NTS GAT Subject (Chemistry) FLP 2 Free Quiz

NTS GAT Subject (Chemistry) – FLP 2

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NTS GAT Subject (Chemistry) – FLP 2 consists of 100 MCQs covering 1 subjects. You have 120 minutes to complete it. Start with the easier questions and manage your time wisely. Good luck!

Chemistry 100 MCQs

1. What does physical chemistry deal with?

A. Physical properties and changes of matter B. Carbon compounds C. Non-carbon compounds D. Analysis of substances

2. What are the three states of matter?

A. Solid, liquid, plasma B. Solid, gas, plasma C. Solid, liquid, gas D. Liquid, gas, plasma

3. What is the ideal gas law?

A. PV = nRT B. PV = nRT C. PV = nRT D. PV = nRT

4. What law states that PV is constant at constant temperature?

A. PV constant B. V/T constant C. P/T constant D. V/n constant

5. What is the amount of solute dissolved in a given amount of solvent called?

A. Molarity B. Molality C. Normality D. Concentration

6. What is the number of moles of solute per kilogram of solvent?

A. Molality B. Molarity C. Normality D. Mole fraction

7. What is the lowering of the freezing point of a solution called?

A. Boiling point elevation B. Vapor pressure lowering C. Freezing point depression D. Osmotic pressure

8. What equation corrects the ideal gas law for intermolecular forces and particle volume?

A. Boyle B. Charles C. Gay-Lussac D. van der Waals

9. What force causes the surface of a liquid to contract?

A. Viscosity B. Surface tension C. Capillary action D. Evaporation

10. What is the functional group of alcohols?

A. Carbonyl B. Carboxyl C. Hydroxyl D. Amino

11. What is the IUPAC name of CH4?

A. Ethane B. Methane C. Propane D. Butane

12. What is the IUPAC name of C2H6?

A. Ethane B. Methane C. Propane D. Butane

13. What aromatic hydrocarbon has the formula C6H6?

A. Cyclohexane B. Cyclohexene C. Benzene D. Hexane

14. What is the introduction of a nitro group onto an aromatic ring?

A. Sulfonation B. Halogenation C. Nitration D. Alkylation

15. What are organomagnesium compounds used to form carbon-carbon bonds?

A. Organolithium B. Grignard C. Organozinc D. Organocopper

16. What reaction is a cycloaddition between a diene and a dienophile?

A. Addition B. Elimination C. Diels-Alder D. Rearrangement

17. What does inorganic chemistry study?

A. Compounds without carbon-hydrogen bonds B. Carbon compounds C. Physical properties D. Analysis of substances

18. What happens to atomic radius across a period?

A. Increases B. Stays the same C. Fluctuates D. Decreases

19. What bonding involves the transfer of electrons?

A. Covalent B. Metallic C. Ionic D. Hydrogen bonding

20. What bonding involves the delocalization of electrons?

A. Ionic B. Metallic C. Covalent D. Hydrogen bonding

21. What rule states that atoms tend to achieve eight valence electrons?

A. Duet rule B. Inert pair effect C. Octet rule D. Eighteen-electron rule

22. What theory predicts molecular geometry?

A. MO theory B. VB theory C. Crystal field theory D. VSEPR theory

23. What is the molecular geometry of CO2?

A. Linear B. Bent C. Tetrahedral D. Trigonal planar

24. What substances donate protons in solution?

A. Bases B. Acids C. Salts D. Oxides

25. What scale measures the acidity or basicity of a solution?

A. Temperature B. Pressure C. pH D. Concentration

26. What does a strong acid do in water?

A. Weak B. Partial C. Reversible D. Completely dissociates

27. What type of analysis identifies the presence of substances?

A. Quantitative B. Volumetric C. Qualitative D. Gravimetric

28. What type of analysis measures the amount of substances?

A. Qualitative B. Volumetric C. Gravimetric D. Quantitative

29. What is a volumetric method for determining concentration?

A. Gravimetric B. Titration C. Spectrophotometric D. Chromatographic

30. What is the point when the amount of titrant is stoichiometrically equal to the analyte?

A. End point B. Inflection point C. Equivalence point D. Half-equivalence point

31. What is indicated by a color change or other signal?

A. Equivalence point B. Inflection point C. Half-equivalence point D. End point

32. What branch studies electrochemical processes?

A. Electroanalytical B. Spectroscopy C. Chromatography D. Gravimetry

33. What spectroscopy is used to determine molecular structure?

A. IR B. UV-Vis C. NMR D. MS

34. What spectroscopy identifies functional groups?

A. NMR B. UV-Vis C. MS D. IR

35. What spectroscopy is used for metal analysis?

A. NMR B. IR C. AAS D. UV-Vis

36. What does the Second Law of Thermodynamics state?

A. Energy conservation B. Enthalpy C. Gibbs free energy D. Entropy increases

37. What does the Third Law of Thermodynamics state?

A. Entropy increases B. Entropy approaches zero C. Entropy constant D. Entropy infinite

38. What is the heat content of a system at constant pressure?

A. Enthalpy B. Internal energy C. Entropy D. Gibbs free energy

39. What is a measure of disorder or randomness?

A. Enthalpy B. Internal energy C. Entropy D. Gibbs free energy

40. What does a negative ΔG indicate?

A. Positive B. Negative C. Zero D. Undefined

41. What does a positive ΔG indicate?

A. Positive B. Negative C. Zero D. Undefined

42. What is the relationship between ΔG, ΔH, and ΔS?

A. ΔG = ΔH + TΔS B. ΔG = ΔH/T + ΔS C. ΔG = ΔH - T/ΔS D. ΔG = ΔH - TΔS

43. What reaction releases heat?

A. Endothermic B. Exothermic C. Isothermal D. Adiabatic

44. What law states that enthalpy change is independent of the pathway?

A. First Law B. Second Law C. Hess's Law D. Third Law

45. What is the enthalpy change when an acid reacts with a base?

A. Neutralization B. Formation C. Combustion D. Solution

46. What is the energy required to break a bond?

A. Formation B. Combustion C. Neutralization D. Bond dissociation

47. What cycle is used to calculate lattice enthalpy?

A. Haber process B. Contact process C. Born-Haber cycle D. Solvay process

48. What is the sum of the exponents in the rate law?

A. Molecularity B. Order C. Rate constant D. Activation energy

49. What is the number of molecules involved in the rate-determining step?

A. Molecularity B. Order C. Rate constant D. Activation energy

50. What is the Arrhenius equation?

A. k = A e^(Ea/RT) B. k = A T e^(-Ea/RT) C. k = A e^(-Ea/T) D. k = A e^(-Ea/RT)

51. What increases the reaction rate by providing an alternative pathway?

A. Reactant B. Product C. Catalyst D. Inhibitor

52. What is the integrated rate law for a second-order reaction?

A. ln[A] = -kt + ln[A]0 B. [A] = -kt + [A]0 C. ln[A] = kt + ln[A]0 D. 1/[A] = kt + 1/[A]0

53. What is the integrated rate law for a zero-order reaction?

A. ln[A] = -kt + ln[A]0 B. [A] = -kt + [A]0 C. 1/[A] = kt + 1/[A]0 D. [A] = kt + [A]0

54. What theory describes the formation of an activated complex?

A. Transition state theory B. Collision theory C. Arrhenius theory D. Eyring theory

55. What theory states that reactions occur when molecules collide with sufficient energy?

A. Transition state B. Arrhenius C. Collision theory D. Eyring

56. What is the maximum rate of an enzyme-catalyzed reaction?

A. Km B. kcat C. Turnover number D. Vmax

57. What does electrochemistry deal with?

A. Electricity and chemical reactions B. Energy changes C. Reaction rates D. Spectra

58. What converts chemical energy into electrical energy or vice versa?

A. Battery B. Fuel cell C. Electrochemical cell D. Electrolytic cell

59. What is oxidation?

A. Gain of electrons B. Reduction C. Neutralization D. Loss of electrons

60. What completes the circuit and maintains electrical neutrality?

A. Salt bridge B. Electrolyte C. Electrode D. External circuit

61. What is the cell potential?

A. E°cathode - E°anode B. E°cathode + E°anode C. E°cathode × E°anode D. E°cathode / E°anode

62. What does a negative E°cell indicate?

A. Positive B. Zero C. Spontaneous D. Negative

63. What is the ability of a solution to conduct electricity?

A. Resistance B. Potential C. Conductivity D. Current

64. What is the conductivity of a solution divided by its concentration?

A. Specific conductivity B. Equivalent conductivity C. Resistance D. Molar conductivity

65. What device converts chemical energy into electrical energy?

A. Battery B. Fuel cell C. Capacitor D. Resistor

66. What method prevents corrosion by making the metal the cathode?

A. Anodic protection B. Galvanization C. Cathodic protection D. Passivation

67. What is the coating of iron with zinc to prevent corrosion?

A. Anodic protection B. Cathodic protection C. Passivation D. Galvanization

68. What ranks metals by their reactivity?

A. Electrochemical series B. Periodic table C. Activity series D. Reactivity series

69. What does coordination chemistry study?

A. Coordination compounds with metal ions and ligands B. Carbon compounds C. Non-carbon compounds D. Analysis

70. What donates a pair of electrons to a metal ion?

A. Central atom B. Coordination sphere C. Ligand D. Chelate

71. What ligands bind through two donor atoms?

A. Monodentate B. Polydentate C. Chelates D. Bidentate

72. What ligands bind through multiple donor atoms?

A. Monodentate B. Polydentate C. Bidentate D. Chelates

73. What theory described the structure of coordination compounds?

A. VSEPR B. MO C. Werner's theory D. VB

74. What theory describes the electronic structure of coordination compounds?

A. CFT B. LFT C. MO D. VB

75. What ranks ligands by their field strength?

A. Activity series B. Electrochemical series C. Periodic table D. Spectrochemical series

76. What ligands cause small splitting and high-spin complexes?

A. Weak field B. Strong field C. Intermediate D. Strong

77. What effect describes the distortion of octahedral complexes?

A. Chelate effect B. Jahn-Teller effect C. Trans effect D. Spectrochemical series

78. What effect describes the influence of a ligand on substitution opposite to it?

A. Trans effect B. Jahn-Teller effect C. Chelate effect D. Spectrochemical series

79. What type of isomerism in octahedral complexes includes cis and trans?

A. Optical B. Structural C. Ionization D. Geometrical

80. What type of isomerism results in enantiomers?

A. Geometrical B. Optical C. Structural D. Ionization

81. What isomerism occurs when a ligand can bind through different donor atoms?

A. Ionization B. Geometrical C. Optical D. Linkage

82. What is the number of wave cycles per second?

A. Wavelength B. Frequency C. Amplitude D. Speed

83. What spectroscopy measures vibrational transitions?

A. UV B. NMR C. MS D. IR

84. What law measures absorbance in spectroscopy?

A. A = εc B. A = bc C. A = εbc D. A = εb

85. What is the ratio of transmitted to incident light intensity?

A. Absorbance B. Reflectance C. Scattering D. Transmittance

86. What spectroscopy measures inelastic scattering of light?

A. IR B. NMR C. Raman D. UV

87. What technique is used for elemental analysis?

A. XRD B. XAS C. XRF D. XPS

88. What spectroscopy measures the binding energies of electrons?

A. XRD B. XRF C. XAS D. XPS

89. What spectroscopy measures electrons emitted after X-ray excitation?

A. XPS B. AES C. XRD D. XRF

90. What is the time for nuclei to return to equilibrium in NMR?

A. Chemical shift B. Coupling constant C. Line width D. Relaxation time

91. What is the amount of substance in a given volume?

A. Concentration B. Path length C. Absorbance D. Transmittance

92. What is widely used in chemistry for identification and quantification of substances?

A. Chromatography B. Titration C. Spectroscopy D. Gravimetry

93. What does environmental chemistry study?

A. Chemical processes in the environment B. Carbon compounds C. Non-carbon compounds D. Analysis

94. What is the contamination of water bodies by harmful substances?

A. Air pollution B. Water pollution C. Soil pollution D. Noise pollution

95. What is another significant greenhouse gas?

A. CO2 B. CH4 C. NO2 D. SO2

96. What causes acid rain?

A. CO2 B. CH4 C. CFCs D. SO2 and NOx

97. What is the excessive growth of algae due to nutrient enrichment?

A. Eutrophication B. Acidification C. Salinization D. Desertification

98. What heavy metals are toxic environmental pollutants?

A. Nutrients B. Heavy metals C. Greenhouse gases D. Ozone-depleting substances

99. What chemicals are used to control insects?

A. Pesticides B. Insecticides C. Herbicides D. Fungicides

100. What is the movement of oxygen through the environment?

A. Carbon cycle B. Oxygen cycle C. Nitrogen cycle D. Water cycle

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