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

Water droplets

Water vapour

Ice

Dust

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

Empty space presenting structure of ice

Change of bond length

Cubic structure of ice

Change of bond angles

3. Evaporation of water in shade is

Faster

None of these

Fast

Slow

4. 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 decreases.

The boiling point decreases and the freezing point increases.

The boiling point increases and the freezing point increases.

The boiling decreases and the freezing point decreases.

5. Stronger the intermolecular forces

May be smaller or greater

None

Greater the Vapour pressure

Lower the Vapour pressure

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

Molecules of water in liquids state

Molecules of hydrogen chloride gas

Molecules of solid iodine

Atoms if helium in gaseous state at high temperature

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

Viscosity

Cohesive forces

Adhesive forces

Surface tension

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

They are formed when atoms gain electrons

They are larger than the atom from which they were formed

They are formed only in metals

They are also known as anions

9. Which of the following statements in incorrect?

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

The boiling point of noble gases increases down the group

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.

10. Vapour pressure of H₂O at 100C° is

355 mm Hg

55 mm of Hg

1489 mm Hg

760 mm of Hg

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

Ionic bonding

Metallic bonding

Covalent bonding

Hydrogen bonding

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

Ion dipole forces

Hydrogen bonding

London forces

Dipole-dipole forces

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

HBr

HCI

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

Na(s) → N²⁺ (g) + 2e¯

Na(s) → N²⁺ (g) + e¯

Na(g) → N²⁺ (g) + e¯

Na(g) → N²⁺ (g) + +¯

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

Of hydrogen bonding in HF.

Of dipole-dipole interactions in CH₄.

HF is more polarizable

CH₄ is polar.

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

15,813

7,000

158,130

23,352

17. 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

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

14.5°C

18°C

100°C

12.8°C

19. Water has maximum density at

4C°

100C°

0C°

2C°

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

Crystallization

Evaporation

Sublimation

Vaporization

21. Ice is _________ crystal

Molecular

Metallic

Ionic

Covalent

22. 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

Polarity increases with molecular size

Dispersion interactions increase with molecular size

23. Water has maximum density at

0⁰C

4⁰C

100⁰C

2⁰C

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

Between 200 torr and 760 torr

Between 760 torr and 1200 torr

765 torr

Any value of pressure

25. 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

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26. 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

Dipole – dipole forces

Ion-dipole forces

27. 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?

Water

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

None of these

Glass

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

Consumes less soap

None of these

Surface tension in less

Surface tension is more

29. Hydrogen bonding is involved in

All

Detergent

Solubility

Biological molecule

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

Neither liberated nor absorbed

Some mass is converted into energy

Energy is liberated

Energy is absorbed

31. Van der Waal’s forces exist in

Polar compounds

All types of atoms and molecules

Covalent

Non-polar

32. Evaporation causes

Cooling

High pressure

High temperature

Vapour pressure

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

Cubic structure of ice

Empty space present in the structure of ice

Change of bond angles

Change of bond length

34. Molar heat of vaporization of water is

40.7 Kcal/mole

40.7 KJ/mole

40.7 J/mole

40.7 cal/mole

35. The strength of dipole-dipole forces depends upon

Electro negativity difference

Both A & B

Electro positivity difference

Distance between atoms

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

Dipole – dipole forces

Dipole – induced dipole forces

London dispersion forces

Ion – dipole forces

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

20.9 kJ

3.09 kJ

79.1 kJ

11.7 kJ

38. Water has high boiling point which is due to

High electric constant

H – bonding between its molecules

Weak dissociation

High specific heat

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

Remains unchanged

None of these

Decrease

Increase

40. 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?

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

Water has the lowest molecular weight

Water is less polar than hydrogen sulfide and hydrogen selenide.

The water molecule is lighter than the other two molecules.

41. Molecular iodine would be most soluble in:

Alcohol

Carbon tetrachloride

Water

Vinegar (acetic acid and water)

42. London dispersion forces are also called

Dipole-induced dipole forces

Dipole-dipole forces

Ion-dipole forces

Instantaneous dipole induced dipole forces

43. Amorphous substances possess

Sharp melting points

No definite heat of fusion

Definite heat of fusion

Sharp B.P.

44. The maximum hydrogen bonding is in

Diethyl ether

Ethanol

Water

Benzene

45. 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?

1.1

.82

.63

2.2

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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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