General Chemistry I — 2023 Past Questions

University of Ilorin CHM101: 70 questions.

Topics: Elementary thermochemistry, Redox reactions and introduction to electrochemistry, Modern electronic theory of atoms, Periodicity and building up of the periodic table., Atoms, elements, molecules, Properties of gases, Structure of solids, Chemical bonding and intermolecular forces, Periodicity and building up of the periodic table, Radioactivity, Electronic configuration, Forces, Chemical equations and stoichiometry, Kinetic theory of matter

  1. Ice floats due to ___
    1. low mass of ice
    2. higher density of water
    3. hydrogen bonding
    4. low melting point of ice
  2. Which has the highest density?
    1. glass
    2. vapour
    3. ethane
    4. dimethyl ether
  3. If hydrogen has ionization energy E, the ionization energy of He would be
    1. 2E
    2. 4E
    3. E/2
    4. E^2
  4. If the enthalpy of atomization of tetrachloromethane is X, what is the bond energy of C--Cl?
    1. X/2
    2. X/3
    3. X/4
    4. 4X
  5. What is electrochemistry?
    1. Study of compounds with oxygen
    2. Study of reactions involving heat
    3. Study of chemical reactions involving electric current
    4. Study of water properties
  6. What is Hess' law?
    1. Energy is created in reactions
    2. Heat change depends on catalyst
    3. Total enthalpy change is path independent
    4. Total entropy remains constant
  7. Mg²⁺, N³⁻, and Na⁺ have ____ electrons.
    1. 10
    2. 11
    3. 12
    4. 13
  8. Which of the following represents electron affinity?
    1. Ca⁺ + e⁻ → Ca
    2. O + 2e⁻ → O²⁻
    3. Na⁺ + e⁻ → Na
    4. None of the above
  9. What is the SHE of hydrogen electrode?
    1. 1.00 V
    2. 0.00 V
    3. -0.76 V
    4. +0.76 V
  10. What is the unit of a first order reaction?
    1. 1/M²
    2. mol/L/s
    3. 1/s
    4. 1/ms
  11. The ratio of the radii of the first orbits of H, He⁺ and Li²⁺ is
    1. 1:2:3
    2. 6:3:2
    3. 9:4:1
    4. 1:3:6
  12. A system that can neither exchange energy nor matter with its surrounding is
    1. Open system
    2. Closed system
    3. Isolated system
    4. Equilibrium system
  13. Which of the following has the highest enthalpy change?
    1. ∆H fusion
    2. ∆H evaporation
    3. ∆H sublimation
    4. ∆H neutralization
  14. If a solution of freshly prepared cisplatin has a concentration of 0.053 mol/dm³, what will be the concentration after 5 half-lives?
    1. 0.1065 mol/dm³
    2. 0.00166 mol/dm³
    3. 0.0265 mol/dm³
    4. 0.00053 mol/dm³
  15. At constant temperature and volume, the heat that flows into the system is equal to
    1. Enthalpy
    2. Entropy
    3. Change in internal energy
    4. Pressure
  16. At constant temperature and pressure, the heat that flows into the system is equal to
    1. Entropy
    2. Enthalpy
    3. Sublimation
    4. Work
  17. Which of the following is NOT true about a galvanic cell?
    1. It converts chemical energy into electrical energy
    2. It has a salt bridge
    3. It uses spontaneous reactions
    4. It produces electricity using non-spontaneous reactions
  18. Na⁺, Mg²⁺, Al³⁺ have how many protons?
    1. 10
    2. 11
    3. 14
    4. 12
  19. When E⁰ is negative, then the reaction is?
    1. Spontaneous
    2. Non-spontaneous
    3. Reversible
    4. Neutral
  20. Hess' Law states that...
    1. Heat absorbed depends on temperature
    2. Total enthalpy change is independent of the path
    3. Enthalpy depends on number of steps
    4. Energy is created during reaction
  21. Orders are known by...
    1. Balanced chemical equation
    2. Experiment only
    3. Catalyst involved
    4. Molar mass of products
  22. What is the unit for a first order reaction?
    1. mol⁻¹ dm³ s⁻¹
    2. mol s⁻¹
    3. s⁻¹
    4. mol⁻² dm⁶ s⁻¹
  23. What is the intermolecular force present in ICl?
    1. Dipole-dipole
    2. London dispersion force; dipole-induced dipole
    3. London dispersion force
    4. Dipole-dipole; London dispersion force
  24. In the electrochemical cell K.K⁺(0.1M)// Cl.Cl⁻(0.2M), which one is the cathode?
    1. K
    2. Cl
    3. K⁺
    4. KCl
  25. When the bond formed is greater than the bond broken, the reaction is
    1. Endothermic
    2. Exothermic
    3. Feasible
    4. Non-feasible
  26. The branch of chemistry which studies energy changes in physical and chemical transformations is
    1. Thermodynamics
    2. Thermochemistry
    3. Electrochemistry
    4. Physical chemistry
  27. What is the ratio of kinetic energy to total energy in Bohr’s model?
    1. -1:2
    2. 1:1
    3. 1:-1
    4. -1:-1
  28. The density of a substance is 2.68 g/mL. What is the substance?
    1. NO₂
    2. CoS
    3. SO₂
    4. Cannot be determined without more data
  29. Vapour pressure increases when
    1. Temperature increases
    2. Temperature decreases
    3. Volume increases
    4. Pressure increases
  30. What is the charge on a proton?
    1. 1.602×10⁻¹⁹ C
    2. -1.602×10⁻¹⁹ C
    3. 0 C
    4. 3.204×10⁻¹⁹ C
  31. The charge of an electron was discovered by
    1. Millikan
    2. Rutherford
    3. J.J. Thomson
    4. Bohr
  32. The deflection of a few alpha particles in the gold foil experiment shows that
    1. The nucleus is heavy
    2. The nucleus is small
    3. Electrons are mobile
    4. Atoms are indivisible
  33. When the electrode potential is in equilibrium
    1. E = 0
    2. E > 0
    3. E < 0
    4. E = 1
  34. An example of a standard electrode is
    1. Calomel electrode
    2. Lead-acid electrode
    3. Alkaline battery
    4. Mercury-zinc cell
  35. When work is done by the system on the surroundings, W is
    1. Negative
    2. Positive
    3. Zero
    4. Infinite
  36. A radioactive decay is always
    1. Zero order
    2. First order
    3. Second order
    4. Third order
  37. What kind of solid is NH₃?
    1. Molecular
    2. Ionic
    3. Covalent
    4. Sky Bison
  38. Determine the half-life of a zero-order reaction with [A]₀ = 1.2 M and k = 0.00625 M/s
    1. 625 s
    2. 69 s
    3. 96 s
    4. 62500 s
  39. A first order reaction is 40% complete in 50 minutes, how many minutes will it take for the same reaction to be 80% complete?
    1. 100 mins
    2. 120 mins
    3. 150 mins
    4. 160 mins
  40. What type of bond exists between hydrogen and fluorine in HF?
    1. Hydrogen bond
    2. Dipole-dipole
    3. Covalent
    4. Ionic
  41. Which of the following has the highest density?
    1. Gas
    2. Liquid
    3. Solid
    4. Plasma
  42. Which is the most electronegative element among O, Se, Te, S?
    1. O
    2. Se
    3. Te
    4. S
  43. What best describes an iso-electronic species?
    1. Atoms of different elements with the same number of protons and electrons
    2. Atoms of the same element with different number of electrons
    3. Atoms of different elements with the same number of neutrons
    4. Atoms of different elements with the same number of electrons
  44. In iso-electronic species,
    1. Ionic radii decrease with increasing atomic number
    2. Ionic radii increase with increasing atomic number
    3. Ionic radii do not depend on atomic number
    4. Ionic radii are constant
  45. The flow of energy into a system at constant temperature and pressure is called
    1. Internal energy
    2. Temperature
    3. Enthalpy change
    4. Entropy
  46. For an exothermic reaction,
    1. Potential of reactants is less than products and ΔH is positive
    2. Potential of products is less than reactants and ΔH is negative
    3. Potential of products is less than reactants and ΔH is positive
    4. Potential of reactants is greater than products and ΔH = 0
  47. The rate of evaporation depends on
    1. Surface area
    2. Temperature
    3. Humidity
    4. All of the above
  48. Which of the following statements about vapor pressure is NOT true?
    1. Vapor pressure increases with increase in temperature
    2. Vapor pressure decreases with increase in temperature
    3. Vapor pressure is independent of temperature
    4. Both II and III
  49. Arrange the following in order of increasing ionic radius: H⁺, Li⁺, Na⁺, K⁺, Rb⁺
    1. H⁺ < Li⁺ < Na⁺ < K⁺ < Rb⁺
    2. Rb⁺ < K⁺ < Na⁺ < Li⁺ < H⁺
    3. Li⁺ < Na⁺ < K⁺ < Rb⁺ < H⁺
    4. H⁺ < Rb⁺ < K⁺ < Na⁺ < Li⁺
  50. Faraday's first law is expressed as
    1. M ∝ Q
    2. M ∝ Q²
    3. M ∝ 1/Q
    4. M ∝ Q/2
  51. What type of bond is present in a molecule of HF?
    1. Hydrogen
    2. Covalent
    3. Ionic
    4. Molecular
  52. Radioactive decay is said to be:
    1. Zero order
    2. First order
    3. Second order
    4. None of the above
  53. Which quantum number cannot be the same for two electrons in the same orbital according to Pauli's exclusion principle?
    1. Principal quantum number
    2. Azimuthal quantum number
    3. Spin quantum number
    4. Magnetic quantum number
  54. Which of these does not belong to f-block elements?
    1. Hafnium
    2. Lawrencium
    3. Thorium
    4. Cerium
  55. Which of these is not an endothermic reaction?
    1. Condensation
    2. Melting
    3. Boiling
    4. Evaporation
  56. Which of the following is not a standard reference electrode?
    1. Silver-silver chloride electrode
    2. Saturated calomel electrode
    3. Standard hydrogen electrode
    4. Membrane electrode
  57. Which of the following represents electron affinity?
    1. X + e⁻ → X⁻
    2. He + e⁻ → He
    3. Cl₂ + energy → Cl
    4. None of the above
  58. Corpuscular theory was proposed by which of the following scientists?
    1. Niels Bohr
    2. Sir Isaac Newton
    3. James Clerk Maxwell
    4. JJ Thomson
  59. When bond is broken, ∆H is:
    1. Positive
    2. Negative
    3. Zero
    4. Undefined
  60. If E° is negative:
    1. Reaction is spontaneous
    2. Reaction is in equilibrium
    3. ∆G is positive
    4. Reaction is non-spontaneous
  61. Which of these is the best oxidizing agent?
    1. Cl₂, E° = +1.36V
    2. O₂, E° = +0.45V
    3. Na⁺, E° = -2.71V
    4. Fe³⁺, E° = +0.77V
  62. Which of the following represents electron affinity?
    1. Cl(g) + e⁻ → Cl⁻(g)
    2. Ca²⁺ + 2e⁻ → Ca(g)
    3. CO²⁺ → CO³⁺ + e⁻
    4. Cl⁺ + energy → Cl(g)
  63. What was the thickness of the gold foil used in Rutherford’s alpha scattering experiment?
    1. 0.04 cm
    2. 0.0004 mm
    3. 0.0004 cm
    4. 0.400 mm
  64. Which of the following is true about vapor pressure and intermolecular forces?
    1. High vapor pressure means strong intermolecular forces
    2. High vapor pressure means weak intermolecular forces
    3. Low vapor pressure means weak intermolecular forces
    4. None of the above
  65. Which of the following is true about ionization energy?
    1. 1st ionization energy is less than 2nd ionization energy
    2. 2nd ionization energy is greater because it's easier to remove a second electron
    3. Group 3 elements always have higher ionization energy than Group 2
    4. All ionization energies are equal for a given element
  66. Which of the following is true about the periodic law?
    1. Periodic properties are a function of atomic masses
    2. Periodic properties are a function of atomic numbers
    3. Periodic properties are random
    4. Periodic properties are a function of chemical formulas
  67. Which of the following is true?
    1. Anions are bigger than all neutral atoms
    2. Anions are smaller than their corresponding atoms
    3. Cations are smaller than their corresponding atoms
    4. Anions are the same size as their corresponding atoms
  68. A reaction that involves two reactants can never be
    1. First order
    2. Second order
    3. Unimolecular
    4. Bimolecular
  69. Which of the following are isoelectronic: N³⁻, O²⁻, F⁻, Na⁺, Mg²⁺?
    1. All of them
    2. Only N³⁻, O²⁻, and F⁻
    3. N³⁻, O²⁻, F⁻, and Na⁺
    4. N³⁻, O²⁻, F⁻, Na⁺, and Mg²⁺
  70. The rate of a zero order reaction is doubled with a 10°C rise. By how much will the rate increase from 10°C to 100°C?
    1. 512 times
    2. 256 times
    3. 64 times
    4. 128 times

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