1. The number of significant figures in 0.06900 is
A. 2
B. 3
C. 4
D. 5
2. One mole of a substance contains
A. 6.022 × 10²³ atoms/molecules
B. 1.6 × 10⁻¹⁹ particles
C. 12 g of carbon-12
D. Both A and C
3. The empirical formula of a compound with molecular formula C₆H₁₂O₆ is
A. CH₂O
B. C₃H₆O₃
C. C₆H₁₂O₆
D. CHO
4. The law of definite proportions was given by
A. Dalton
B. Proust
C. Avogadro
D. Gay-Lussac
5. 18 g of water contains
A. 1 mole of H₂O
B. 2 moles of H atoms
C. 1 mole of O atoms
D. All of the above
6. The molar mass of CaCO₃ is
A. 50 g/mol
B. 74 g/mol
C. 100 g/mol
D. 114 g/mol
7. In which of the following is the number of molecules maximum at STP?
A. 22.4 L of CO₂
B. 11.2 L of NH₃
C. 44.8 L of N₂
D. 5.6 L of O₂
8. The limiting reagent in a reaction is the one which
A. is completely consumed first
B. has maximum mass
C. produces maximum product
D. is left unreacted
9. The percentage composition of oxygen in H₂O is approximately
A. 11.1%
B. 88.9%
C. 50%
D. 33.3%
10. Avogadro's law is related to
A. equal volumes of gases at same T & P
B. equal number of molecules
C. Both A and B
D. None of the above
11. The maximum number of electrons in n = 3 shell is
A. 8
B. 18
C. 32
D. 2
12. The shape of orbital with azimuthal quantum number l = 1 is
A. spherical
B. dumbbell
C. double dumbbell
D. clover leaf
13. Quantum number which determines the orientation of orbital is
A. n
B. l
C. m
D. s
14. The de Broglie wavelength is inversely proportional to
A. velocity
B. momentum
C. mass
D. Both B and C
15. Bohr's model is applicable to
A. H atom only
B. H-like species
C. multi-electron atoms
D. Both A and B
16. The uncertainty in position and momentum is given by
A. Heisenberg principle
B. Bohr postulate
C. Pauli principle
D. Hund's rule
17. The volume of 2 moles of an ideal gas at STP is
A. 22.4 L
B. 44.8 L
C. 11.2 L
D. 67.2 L
18. Boyle's law is represented as
A. PV = constant
B. V/T = constant
C. P/T = constant
D. PV/T = constant
19. The temperature at which real gases behave ideally is called
A. Boyle temperature
B. Critical temperature
C. Inversion temperature
D. Absolute zero
20. According to kinetic theory, pressure is due to
A. collision of molecules with walls
B. intermolecular forces
C. volume of molecules
D. mass of molecules
21. The SI unit of pressure is
A. atm
B. bar
C. pascal
D. torr
22. In thermodynamics, system which can exchange both matter and energy is
A. isolated
B. closed
C. open
D. adiabatic
23. First law of thermodynamics is based on
A. conservation of energy
B. conservation of mass
C. conservation of momentum
D. conservation of charge
24. For an isothermal process, ΔU =
A. zero
B. positive
C. negative
D. equal to q
25. Enthalpy change at constant pressure is equal to
A. heat absorbed/released
B. work done
C. internal energy change
D. Gibbs free energy
26. The state function among the following is
A. heat
B. work
C. enthalpy
D. path function
27. Equilibrium constant Kc has units when
A. Δn = 0
B. Δn ≠ 0
C. reaction is elementary
D. reaction is complex
28. Le Chatelier's principle applies to
A. physical equilibrium only
B. chemical equilibrium only
C. both physical and chemical equilibrium
D. irreversible reactions
29. For the reaction N₂ + 3H₂ ⇌ 2NH₃, increasing pressure favours
A. forward reaction
B. backward reaction
C. no effect
D. equilibrium constant decreases
30. Oxidation number of Cr in K₂Cr₂O₇ is
A. +3
B. +6
C. +7
D. +4
31. In which compound oxygen shows +2 oxidation state?
A. H₂O
B. OF₂
C. CO₂
D. SO₂
32. The process of losing electrons is called
A. oxidation
B. reduction
C. redox
D. disproportionation
33. In balancing redox reactions, number of electrons lost equals
A. electrons gained
B. atoms oxidized
C. atoms reduced
D. charge on ions
34. Which of the following is not a physical change?
A. Melting of ice
B. Evaporation of water
C. Rusting of iron
D. Dissolution of sugar
35. PPM stands for
A. parts per million
B. percentage per mole
C. parts per mole
D. proportion per mass
36. Molality is defined as
A. moles of solute per kg solvent
B. moles per litre solution
C. mass per volume
D. equivalent per litre
37. The unit of molarity is
A. mol/kg
B. mol/L
C. g/L
D. mol/m³
38. Which has highest number of atoms?
A. 1 mole Na
B. 1 mole O₂
C. 1 mole CO₂
D. 1 mole CH₄
39. The atomicity of ozone (O₃) is
A. 1
B. 2
C. 3
D. 4
40. Graham's law is related to
A. diffusion/effusion of gases
B. Boyle's law
C. Charles' law
D. Avogadro's law
41. The root mean square speed is proportional to
A. √T
B. T
C. 1/√M
D. Both A and C
42. In adiabatic process,
A. q = 0
B. ΔU = w
C. temperature changes
D. All of the above
43. Hess's law is based on
A. first law of thermodynamics
B. second law
C. third law
D. zeroth law
44. For exothermic reaction, ΔH is
A. positive
B. negative
C. zero
D. infinite
45. The equilibrium constant Kp for gaseous reaction is expressed in terms of
A. partial pressures
B. concentrations
C. mole fractions only
D. volume
46. If Kc > 1, the reaction proceeds
A. towards products
B. towards reactants
C. remains at equilibrium
D. cannot be predicted
47. In disproportionation reaction, same element is
A. oxidised and reduced
B. only oxidised
C. only reduced
D. neither oxidised nor reduced
48. The oxidation number of S in H₂SO₅ is
A. +6
B. +8
C. +4
D. +2
49. Which is an extensive property?
A. Temperature
B. Density
C. Volume
D. Pressure
50. The number of moles in 4 g of oxygen gas (O₂) is
A. 0.125
B. 0.25
C. 0.5
D. 1
You can now use these for practice tests, worksheets, or self-assessment.
If you want another set (with or without answers) on a different topic, just let me know! Good luck with your studies!