Solve 54 MCQ'S PHYSICAL chemistry for B.Sc. first year students

This article will help you to test basic knowledge of physical chemistry. We have provides 54 multiple choice questions with 

Solve 54 MCQ'S PHYSICAL chemistry for B.Sc. first year students 

 1. Gaseous state has

A. Definite shape and definite volume

B. No definite shape and no definite volume

C. Definite shape but no definite volume

D. No definite shape but definite volume

2. Which of the following is not an assumption of the kinetic molecular theory of gas?

A. Attractive forces of the gas molecules are sufficiently strong

B. Molecules of the gas have constant and random motion

C. Volume of gaseous molecules are negligible

D. average kinetic energy of gas molecules is directly proportional to the absolute temperature of the gas

3. In case of an ideal gas compressibility factor is

A. One

B. Two

C. Three

D. Zero

4. van der Waal’s equation is for

A. ideal gas

B. real gas

C. perfect gas

D. compressed gas

5. The critical temperature of the water is 647 K, which means

A. The boiling point of water is 647 K

B. At 647 K liquid water is in equilibrium with solid ice

C. Below 647 K gas never does liquify

D. Above 647 K gas never does liquify

6. The pressure exerted by the vapor of liquid above it at equilibrium is known as

A. Critical pressure

B. Vapour pressure

C. Osmotic pressure

D. Absolute pressure

7. The effect of temperature on viscosity is

A. Viscosity Increase with temperature

B. Viscosity and temperature are not related

C. Viscosity decreases with temperature

D. Random effect of temperature on viscosity

8. Metallotropic liquid crystals consist of

A. Only organic molecules

B. Only inorganic molecules

C. Both organic and inorganic molecules

D. Only metals

9. Acetic acid adsorbed on charcoal. Here acetic acid is

A. Adsorbent

B. Adsorbate

C. Solute

D. Solvent

10. In chemical adsorption, adsorption is

A. Several molecular layer thick

B. Multimolecular layer thick

C. Two or more molecular layer thick

D. Unimolecular layer thick

11. In case of negative catalysis, In presence of a catalyst,

A. The rate of reaction increases

B. The rate of reaction decreases or slowdowns or stopped the reaction.

C. The rate of reaction increases and decreases

D. The rate of reaction increases only

12. In the manufacture of ammonia by Haber’s process, the catalyst is

A. MnO₂

B. Fe

C. Pt

D. Ni

13. A colloidal system in which a solid is dispersed in a liquid is called

A. Foam

B. Sol

C. Gel

D. Emulsion

14. Milk is an example of

A. Foam

B. Sol

C. Gel

D. Emulsion

15. Zigzag motion of the particles of the colloidal solution is called

A. Tyndall effect

B. Scattering

C. Brownian movement

D. Electrophoresis

16. Angular wave function describes

A. Shape and direction of orbital

B. Size of orbital

C. Length of orbital

D. Hybridization of orbital

17. Wave nature of electron was demonstrated by

A. Schrodinger

B. de Broglie

C. Davisson

D. Heisenberg

18. In the Schrodinger equation the symbol 'ψ' (psi) represents the

A. the wavelength of the wave

B. the amplitude of the wave

C. frequency of the wave

D. the energy of the wave

19. The radius of the first orbit of a Hydrogen atom is _____ angstrom

A. 0.529

B. 0.0529

C. 5.29

D. 0

20. Which of the following electromagnetic radiations have wavelengths shorter than visible light

A. micro-waves

B. X-rays

C. radio waves

D. infrared

21. Compare to 800 nm light, 400 nm light has

A. higher frequency

B. lower frequency

C. higher energy and lower energy

D. higher frequency and higher energy

22. The evidence for wave-particle duality of light is

A. the photograph effect

B. the photoelectric effect

C. the electron diffraction

D. both a and c

23. The de-Broglie wavelength of an electron with the kinetic energy of 1.00 eV is

A. 1.23 nm

B. 12.3 pm

C. 0.123 nm

D. 28.7 pm

24. The first series in the Hydrogen spectrum is

A. Pfund

B. Balmer

C. Lyman

D. Brackett

25. For the Paschen series of Hydrogen spectrum the value of n1 is

A. 0

B. 1

C. 2

D. 3

26. The wavenumber associated with a wave having wavelength 580 nm is

A. 17241 cm⁻¹

B. 17.241 cm⁻¹

C. 580 cm⁻¹

D. 58.1 cm⁻¹

27. Thermodynamics is applicable to ………

A. microscopic systems only

B. macroscopic systems only

C. homogenous systems only

D. heterogeneous systems only

28. A thermos flask is an example of …….

A. isolated system

B. closed system

C. homogenous system

D. open system

29. A closed system is one which cannot transfer matter but transfer ……. to and from its Surrounding.

A. Heat

B. work

C. energy

D. all of these

30. Which of the following sets of properties constitute intensive properties?

A. temperature, pressure, and volume

B. mass, density, and volume

C. density, pressure, and temperature

D. internal energy, density, and pressure

31. The efficiency of Carnot’s engine is one if

A. the temperature of the source is 0 K

B. the temperature of the sink is 0 K

C. the temperature of sink is 0 °C

D. the temperature of the source is 0 °C

32. The efficiency of a Carnot machine operates between 300 K and 400 K is

A. 1.333

B. 0.75

C. 0.25

D. 100

33. One mole of an ideal gas at 300 K is expanded isothermally from 1-liter volume to 10-liter volume, E for this process is… ( R =2 cal K⁻¹ mol ⁻¹)

A. 300 cal

B. 604.87 J

C. 1208 J

D. 0 Cal

34. The work done when 1 mole of an ideal gas expands reversibly and isothermally from 5 atm to 1 atm at 300 K is,

A. -4015 J

B. +4015 J

C. -1500 J

D. 0 J

35. Osmosis is

A. reversible process

B. spontaneous process

C. adiabatic process

D. exothermic process

36. The units’ erg, joule, and calorie are interconvertible, which of the following is incorrect?

A. 10 7 ergs = 1 Joule

B. 4.184 J = 1 cal

C. 1 Joule = 0.2390 cal

D. 1erg = 4.184 cal.

37. The value of N is----

A. 6.022 x 10²³

B. 2.66 x 10²³

C. 12.1 x 10²³

D. 22400

38. The quantitative aspect dealing with ------------- and the --------------- relationship between the reactant and product is called stoichiometry.

A. Atomic weight, atomic mass

B. Mass, volume

C. Molecular weight, molecular volume

D. Gram mole, volume

39. Strength in gm/lit =

A. 2 x vapor density

B. Normality x equivalent weight

C. volume x 22.4

D. 2 x atomic weight

40. Substance such as -------------- is used as a primary standard substance

A. CaCO₃, acetic acid

B. NaOH, Salicylic acid

C. KOH, HCl

D. Na₂CO₃, benzoic acid

41. When concentration of solution is expressed in ppm, it means 1 part in ---------- parts per solution.

A. 10³

B. 10⁶

C. 10⁹

D. 10¹⁵

42. Equivalent weight of Na₂CO₃ is 53. When we dissolve 0.53 gm of Na₂CO₃ in 100 ml .water itis -------- N solution

A. 1

B. 0.1

C. 0.01

D. 0.53

43. The process or reaction in which there is the loss of electron is called -----------

A. Oxidizing agent

B. Reduction

C. De-electronation

D. Electronation

44. In the reaction, 2 Mg + O₂ ------>

A. Mg₂

B. 4MgO

C. MgO

D. 2MgO

45. The oxidation number of S in metallic sulfides is ----------

A. + 6

B. + 5

C. + 3

D. - 2

46. The bond in NaCl is ---

A. Ionic bond

B. Covalent bond

C. Co-ordinate bond

D. Semi polar bond

47. Covalent bond is formed by -------

A. Loss of electrons

B. Gain of electron

C. sharing of electrons

D. None of the above

48. In a double bond connecting two atoms, there is a sharing of --------

A. 2 electron

B. 4 electron

C. 1 electron

D. 5 electron

49. How many Pi bonds are formed in nitrogen molecules?

A. 0

B. 1

C. 2

D. 3

50. Which one of the following molecules shows non-polar covalent bonding?

A. H2

B. HCl

C. HF

D. H2O

51. Which of the following contains a coordinate covalent bond?

A. NH₄⁺

B. HCl

C. H₂O

D. CCl₄

52. Non-metals generally form ------

A. Ionic bond

B. Covalent bond

C. Co-ordinate bond

D. Semi-polar bond

53. Which one of the following is axial overlapping?

A. s-px

B. py-py

C. px-px

D. none of these

54. Metal atoms are held together by a different kind of bond is called ------

A. ionic solids

B. covalent solids

C. molecular solids

D. metallic bond