Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. A solution containing 12.5 g of a non-electrolyte substance in 175 g of water gave boiling point elevation of 0.70 K. Calculate the molar mass of the substance. 150 g/mol 250 g/mol 200 g/mol 100 g/mol None Hint 2. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From ethyl bromide From ethane From amide From ethanoic acid None Hint 3. Which observation of Rutherford’s α-ray scattering experiment led to the conclusion that all the positive charge of the atom was contained in the nucleus? The α-particles scattered uniformly in all directions. Most of the α-particles passed straight through the foil. The α-particles lost energy while passing through the foil. A few α-particles were deflected at large angles. None Hint 4. What is the oxidation number of atoms in their elemental form? -1 +1 0 +2 None Hint 5. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: not related to each other exponentially related to each other inversely related to each other directly related to each other None Hint 6. Why is the shape of ammonia molecule trigonal pyramidal? Due to repulsion between lone pair electrons. Because of linear arrangement of atoms. Due to the presence of three bonded pairs only. Because of double bonds between nitrogen and hydrogen. None Hint 7. Vulcanization of rubber produces: a plasticizer an elastomer a thermoplastic polymer a thermosetting polymer None Hint 8. Complete and balance the following chemical equations: XeF6 + 2H2O → XeO3 + 6HF XeF4 + 4HF XeO2F2 + 4HF XeOF4 + 2HF None Hint 9. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Molality Normality Molarity Mole fraction None Hint 10. How can you obtain propanamine using Hofmann Bromamide reaction? From alkene using HBr From alcohol using NH3 From amide using bromine and NaOH From alkane by nitration None Hint 11. Why is chloroform stored in dark colored bottles? To keep it cool To protect from light which decomposes it To avoid evaporation For aesthetic reasons None Hint 12. How will you carry out the following conversions? (i) Ethanol to But-2-enal (ii) Propanone to 2-Methyl Butan-2-ol (iii) Butanoic acid to 2-Bromobutanoic acid Reduction, Oxidation, Addition Oxidation, Grignard reaction, Substitution Elimination, Substitution, Oxidation Substitution, Addition, Elimination None Hint 13. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → Na2SO4 + HCl NaHSO4 + Cl2 NaHSO4 + HCl NaHSO4 + HCl None Hint 14. State Heisenberg’s uncertainty principle. Momentum is always zero. Position can be measured exactly. It is impossible to know both the exact position and momentum of a particle simultaneously. It is possible to know the exact position and momentum simultaneously. None Hint 15. Which of the following is not a function of salt bridge? It maintains electrical neutrality. It completes the inner circuit. It prevents accumulation of charges in the two half cells. It completes the outer circuit. None Hint 16. Enthalpy is a __ function. state isolated closed path None Hint 17. What is the pH of a 0.001 M aqueous solution of HCl? 11 3 1 7 None Hint 18. A system which can exchange energy but not matter with the surroundings is called __ system. open path closed isolated None Hint 19. Bronsted-Lowry concept of an acid and a base is based on: acceptance of proton and donation of proton respectively donation of H⁺ ion and OH⁻ ion respectively formation of H₃O⁺ ion and OH⁻ ion donation of proton and acceptance of proton respectively None Hint 20. Why does an ice cube float on water? Water contracts on freezing Ice has higher melting point Ice is denser than water Ice is less dense than water None Hint 21. Classify the following oxides into acidic, basic or amphoteric oxides: FeO, SiO2, SO2, Al2O3 FeO - Acidic, SiO2 - Basic, SO2 - Amphoteric, Al2O3 - Acidic FeO - Acidic, SiO2 - Amphoteric, SO2 - Basic, Al2O3 - Acidic FeO - Amphoteric, SiO2 - Basic, SO2 - Acidic, Al2O3 - Basic FeO - Basic, SiO2 - Acidic, SO2 - Acidic, Al2O3 - Amphoteric None Hint 22. What are ozonides? Give chemical equation for their formation. Compounds formed by alkali metals and ozone Compounds formed by alkenes and ozone Compounds formed by oxygen and water Compounds formed by hydrogen and ozone None Hint 23. Define bond enthalpy. Calculate the bond enthalpy of CH4 molecule if average bond enthalpy of C-H bond is 414 kJ/mol. Energy change in electron transfer Energy released in bond formation Energy required to break one mole of bonds in gaseous molecules Energy required to break ionic bonds None Hint 24. Which of the following is not a function of salt bridge? It completes the outer circuit. It completes the inner circuit. It prevents accumulation of charges in the two half cells. It maintains electrical neutrality. None Hint 25. Choose the most electronegative element from the following: Oxygen Fluorine Nitrogen Sulphur None Hint 26. Low density polyethylene: has branching in polymer chains is harder and stronger than polypropylene has linear chain of molecules is packed in a compact fashion None Hint 27. Write True (T) or False (F) for the following statements: Raoult’s law is applicable only if the liquids are volatile and miscible. False Depends on temperature Sometimes true True None Hint 28. What is the active component of soap? What is the polar part in (i) a soap molecule and (ii) a synthetic detergent molecule? Fatty acid; carboxyl group Fatty acid; methyl group Alcohol; hydroxyl group Detergent; sulphate group None Hint 29. Low density polythene: Has branching in polymer chains Is harder and stronger than polypropylene Has linear chain of molecules Is packed in a compact fashion None Hint 30. What is the pH of a 0.001 M aqueous solution of HCl? 1 3 2 4 None Hint 31. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 199, 80, 199 80, 119, 80 80, 199, 80 119, 80, 119 None Hint 32. What is the oxidation number of atoms in their elemental form? +1 +2 0 −1 None Hint 33. Geometrical isomerism is shown by isomers... possible for coordination number: less than or equal to four greater than or equal to four equal to two greater than or equal to two None Hint 34. Vulcanization of rubber produces: a thermosetting polymer a plasticizer a thermoplastic polymer an elastomer None Hint 35. Write the IUPAC name of the compound (benzene ring with two Br at 1,3 positions and CH2CH3 at 4): 3,4-Dibromo-1-ethylbenzene 1,3-Dibromo-4-ethylbenzene 1,4-Dibromo-3-ethylbenzene 1,2-Dibromo-4-ethylbenzene None Hint 36. The standard enthalpy of atomisation of a substance is the change in enthalpy when: One molecule of a substance is converted into its atom in gaseous state at a given temperature and 1 bar pressure. One molecule of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at a given temperature and 1 bar pressure. None Hint 37. In every chemical reaction, total mass of all the reactants is equal to the total mass of all the products. This statement is according to: Law of constant proportions Law of conservation of mass Postulates of Dalton’s atomic theory Law of multiple proportions None Hint 38. State the oxidation number of N and Cl in NCl3. N = +1, Cl = -3 N = 0, Cl = 0 N = +3, Cl = -1 N = -3, Cl = +1 None Hint 39. What is the shape and magnetic behaviour of Ni(CO)₄? Square planar and paramagnetic Linear and diamagnetic Octahedral and paramagnetic Tetrahedral and diamagnetic None Hint 40. The 3d series of transition metals/elements is from: Scandium to Copper Scandium to Zinc Yttrium to Lanthanum Actinium to Lawrencium None Hint 41. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 4-Chloropentane 2-Chloropentane 3-Chloropentane 1-Chloropentane None Hint 42. Which liquid pairs show negative deviation from Raoult's Law? Benzene and toluene Water and ethanol Water and salt solution Chloroform and acetone None Hint 43. Geometrical isomerism is shown by isomers in which first coordination sphere is same but geometrical arrangement of ligands varies. This isomerism is only possible for coordination number: Greater than or equal to two Less than or equal to two Equal to two Greater than or equal to four None Hint 44. Which compound forms ethyl carbocation? Ethene Ethyl chloride Ethane Ethanol None Hint 45. A solution containing 12.5 g of a non-electrolyte substance in 175 g of water gave boiling point elevation of 0.70 K. The molar mass of the substance is: 125 g/mol 75 g/mol 50 g/mol 100 g/mol None Hint 46. The 3d series of transition metals/elements is from: Actinium to Lawrencium Yttrium to Lanthanum Scandium to Copper Scandium to Zinc None Hint 47. If 3d and 4p orbitals are to be filled in an atom by an electron then which orbital will be occupied first? 3d orbital 4p orbita Depends on the element Both at the same time None Hint 48. (i) State Faraday's first law of electrolysis. (ii) What is the mass of silver deposited when 300 coulomb electricity is passed through AgNO3 solution? (Atomic mass Ag = 108 u) Mass ∝ time taken Mass ∝ concentration Mass ∝ charge passed Mass ∝ voltage applied None Hint 49. State the function of oxytocin: Controls digestion Controls muscle contraction Controls childbirth and lactation Controls blood pressure None Hint 50. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Molality Molarity Normality Mole fraction None Hint 51. In every chemical reaction, total mass of all the reactants is equal to the total mass of all the products. This statement is according to: Law of multiple proportions Law of constant proportions Law of conservation of mass Postulates of Dalton’s atomic theory None Hint 52. Match the following: Yellow and transparent crystalline substance → (4) Sulphur dioxide Tailing of mercury → (1) Conc. Sulphuric acid Decomposed in a strong beam of light → (3) Ozone Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur None Hint 53. The factors affecting conductivity of an electrolyte are: nature of the electrolyte and temperature temperature and concentration nature of the electrolyte, temperature and concentration nature of the electrolyte and concentration None Hint 54. Predict the shape of methane molecule on the basis of VSEPR theory. Octahedral Tetrahedral Trigonal planar Linear None Hint 55. State the function of oxytocin. Controls blood sugar Regulates metabolism Increases heart rate Stimulates uterine contraction None Hint 56. State one physical property which is same for lithium and magnesium. Low electronegativity Large atomic radius High melting point Low density None Hint 57. What is the shape and magnetic behavior of [Ni(CN)4]2- ion according to Valence Bond Theory (VBT)? Tetrahedral and paramagnetic Octahedral and diamagnetic Linear and paramagnetic Square planar and diamagnetic None Hint 58. One atomic mass unit is equal to: Mass of one C–12 atom × 12 Mass of one mole of C–12 atoms ÷ 12 Mass of one C–12 atom ÷ 12 Mass of one mole of C–12 atoms None Hint 59. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: inversely related to each other exponentially related to each other not related to each other directly related to each other None Hint 60. Which of the following is equal to 1 mole O₂? 6.022 × 10²³ molecules of Oxygen 60.22 × 10²³ atoms of Oxygen 6.022 × 10²³ atoms of Oxygen 60.22 × 10²² molecules of Oxygen None Hint 61. The standard enthalpy of atomisation of a substance is the change in enthalpy when: One molecule of a substance is converted into its atom in gaseous state at a given temperature and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at a given temperature and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. One molecule of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. None Hint 62. If the bond enthalpy of C–H and C–Cl bonds are 415 kJ mol⁻¹ and 339 kJ mol⁻¹ respectively, then the energy released in the formation of one mole of CH₃Cl molecules is: +1574 kJ mol⁻¹ +20 kJ +80 kJ −1574 kJ mol⁻¹ None Hint 63. Bronsted–Lowry concept of an acid and a base is based on: donation of proton and acceptance of proton respectively formation of H₃O⁺ ion and OH⁻ ion donation of H⁺ ion and OH⁻ ion respectively acceptance of proton and donation of proton respectively None Hint 64. A system which can exchange energy but not matter with the surroundings is called: Open system Isolated system Closed system State system None Hint 65. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 80, 199, 80 119, 80, 119 199, 80, 199 80, 119, 80 None Hint 66. Which type of compound water is? Hydrogen Ionic Covalent Metallic None Hint 67. Write True (T) or False (F) for the following statements: Boiling point of a liquid is the temperature at which the vapor pressure of the liquid becomes zero. False True Always true Never true None Hint 68. Adiabatic processes proceeds with: an exchange of heat between the system and the surroundings no change in temperature a change in pressure a change in temperature None Hint 69. The percentage of oxygen in Fe₃O₄ is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) 72.41% None of these 27.59% 27.89% None Hint 70. The factors affecting conductivity of an electrolyte are: nature of the electrolyte and concentration temperature and concentration nature of the electrolyte, temperature and concentration nature of the electrolyte and temperature None Hint 71. What is the active component of soap? What is the polar part in: (i) a soap molecule (ii) a synthetic detergent molecule Ester, -OH Alcohol group, -CH3 Hydrocarbon chain, -COONa Ketone, -NH2 None Hint 72. Adiabatic processes proceeds with: A change in temperature No change in temperature An exchange of heat between the system and the surroundings A change in pressure None Hint 73. The empirical formula of fructose is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) CHO₂ CHO None of these CH₂O None Hint 74. When a certain change is accompanied by absorption of 50 kJ of heat and expenditure of 30 kJ of work, then the change in internal energy is: Complete the following by given options below: (+20 kJ, +80 kJ, −1574 kJ mol⁻¹, +1574 kJ mol⁻¹) +80 kJ B. +20 kJ +1574 kJ mol⁻¹ −1574 kJ mol⁻¹ None Hint 75. State Heisenberg’s uncertainty principle: v = λf E = hv ΔE · Δt = h Δx · Δp ≥ h/4π None Hint 76. How are hormones transported to their place of action? By blood By diffusion By water By air None Hint 77. Lanthanide contraction is due to increase in: Effective nuclear charge Shielding by 4f electrons Atomic number Size of 4f orbital None Hint 78. State the oxidation number of N and Cl in NCl₃. N = +1, Cl = −3 N = −3, Cl = +1 N = +5, Cl = −1 N = +3, Cl = −1 None Hint 79. Give the mathematical expression of de-Broglie equation. λ = h / mv λ = h × mv ) λ = mv / h λ = m / hv None Hint 80. Enthalpy is a __ function. Path State Open Closed None Hint 81. Give the mathematical expression of de-Broglie equation: E = mc² p = mv λ = h/mv F = ma None Hint 82. How are hormones transported to their place of action? Through nerves By diffusion Through bloodstream By active transport None Hint 83. The consequence of lanthanide contraction is: Radii of elements of second and third transition series becomes similar. Radii of third transition series is smaller than elements of second transition series. Radii of elementstransition series decreases. Radii of elements of second transition series increases. None Hint 84. Choose the most electronegative element from the following: Nitrogen Sulphur Fluorine Oxygen None Hint Time's up Share: admin Previous post Physics Nios Plus Two PQ III July 5, 2025 Next post Malayalam Nios plus two II July 10, 2025
