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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. Amorphous substances possess

No definite heat of fusion

Sharp melting points

Sharp B.P.

Definite heat of fusion

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

Dipole – induced dipole forces

Dipole – dipole forces

London dispersion forces

Ion – dipole forces

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

Molecules of hydrogen chloride gas

Molecules of solid iodine

Atoms if helium in gaseous state at high temperature

Molecules of water in liquids state

4. Evaporation causes

High temperature

Vapour pressure

Cooling

High pressure

5. Hydrogen bonding is involved in

All

Biological molecule

Solubility

Detergent

6. Ice is _________ crystal

Ionic

Molecular

Covalent

Metallic

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

Pyramidal structure of NH₃

Very small size of nitrogen

Ione pair of electrons present on nitrogen

Enhanced electronegative character of nitrogen

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

Water droplets

Dust

Water vapour

Ice

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

The boiling decreases and the freezing point decreases.

The boiling point increases and the freezing point decreases.

The boiling point increases and the freezing point increases.

The boiling point decreases and the freezing point increases.

10. 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?

2.2

.82

1.1

.63

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

Some mass is converted into energy

Energy is liberated

Energy is absorbed

Neither liberated nor absorbed

12. Van der Waal’s forces exist in

Polar compounds

Covalent

All types of atoms and molecules

Non-polar

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

Surface tension in less

None of these

Consumes less soap

Surface tension is more

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

Adhesive forces

Viscosity

Cohesive forces

Surface tension

15. Which of the following statements in incorrect?

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

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.

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

18°C

14.5°C

12.8°C

100°C

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

Of dipole-dipole interactions in CH₄.

HF is more polarizable

CH₄ is polar

Of hydrogen bonding in HF

18. Water has high boiling point which is due to

High specific heat

Weak dissociation

H – bonding between its molecules

High electric constant

19. Water has maximum density at

4⁰C

0⁰C

100⁰C

2⁰C

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

None of these

Remains unchanged

Decrease

Increase

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

Dipole-induced dipole interactions increase with molecular size

Dipole-dipole interactions increase with molecular size

Dispersion interactions increase with molecular size

Polarity increases with molecular size

22. 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

23. 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

Water

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

Glass

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

11.7 kJ

3.09 kJ

79.1 kJ

20.9 kJ

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

Metallic bonding

Covalent bonding

Ionic bonding

Hydrogen bonding

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

HCI

HBr

27. Vapour pressure of H₂O at 100C° is

355 mm Hg

55 mm of Hg

760 mm of Hg

1489 mm Hg

28. The strength of dipole-dipole forces depends upon

Electro negativity difference

Both A & B

Electro positivity difference

Distance between atoms

29. Evaporation of water in shade is

Fast

Slow

None of these

Faster

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

Empty space present in the structure of ice

Change of bond angles

Cubic structure of ice

Change of bond length

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

Sublimation

Evaporation

Crystallization

Vaporization

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

765 torr

Any value of pressure

Between 760 torr and 1200 torr

Between 200 torr and 760 torr

33. Stronger the intermolecular forces

Greater the Vapour pressure

May be smaller or greater

None

Lower the Vapour pressure

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

Na(g) → N²⁺ (g) + +¯

Na(s) → N²⁺ (g) + e¯

Na(s) → N²⁺ (g) + 2e¯

Na(g) → N²⁺ (g) + e¯

35. Molecular iodine would be most soluble in:

Alcohol

Vinegar (acetic acid and water)

Water

Carbon tetrachloride

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

London forces

Hydrogen bonding

Ion dipole forces

Dipole-dipole forces

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

They are formed when atoms gain electrons

They are formed only in metals

They are also known as anions

They are larger than the atom from which they were formed

38. Molar heat of vaporization of water is

40.7 cal/mole

40.7 KJ/mole

40.7 J/mole

40.7 Kcal/mole

39. The maximum hydrogen bonding is in

Diethyl ether

Benzene

Ethanol

Water

40. Water has maximum density at

2C°

0C°

4C°

100C°

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

23,352

158,130

15,813

7,000

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

Cubic structure of ice

Change of bond angles

Empty space presenting structure of ice

Change of bond length

43. London dispersion forces are also called

Dipole-dipole forces

Ion-dipole forces

Instantaneous dipole induced dipole forces

Dipole-induced dipole forces

44. 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 has the lowest molecular weight

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

The water molecule is lighter than the other two molecules.

Water is less polar than hydrogen sulfide and hydrogen selenide.

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

Ion-dipole forces

Instantaneous dipole – induced dipole forces

Dipole – dipole forces

Dipole – induced dipole forces

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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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