical temperature

(c)

below absolute zero

(d)

above absolute zero

42.

Electronic configuration of species M²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ and its atomic weight is 56. The number of neutrons in the nucleus of species M is _______________

(a)

(b)

(c)

(d)

43.

Isotopes have ______________

(a)

same number of protons

(b)

same number of neutrons

(c)

different number of electrons

(d)

different atomic number.

44.

The atomic number of an element is 17 and its mass number is 37. The number of protons, electrons and neutrons present in the neutral atom are __________

(a)

17,37,20

(b)

20,17,37

(c)

17,17,20

(d)

17,20,17

(e)

37,20,17.

45.

Why Cs and K are used as electrodes in photoelectric cells ___________

(a)

Due to their less ionisation energy

(b)

Due to high ionisation energy

(c)

Due to diagonal relationship

(d)

None of these

46.

The partial pressure of dry gas is ____________

(a)

greater than that of wet gas

(b)

lesser than that of wet gas

(c)

equal to that of wet gas

(d)

none of these

47.

Find the incorrect statement.

(a)

Smallest atom of periodic table is He

(b)

p-block elements are metals, nonmetals and metalloids

(c)

Noble gases have 8 valence electrons except He

(d)

Valence electron and valency is same for group I

48.

Elements which generally exhibit multiple oxidation states and whose ions are usually coloured are ___________

(a)

metalloids

(b)

transition elements

(c)

non-metals

(d)

gases

49.

The element with atomic number 57 belongs to _____

(a)

s-block

(b)

p-block

(c)

d-block

(d)

f-block

50.

Hydrogen accepts an electron to attain the inert gas configuration. In this way it resembles __________

(a)

chalcogens

(b)

halogens

(c)

transition metals

(d)

alkali metals

51.

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)

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

52.

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)

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

53.

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

54.

The electronic configuration of copper is ______

(a)

[Ar]4s²3d⁹

(b)

[Ar]4s¹3d¹⁰

(c)

[Ar]4s⁰3d¹⁰

(d)

All

55.

Consider the following statements and pick the incorrect statement(s).
1. Schrodinger wave equation is used to determine the probability of finding a electron at a given point in space.
2. The energy of a electron at infinity is positive
3. Angular momentum quantum number gives information regarding subshells.

(a)

1&3

(b)

only 1

(c)

only 2

(d)

1,2 & 3

56.

The oxidation number of oxygen in O₂ is__________

(a)

(b)

(c)

(d)

-2

57.

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

58.

Carbon forms two oxides, namely carbon monoxide and carbon dioxide. The equivalent mass of which element remains constant ?

(a)

Carbon

(b)

Oxygen

(c)

Both carbon and oxygen

(d)

Neither carbon nor oxygen

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Answers Key:

Multiple Choice Question

58 x 1 = 58

(a)
Statements-I and II are correct and Statement-II is the correct explanation of statement-I.

(b)

A B C D

3 4 1 2

(a)
-30.39 J

(d)
Isochoric process

(a)
KMnO₄

(b)
6 moles

10.

(d)
CaO

11.

(b)
(i) & (ii)

12.

(b)
PV = RT

13.

14.

(b)
Aluminium

15.

(a)
(i) only

16.

17.

(d)
Cu

18.

(d)
Ga, Ge

19.

(a)
Calcium hydride

20.

21.

(d)
Platinum

22.

(a)
Hydrogen

23.

(b)
No.of molecules inA is more than that inB

24.

25.

26.

(d)
p-electron in CI (Z = 17)

27.

(b)
\({10}\sqrt{\frac{h}{m}}\)

28.

(d)
-w-P\(\Delta\)V

29.

30.

(a)
1 : 2 : 8

31.

(d)
Spontaneous

32.

(a)
Heat absorbed at constant pressure

33.

(a)
(P_int+ dP)

34.

(b)
(i), (ii) and (iii)

35.

(d)
Work

36.

(d)
CaSO₄.2H₂O

37.

(a)
More is the shielding of valence electrons more is the ionization energy

38.

39.

(a)
C₆H₁₂O₆

40.

(a)
Li

41.

(b)
above critical temperature

42.

43.

(a)
same number of protons

44.

45.

(a)
Due to their less ionisation energy

46.

(b)
lesser than that of wet gas

47.

(a)
Smallest atom of periodic table is He

48.

(b)
transition elements

49.

50.

(b)
halogens

51.

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

52.

53.

(a)
NO

54.

(b)
[Ar]4s¹3d¹⁰

55.

56.

(a)
0

57.

(b)
spin quantum number

58.

(b)
Oxygen

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Questions:

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