ECAT Pre Engineering Chemistry Chapter 4 MCQ Test With Answer

Question # 1

Evaporation of water is possible at:

Above 100°C A
0°C B
100°C C
At all temperature D

Question # 2

Which of the following liquids has low vapour pressure at 25⁰C

Diethyl ether A
Acetone B
Water C
Ethyl alochol D

Question # 3

Hydrocarbon molecules with large chain lengths experience

Weaker attractive forces A
Stronger attractive forces B
Repulsive forces C
No attractive forces D

Question # 4

Chloroform and acetone are soluble in each other due to:

Instantaneous dipole interactions. A
Dipole-dipole interactions. B
Inter molecular hydrogen bonding. C
All of above D

Question # 5

Hydrocarbon molecule with large chain lengths experience:

Weaker attractive forces A
Stronger attractive forces B
Repulsive forces C
No attractive forces D

Question # 6

Hydrogen bonding is present in one of the following pairs:

NH₃ A
H₂O B
HF C
All of above D

Question # 7

Debye forces are present in one of the following pairs

Na⁺ion and water A
Argon and water B
Argon and Na⁺ion C
Ne and Water D

Question # 8

Which of the following liquids has low vapor pressure at 25°C:

Diethyl ether A
Acetone. B
Water. C
Ethyl alcohol. D

Question # 9

Rate of evaporation and rate of condensation at equilibrium

Become very low A
Become very high B
Become equal C
Can never be equal D

Question # 10

Which one of the following is weakest inter molecular force?

Dipole induced dipole forces A
Ionic dipole forces B
Electrostatic forces b/w ions C
Dipole dipole forces D

Question # 11

Trend of boiling point of halogens from fluorine to Iodine is that it

Decreases A
Is negligible B
Increases C
Remains constant D

Question # 12

The boiling point of NH₃is maximum among the hydrides of group V elements due to

Enhanced electronegative character of Nitrogen A
Pyramidal structure of NH₃ B
Very small size of Nitrogen C
Enhanced electropositive character of Nitrogen D

Question # 13

A liquid on evaporation causes:

Heating effect. A
Cooling effect. B
Suffocation . C
All of above D

Question # 14

Ionic Solids are characterized by

Low melting points A
Good conductivity in solid state B
High vapour pressure C
Solubility in polar solvents D

Question # 15

The strongest forces are

Debye forces A
London dispersion forces B
Dipole-dipole attraction C
Hydrogen D

Question # 16

The strongest forces are:

Debye froces A
London dispersion B
Dipole-dipole attraction C
Hydrogen bonding D

Question # 17

The boiling point of NH_{3 is maximum among the hydrides of group V elementsdue to:}

Enhanced electronegative character of Nitrogen A
Pyramidal structure of NH3 B
Very small size of Nitrogen. C
Enhanced electropositive character of Nitrogen D

Question # 18

Hydrogen bonding is present between the molecules of

NH₃ A
H₂O B
HF C
All of above D

Question # 19

The molecules of CO_{2 in dry ice from the :}

Ionic crystals A
Coverlet crystals B
Molecular crystals C
Any type of crystals D

Question # 20

In a group on going downward, polarizability generally:

Decreases A
Increases B
Remain constant C
Negligible D

Question # 21

The only forces are London dispersion forces among the

Atoms of He in gaseous state at high temperature A
Molecules of water in liquid state B
Molecules of solid I₂ C
Molecular of hydrochloric acid gas D

Question # 22

At sea level and at 100°C the vapor pressure of water in an open system is:

1000 mm Hg A
760 mm Hg B
730 mm Hg C
670 mm Hg D

Question # 23

The inter-molecular forces in liquids are:

Negligible A
Very weak B
Very strong C
Reasonably strong D

Question # 24

The molecules of CO₂in dry ice from the

Ionic crystalls A
Covalent crystals B
Molecular crystals C
Any type of crystal D

Question # 25

Amorphous solids

Have sharp melting point A
Undergo clean cleavage when cut with knife B
Have perfect arrangement of atoms C
Can possesses small regions of orderly arrangement of atoms D

Question # 26

The density of water decreases, When it is freezed at 0°C

Change of bond length A
Change of bond angles B
Cubic structure of ice C
Empty spaces present in the structure of ice D

Question # 27

Heat of vapourization for liquids with strong dipole-dipole forces will have

Negligible Values A
Reasonably high values B
Very high values C
very low values D

Question # 28

Chloroform and acetone are soluble in each other due to

Instantaneous dipole interactions A
Dipole-dipole interactions B
Intermolecular hydrogen bonding C
All of above D

Question # 29

The density of water decreases, when it is freezed at 0^oC because of

Change of bond lengths A
Change of bond angles B
Cubic structure of ice C
Empty spaces present in the structure of Ice D

Question # 30

H₂S is a gas which H₂O is liquid at room temperature. it is due to

Less intermolecular forces in water A
Covalent bond in H-O in water molecule B
Hydrogen bonding in water molecules C
Ionic characters in water molecules D

Sr.#	Question	Answer
1	Chloroform and acetone are soluble in each other due to:	A. Instantaneous dipole interactions. B. Dipole-dipole interactions. C. Inter molecular hydrogen bonding. D. All of above
2	The intermolecular forces in liquids are	A. Negligible B. Very weak C. Very strong D. Reasonably strong
3	The boiling point of NH_{3 is maximum among the hydrides of group V elementsdue to:}	A. Enhanced electronegative character of Nitrogen B. Pyramidal structure of NH3 C. Very small size of Nitrogen. D. Enhanced electropositive character of Nitrogen
4	Force of attraction b/w atoms of He is :	A. London dispersion forces B. Hydrogen bonding C. Coordinate covalent bond D. Covalent bond
5	Debye forces are present in on of the following pairs:	A. Na+ion and water B. Argon and water C. Argon and Na+ion D. Ne and water
6	London dispersion forces are alos called:	A. Hydrogen bonding. B. Debye forces C. Van der Waal's forces D. Instantaneous dipole-induced dipole forces.
7	Polypeptide chains are coiled about one another into a spiral by:	A. Ionic bonds B. Covalent bonds C. Van der Waal's forces D. Hydrogen bonds
8	Force of attraction between atoms of He is	A. London dispersion forces B. Hydrogen bondign C. Coordinate covalent bond D. Covalent bond
9	Amorphous solids:	A. Have a sharp melting point B. Undergo clean cleavage when cut with knife C. Have a perfect arrangement of atoms D. Can possesses small regions of orderly arrangement of atoms
10	A liquid on evaporation causes:	A. Heating effect. B. Cooling effect. C. Suffocation . D. All of above

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ECAT Pre Engineering Chemistry Chapter 4 MCQ Test With Answer

MCQ's Test For ECAT Chemistry Chapter 4 Liquids & Solids

ECAT Chemistry Chapter 4 Liquids & Solids

Evaporation of water is possible at:

Which of the following liquids has low vapour pressure at 250C

Hydrocarbon molecules with large chain lengths experience

Chloroform and acetone are soluble in each other due to:

Hydrocarbon molecule with large chain lengths experience:

Hydrogen bonding is present in one of the following pairs:

Debye forces are present in one of the following pairs

Which of the following liquids has low vapor pressure at 25°C:

Rate of evaporation and rate of condensation at equilibrium

Which one of the following is weakest inter molecular force?

Trend of boiling point of halogens from fluorine to Iodine is that it

The boiling point of NH3is maximum among the hydrides of group V elements due to

A liquid on evaporation causes:

Ionic Solids are characterized by

The strongest forces are

The strongest forces are:

The boiling point of NH3 is maximum among the hydrides of group V elementsdue to:

Hydrogen bonding is present between the molecules of

The molecules of CO2 in dry ice from the :

In a group on going downward, polarizability generally:

The only forces are London dispersion forces among the

At sea level and at 100°C the vapor pressure of water in an open system is:

The inter-molecular forces in liquids are:

The molecules of CO2in dry ice from the

Amorphous solids

The density of water decreases, When it is freezed at 0°C

Heat of vapourization for liquids with strong dipole-dipole forces will have

Chloroform and acetone are soluble in each other due to

The density of water decreases, when it is freezed at 0oC because of

H2S is a gas which H2O is liquid at room temperature. it is due to

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