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