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ECAT Chemistry Liquids Test Online

Mustansar KhanLast Updated: April 19, 2025

Chemistry Liquids MCQS Online Test

ECAT Chemistry Liquids Chapter Online Test

Total Questions:	45
Time Allowed:	20 Minutes
Total Marks:	45
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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ECAT Chemistry Liquids Test

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Chemistry

1. Which one of the following is not a form of chemical bonding?

Metallic bonding

Covalent bonding

Ionic bonding

Hydrogen bonding

2. Stronger the intermolecular forces

Lower the Vapour pressure

Greater the Vapour pressure

May be smaller or greater

None

3. What do we see on the surface of the glass containing ice-chilled water?

Dust

Water droplets

Water vapour

Ice

4. Molecular iodine would be most soluble in:

Alcohol

Water

Vinegar (acetic acid and water)

Carbon tetrachloride

5. When water freezes at 0c its density decreases due to

Empty space presenting structure of ice

Change of bond angles

Cubic structure of ice

Change of bond length

6. Evaporation of water in shade is

None of these

Fast

Faster

Slow

7. London dispersion forces are also called

Dipole-dipole forces

Instantaneous dipole induced dipole forces

Dipole-induced dipole forces

Ion-dipole forces

8. The strength of dipole-dipole forces depends upon

Electro negativity difference

Both A & B

Electro positivity difference

Distance between atoms

9. The quantity of heat required to convert one mole of liquid into its vapors at its boiling point is called heat of

Crystallization

Vaporization

Sublimation

Evaporation

10. In order to mention B.P of H₂O at 110°C, the external pressure should be

Any value of pressure

Between 200 torr and 760 torr

Between 760 torr and 1200 torr

765 torr

11. Which of the following statements in incorrect?

The layers in graphite are held together by van der Waals forces

H₂O has higher than expected b.p. because of intermolecular Van der Waals forces.

The boiling point of noble gases increases down the group

The greater the number of electrons in a molecule, the greater the van der Waals forces

12. The attracted forces which are created due to repulsion of electronic cloud of the molecules are

Dipole – induced dipole forces

Instantaneous dipole – induced dipole forces

Ion-dipole forces

Dipole – dipole forces

13. Vapour pressure of H₂O at 100C° is

760 mm of Hg

355 mm Hg

1489 mm Hg

55 mm of Hg

14. An 8.29 g sample of calcium carbonate [CaCO₃(s)] absorbs 50.3 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. What is the specific heat of calcium carbonate?

.63

.82

1.1

2.2

15. Molar heat of vaporization of water is

40.7 KJ/mole

40.7 cal/mole

40.7 J/mole

40.7 Kcal/mole

16. Evaporation causes

Cooling

Vapour pressure

High pressure

High temperature

17. When the external pressure is 101.3 kPa torr, water will boil at what temperature?

12.8°C

14.5°C

18°C

100°C

18. It is easy to wash clothes in hot water because its

Surface tension is more

None of these

Consumes less soap

Surface tension in less

19. On mixing the salt in water, the surface tension of water will

Increase

Decrease

Remains unchanged

None of these

20. NH₃ shows a maximum boiling point among the hydrides of V – A group elements due to

Enhanced electronegative character of nitrogen

Pyramidal structure of NH₃

Very small size of nitrogen

Ione pair of electrons present on nitrogen

21. Water has high boiling point which is due to

H – bonding between its molecules

Weak dissociation

High specific heat

High electric constant

22. How many joules of heat are absorbed when 70.0 grams of water is completely vaporized at its boiling point?

158,130

7,000

23,352

15,813

23. Water has maximum density at

4C°

100C°

0C°

2C°

24. Water has maximum density at

4⁰C

100⁰C

2⁰C

0⁰C

25. g point of water is about 200°C higher than one would predict from the boiling points of hydrogen sulfide and hydrogen selenide. One may explain this apparent anomaly by which of the following?

Water is less polar than hydrogen sulfide and hydrogen selenide.

The water molecule is lighter than the other two molecules.

The intermolecular attractive forces are much greater in water than in hydrogen sulfide and hydrogen selenide.

Water has the lowest molecular weight

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26. Which one of the following exhibits intermolecular hydrogen bonding?

HCI

HBr

27. A solute is most likely to be highly soluble in a solvent of the solute is ________ and the solvent is ________.

Of dipole-dipole interactions in CH₄.

Of hydrogen bonding in HF.

CH₄ is polar.

HF is more polarizable

28. Van der Waal’s forces exist in

Polar compounds

All types of atoms and molecules

Covalent

Non-polar

29. Amorphous substances possess

Sharp B.P.

No definite heat of fusion

Definite heat of fusion

Sharp melting points

30. Hydrogen bonding is involved in

All

Solubility

Detergent

Biological molecule

31. Which of the following equations represents the 2nd ionization energy of Na?

Na(g) → N²⁺ (g) + +¯

Na(s) → N²⁺ (g) + 2e¯

Na(s) → N²⁺ (g) + e¯

Na(g) → N²⁺ (g) + e¯

32. Rising of an wetting liquid in a capillary tube is due to

Viscosity

Cohesive forces

Adhesive forces

Surface tension

33. The boiling point increases down the zero group element due to

Dipole-dipole forces

London forces

Ion dipole forces

Hydrogen bonding

34. Two droplets merge with each other and forms a large droplet. In this process

Energy is liberated

Energy is absorbed

Neither liberated nor absorbed

Some mass is converted into energy

35. How are the boiling and freezing point of a sample of water affected when salt is dissolved in the water?

The boiling point increases and the freezing point increases.

The boiling point decreases and the freezing point increases.

The boiling point increases and the freezing point decreases.

The boiling decreases and the freezing point decreases.

36. What amount of heat (in kJ) is required to melt 35.0 g of ice at 0°C?

3.09 kJ

20.9 kJ

11.7 kJ

79.1 kJ

37. The forces present between the ions and water molecules are called

Ion – dipole forces

London dispersion forces

Dipole – dipole forces

Dipole – induced dipole forces

38. The maximum hydrogen bonding is in

Benzene

Water

Diethyl ether

Ethanol

39. Which one of the following statements about negative ions is incorrect?

They are also known as anions

They are larger than the atom from which they were formed

They are formed when atoms gain electrons

They are formed only in metals

40. Ice is _________ crystal

Molecular

Covalent

Ionic

Metallic

41. Water has a specific heat of 4.184 J/g deg while glass (Pyrex) has a specific heat of 0.780 J/g deg. If 10.0 J of heat is added to 1.00 g of each of these, which will experience the larger increase of temperature?

None of these

They both will experience the same change in temperature since only the amount of a substance relates to the increase in temperature

Glass

Water

42. London dispersion forces are the only force present among the

Molecules of hydrogen chloride gas

Molecules of water in liquids state

Atoms if helium in gaseous state at high temperature

Molecules of solid iodine

43. The boiling point of CH₄ is much lower than that of HF. This is because:

Of dipole-dipole interactions in CH₄.

Of hydrogen bonding in HF

HF is more polarizable

CH₄ is polar

44. When water freezes at 0⁰C its density decreases due to

Cubic structure of ice

Change of bond length

Empty space present in the structure of ice

Change of bond angles

45. At room temperature, F₂, and Cl₂ are gases, Br₂ is a liquid, and I₂ is a solid. This is because:

Polarity increases with molecular size

Dispersion interactions increase with molecular size

Dipole-dipole interactions increase with molecular size

Dipole-induced dipole interactions increase with molecular size

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Mustansar KhanLast Updated: April 19, 2025

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ECAT Chemistry Liquids Test Online

Chemistry Liquids MCQS Online Test

ECAT Chemistry Liquids Chapter Online Test

ECAT Chemistry Liquids Test

Chemistry

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Chemistry Liquids MCQS Online Test

ECAT Chemistry Liquids Chapter Online Test

ECAT Chemistry Liquids Test

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Mustansar Khan

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