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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.
Test Helpful For:	ECAT Entry Test Chemistry Online Test Interview Questions about Chemisttry All Universities Entrance Test Recruitments Tests

ECAT Chemistry Liquids Test

Page 1 of 2

Chemistry

1. The maximum hydrogen bonding is in

Benzene

Ethanol

Water

Diethyl ether

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

100°C

12.8°C

18°C

14.5°C

3. 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 decreases and the freezing point decreases.

The boiling point increases and the freezing point increases.

4. The strength of dipole-dipole forces depends upon

Electro negativity difference

Electro positivity difference

Both A & B

Distance between atoms

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

Dipole – induced dipole forces

Dipole – dipole forces

Ion-dipole forces

Instantaneous dipole – induced dipole forces

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

Evaporation

Crystallization

Sublimation

Vaporization

7. Water has maximum density at

100⁰C

4⁰C

0⁰C

2⁰C

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

23,352

7,000

15,813

158,130

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

Dipole-dipole interactions increase with molecular size

Dispersion interactions increase with molecular size

Polarity increases with molecular size

Dipole-induced dipole interactions increase with molecular size

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

Viscosity

Cohesive forces

Adhesive forces

Surface tension

11. Hydrogen bonding is involved in

Biological molecule

All

Detergent

Solubility

12. Molecular iodine would be most soluble in:

Carbon tetrachloride

Vinegar (acetic acid and water)

Alcohol

Water

13. 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.

Water has the lowest molecular weight

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.

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

Water droplets

Water vapour

Dust

Ice

15. Amorphous substances possess

Sharp melting points

Sharp B.P.

No definite heat of fusion

Definite heat of fusion

16. Stronger the intermolecular forces

Lower the Vapour pressure

Greater the Vapour pressure

None

May be smaller or greater

17. London dispersion forces are also called

Dipole-induced dipole forces

Dipole-dipole forces

Instantaneous dipole induced dipole forces

Ion-dipole forces

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

Hydrogen bonding

Metallic bonding

Ionic bonding

Covalent bonding

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

HF is more polarizable

Of hydrogen bonding in HF.

CH₄ is polar.

Of dipole-dipole interactions in CH₄.

20. Water has high boiling point which is due to

Weak dissociation

High specific heat

High electric constant

H – bonding between its molecules

21. Evaporation of water in shade is

None of these

Faster

Fast

Slow

22. 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

2.2

.63

.82

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

11.7 kJ

20.9 kJ

79.1 kJ

3.09 kJ

24. Evaporation causes

High pressure

Cooling

High temperature

Vapour pressure

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

765 torr

Between 200 torr and 760 torr

Any value of pressure

Between 760 torr and 1200 torr

Page 2 of 2

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

Consumes less soap

None of these

Surface tension is more

Surface tension in less

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

HBr

HCI

28. 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?

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

Water

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

Na(s) → N²⁺ (g) + e¯

Na(s) → N²⁺ (g) + 2e¯

Na(g) → N²⁺ (g) + +¯

Na(g) → N²⁺ (g) + e¯

30. Molar heat of vaporization of water is

40.7 KJ/mole

40.7 Kcal/mole

40.7 J/mole

40.7 cal/mole

31. Ice is _________ crystal

Metallic

Molecular

Covalent

Ionic

32. Van der Waal’s forces exist in

Polar compounds

Non-polar

Covalent

All types of atoms and molecules

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

Ion – dipole forces

London dispersion forces

Dipole – dipole forces

Dipole – induced dipole forces

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

Increase

Remains unchanged

Decrease

None of these

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

Of hydrogen bonding in HF

Of dipole-dipole interactions in CH₄.

CH₄ is polar

HF is more polarizable

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

Very small size of nitrogen

Ione pair of electrons present on nitrogen

Enhanced electronegative character of nitrogen

Pyramidal structure of NH₃

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

Dipole-dipole forces

Hydrogen bonding

Ion dipole forces

London forces

38. Water has maximum density at

4C°

2C°

0C°

100C°

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

Energy is liberated

Neither liberated nor absorbed

Some mass is converted into energy

Energy is absorbed

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

Change of bond length

Change of bond angles

Cubic structure of ice

Empty space presenting structure of ice

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

Change of bond angles

Cubic structure of ice

Empty space present in the structure of ice

Change of bond length

42. Vapour pressure of H₂O at 100C° is

1489 mm Hg

55 mm of Hg

760 mm of Hg

355 mm Hg

43. Which of the following statements in incorrect?

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.

The boiling point of noble gases increases down the group

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

They are formed only in metals

They are formed when atoms gain electrons

They are larger than the atom from which they were formed

They are also known as anions

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

Molecules of hydrogen chloride gas

Atoms if helium in gaseous state at high temperature

Molecules of water in liquids state

Molecules of solid iodine

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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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Mustansar Khan

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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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