Sample PaperScience Quiz (Chemistry)

Q 1. The equivalent weight of a metal, 6 g of which evolve 5.6 L of H2 at NTP from an acid

is:

(a) 6 (b) 12 (c) 24 (d) 2.4

Q 2. The percentage of H2 in the hydride of an element having equivalent weight 11.5 is:

(a) 7.06 (b) 8.06 (c) 4.03 (d) 12.09Q. 3 The equivalent weight of SnCl2

in the following reaction, SnCl2 + Cl2 → SnCl4 is:

(a) 190 (b) 119 (c) 95 (d) 380

Q4. Chloride of a metal M contains 47.23% of the metal. 1.0 g of this metal displaced from a compound 0.88 g of another metal N. The equivalent weight of M and N are respectively:

(a) 39.77, 29.96 (b) 63.54, 28 (c) 31.77, 81.7 (d) 31.77, 27.96

Q 5. On heating 0.398 g of a metal oxide in a current of dry hydrogen, 0.09g of water were formed. The equivalent weight of the metal is:

(a) 31.8 (b) 63.6 (c) 15.9 (d) 2.0

Q 6. 1.52 g of the hydroxide of a metal gave on ignition, 0.995 g of the oxide. The equivalent weight of the metal is:

(a) 4.53 (b) 9.06 (c) 27.18 (d) 36.24

Q 7. The equivalent weight of HNO3 in the reaction:

2HNO3 → 2NO + H2O + 3 O is :

(a) 21 (b) 42 (c) 63 (d) 10.5

Q 8. The equivalent weight of H2SO4 in the reaction:

Na2CO3 + H2SO4 → Na2SO4 + CO2 + H2O is :

(a) 98 (b) 49 (c) 32.6 (d) 16.3

Q 9. The equivalent weight of H2SO4 in the reaction:

Na2CO3 + H2SO4 → NaHSO4 + CO2 + H2O is :

(a) 49 (b) 4.9 (c) 98 (d) 196

Q 10. The number of milliequivalents of Mg (OH)2 in its 5.8 g are:

(a) 100 (b) 200 (c) 400 (d) 600

Q 11. The equivalent weight of Ca (OH)2 whose 250 milliequivalents solution contains 18.5 g of it, is :

(a) 37 (b) 18.5 (c) 74 (d) 148

Q 12. The number of milliequivalents present in 25 mL of 0.2 M Mg(OH)2 are:

(a) 5.0 (b) 10.0 (c) 15.0 (d) 20.0

Q 13. The number of milliequivalents present in 25 mL of 0.2 N Mg(OH)2 are:

(a) 0.5 (b) 0.25 (c) 5.0 (d) 10.0

Q 14. The equivalent weight of NO3¯

in :

NO3¯

→ N2O is :

(a) 15.5 (b) 31.0 (c) 62 (d) 124

Q 15. The equivalent weight of SO2 in the reaction:

SO2 + H2O + O → H2 SO4 is :

(a) 8 (b) 16 (c) 32 (d) 64

Q 16 An element having three isotopes has mass numbers M, M + 1 and M+2. Their mean atomic mass is M + 1.2. The ratio which corresponds to the given data is :

(a) 1:1:1 (b) 1:2:3 (c) 2:3:4 (d) 1:3:5

Q 17 A certain metal is divalent. 2.65 g of its oxide when reduced in a current of hydrogen leaves 2.454 g of the metal. The atomic weight of the metal will be :

(a) 100.16 (b) 200:32 (c) 50.08 (d) 25.04

Q 18 0.45 g of a metal displaced 560 cm3 of hydrogen at N.T.P. from an acid. If specific heat of metal is 0.214, the atomic weight of the metal is:

(a) 27 amu (b) 13.5 amu (c) 54 amu (d) None of these

Q 19. When a metal weighing 0.3g was treated with an acid, liberated 280 cm3 of H2 at STP. It forms an oxide MO where M stands for the metal. The atomic weight of the metal is :

(a) 6g (b) 1.1 amu (c) 24 amu (d) 12 amu

Q 20. When a metal carbonate weighing 0.84g was heated strongly, 0.40 g of metal oxide was left as the residue. The specific heat of the metals 0.25. The atomic weight of the metal is :

(a) 6 amu (b) 12 amu (c) 18 amu (d) 24 amu

Q 21. The vapour densities of four compounds of a certain metal are 8.5, 22, 23 and 26 respectively. The percentage of same elements in these compounds are 82.4, 63.7, 89.4 and 58.8 respectively. The atomic weight of the metal is :

(a) 14 (b) 41 (c) 28 (d) 30.5

Q 22. Three atoms of a metal combine with two atoms of nitrogen to form metal nitride. If the metal nitride contains 81.08% metal and 18.92%, nitrogen, the atomic weight of the metal is :

(a) 10 (b) 20 (c) 40 (d) 35

Q 23. 1.5276g of CdCl2 was found to contain 0.9367 g of cadmium. The atomic weight of cadmium is :

(a) 112.54 amu (b) 52.27 amu (c) 225.08 amu (d) None of these

24. On dissolving 2.00 g of a metal in sulphuric acid, 4.51 g of the metal sulphate was formed. The specific heat of the metal is 0.057 cal(g ¯). The valency of the metal and its exact atomic weight are :

(a) 228 amu (b) 114.75 amu (c) 110 amu (d) 56 amu

25. A compound contains 28 percent of nitrogen and 72 percent of a metal by weight. 3 atoms of the metal combine with 2 atoms of N. The atomic weight of the metal is : (a) 6 amu (b) 12 amu (c) 24 amu (d) 18 amu

26. In order to obtain 1 gm of hydrogen from dil. H2SO4, 32.5 g of zinc has to be dissolved. If the atomic weight of the zinc is 67, its valency is :

(a) 1 (b) 2 (c) 3 (d) 4

27. A solid element has a specific heat of 1 J g¯ K¯. The approximate atomic mass of the element is : (a) 17 (b) 27 (c) 2.7 (d) 1.

28. In oxide of an element possesses the formula M2SO3. If the equivalent weight of the metal is 9, then the atomic weight of the metal will be:

(a) 18 (b) 1.8 (c) 2.7 (d) 27

29. Density of ethanol is 0.791 g cm¯3. Its value in SI unit will be :

(a) 7.91 g cm¯3. (b) 79.1 g cm¯3. (c) 791 g m¯3. (d) 791 kg m¯3

30. The mass of carbon tetrachloride having volume 6.25 L and density 1.6 g cm¯3. will be :

(a) 10 g (b) 100 g (c) 10 kg (d) 200 g

31. 25 cm3 of an unknown acid (density, 1.2 g cm¯3) contains 9.2 g of the acid. The percent by weight of the acid in the concentrated acid will be :

(a) 69.33% (b) 30.67% (c) 20% (d) 80%

32. At a particular place, 1000 mL of air weighs 1.248 g. The specific gravity of air in terms of hydrogen if 1g H2 occupies 11200 mL volume will be :

(a) 13.98 (b) 10 (c) 16 (d) 2.47

33. 224 cm3 of a gas at S.T.P. weighs 0.44 g. The vapour density of the gas will be :

(a) 22 (b) 11 (c) 1.1 (d) 3.3

34. The density of nitrogen gas at 350 C and 2 atmospheric pressure is :

(a) 1.11 g cm¯3 (b) 2.22 g L¯ (c) 3.1 g L¯ (d) 4.5 kg m¯3

35. The specific gravity of a sample of 22% pure liquid is 1.1 g (mL¯). The volume of it required to get 56 g of it will be :

(a) 10 mL (b) 200 mL (c) 50 mL (d) 231.4 mL

36. A sample of 98% acid has a density of 1.9 g cm¯3. The amount of pure acid present in 2 L of the acid is :(a) 3.724 kg (b) 372.4 g (c) 3.724 g (d) 100 g

37. 2 dm3 of a gas at STP weighs 2.88 g. If 1 dm3 of H2 gas weighs 0.09 g at NTP, the mol. wt. of the gas would be:

(a) 4 g mol¯ (b) 8 g mol¯ (c) 32 g mol¯ (d) 64 g mol¯

38. 5 dm3 of a gas at 140C and 729 mm pressure weighs 8.96 g. The mol. wt. of the gas is:

(a) 87 (b) 44.0 (c) 21.75 (d) 17

39. If atomic weights of zinc and oxygen are 65 amu and 16 amu respectively, the molecular weight of zinc oxide in g mol¯will be :

(a) 8.1 g mol¯ (b) 1.8 g mol¯ (c) 81 g mol¯ (d) None of these

40. The molecular weight of a gaseous substance is 80. The volume of the one gram of the gas at 00C and 720 mm of mercury pressure will be :

(a) 295.7 mL (b) 0.2 L (c) 0.3 L (d) 397 mL

41. The weight of sulphur dioxide contained in the same volume as that which contains 7.0 g nitrogen is :

(a) 8 g (b) 16 g (c) 32 g (d) 64 g

42. 1.25 g of the carbonate of a metal on ignition leave a residue of 0.7 g and a gas evolved occupying 312 cm3 at 270C and 755 mm. The molecular weight of the gas should be :

(a) 21.7 g (b) 43.69 g (c) 87.28 g (d) 0.55 g

43. 2.24 cm3 of a gas is produced at NTP by the action of 8.24 mg of alcohol (ROH) on methyl magnesium bromide. The molar mass of alcohol is :

(a) 92.29 g (b) 184.58 g (c) 369.16 g (d) 22.4 g

44. A compound on analysis was found to contain 8% sulphur by mass. The least molar mass of that compound will be :

(a) 32 a.m.u. (b) 256 a.m.u. (c) 400 a.m.u. (d) 92 a.m.u.

45. 0.40 g of chloroplatinate of monoacid base on ignition gave 0.125 g of platinum. The molar mass of the base is :

(a) 214 g mol¯ (b) 107 g mol¯ (c) 2.14 g mol¯ (d) 12 g mol¯(at.wt.Pt=195)

46 Silver salt of a dibasic acid weighing 1.8 g gave 1.08 g of silver. The molar mass of the acid is :

(a) 166 g mol¯ (b) 1.66 g mol¯ (c) 146 g mol¯ (d) 292 g mol¯

47. 0.45 g of a diacid base were dissolved in water and the solution was made up to 250 ml. 20 ml of this diluted acid required 15 ml of N/25 HCI for complete neutralisation. The molecular weight of the base is :

(a) 120 g mol¯ (b) 60 g mol¯ (c) 180 g mol¯ (d) None of these

48. One molecule of a substance contains 6 carbon atoms, 12 hydrogen atoms and 1.5936 X 10 ¯22 g of the third component. The molecular weight of the substance is?

(a) 84 g mol¯ (b) 180 g mol¯ (c) 8.4 g mol¯ (d)85.5936X10 ¯22 g mol¯

49. A plant virus is found to consist of uniform cylindrical particles of 150 A 0 in diameter and 5000 Å long. The specific volume of the virus is 0.75 cm3 g¯. If the virus is considered to be a simple particle, the molecular weight of the virus will be :

(a) 108 g mol¯ (b) 1.234 x 107 g mol¯ (c) 7.095 X 107 g mol¯ (d) 50,000 g mol¯

50. 56 cm3 of oxygen combine with 112 cm3 of hydrogen to form water : When 56 cm3 of H2

is passed over heated capric oxide, the latter loses 0.04 g of its weight. All measurements are done under similar conditions of temperature and pressure (at. wt., H=1, O=16). Which of the following law is obeyed by this data?

(a) Gay Lussac’s law of gaseous volume (B) Law of constant composition (c) Law of multiple proportion (d) Law of reciprocal proportion

51. ICI contains 77.8% iodine, Kl contains 23.6% K and KCI contains 52% of K. These results obey the law of :

(a) constant composition (b) Reciprocal proportion(c) multiple proportion (d) conservation of mass

52. Hydrated zinc sulphate contains 22.65% Zn and 43.9% H2O. If the law of definite proportion is true, the weight of zinc used to produce 7.2 g of crystal would be :

(a) 3.2 g (b) 1.63 g (c) 0.815 g (d) None of these

53. An iodine compound on analysis was found to contain iodine and oxygen in the ratio of 127 g and 40 g by weight. If atomic weight of iodine and oxygen are 127 and 16 respectively, the formula of the compound will be :

(a) 12O3 (b) 12O4 (c) 12O5 (d) 12O

54. In an experiment, 1.0 g of lime stone (CaCO3) gave 224 cm3 of CO2 at NTP and 0.56 g of calcium oxide. These data illustrate the law of :

(a) Multiple proportion (b) Reciprocal proportion(c) Gaseous volume (d) Conservation of mass

55. A sample of Mg CO3 has 28.57% Mg, 14.29% C and 57.14% oxygen. If the law of constant proportion is true, then the weight of carbon in 2.1 g of MgCO3 from another source will be : (a) 0.1 g (b) 0.2 g (c) 0.3 g (d) 0.4 g

56. Two isotopes of 35 Cl and 37 Cl combine with sodium metal to form two samples of 17 17sodium chloride. These compound formation obey the law of :

(a) equivalents (b) multiple proportion(c) constant composition (d) None of these

57. 8.5 g of silver nitrate react with KCI solution to give 7.15 g silver chloride and 5.05 g KNO3. If the law of conservation of mass is obeyed, the weight of KCI used will be :

(a) 1.8 g (b) 3.7 g (c) 2.9 g (d) 10.6 g

58. Out of two oxides formed by a metal, 0.72 g of the lower oxide forms 0.8 g of higher oxide. If the higher oxide contains 80% metal, the data is true for the law of :(a) multiple proportion (b) combining weights(c) gaseous volume (d) constant composition

59. Out of the two unknown hydrocarbons, 0.052 g of one gave 95.8 cm3 of CO2 , 0.016g of the other produced 23.9 cm3 of CO2. If both experiments were done at 150C and 755 mm pressure, the data illustrates the law of :

(a) combining proportion (b) definite proportion(c) multiple proportion (d) gaseous volume

60. 3.0 g of ethane (C2H6) gave 5.4 g H2O and 8.8g CO2 on complete combustion in oxygen. The data is true for the law of :

(a) constant composition (b) multiple proportion (c) reciprocal proportion (d) conservation of mass

61. Some results of experiments are given below:

(a) In phosphorous chloride, P = 22.57%, Cl = 77.43%(b) In phosphine, P = 91.18%, H = 8.82%(c) In hydrogen chloride, H = 2.77%, Cl = 97.23%The law of combination that obeys the given results is :

(a) conservation of mass (b) reciprocal proportion (c) definite proportion (d) Gay Lussac’s law of gaseous volume

62. ‘x’ g of sulphur and ‘y’ g of oxygen are allowed to react in a closed vessel so that no solid sulphur is left behind. The ratio of weights of x and y is :

(a) 2:1 (b) 1:2 (c) 1:1 (d) 4:1

63. x g of an element A reacts with y g of an element B. Also, y g of element B combines with 2 z of C. If one gram equipment of B weighs y g, then the mass ratio in which A and C combine is :

(a) x:y (b) y:z (c) x:2z (d) y:2z

64. If the absolute temperature of a gas is doubled and the pressure is reduced to one half, the volume of gas will :

(a) remain unchanged (b) be doubled (c) increase four fold(d) be halved (e) be reduced to one fourth 65. To what temperature must a neon gas sample be heated to double the pressure, if the initial volume of the gas at 750C is decreased by 15%?

(a) 3190C (b) 5920C (c) 1280C (d) 600C (e) 900C

66. 2 g of O2 at 270C and 760 mm of Hg pressure has volume

(a) 1.5 lit. (b) 2.8 lit. (c) 11.2 lit. (d) 22.4 lit.

67. A certain sample of gas has a volume of 0.2 litre measured at 1 atm pressure and 00C. At the same pressure but 2730C, its volume will be :

(a) 0.4 litres (b) 0.8 litres (c) 27.8 litres. (d) 55.6 litres

68. One mole of monoatomic ideal gas at T (K) is expanded from 1 L to 2 L adiabetically under a constant external pressure of 1 atm. The final temperature of the gas in kelvin is :

(a) T (b) T __ (c) T - 2 (d) T + 3 25/3-1 3x0.0821 2x0.0821

69. The ratio of rate of diffusion of helium with respect to methane under similar conditions of constant temperature and pressure is :

(a) 2 (b) 0.5 (c) 16 (d) 4

70. The average and total kinetic energies of 0.5 mol of an ideal gas at 273 K are respectively in KJ mol¯ :

(a) 2.5x102;3.9 (b) 3.405;1.7025 (c) 5.0x10¯4;7.8 (d) 6.81;4.08

71. 1 mole of a N2O4(g) is kept in a container under 1.0 atmospheric pressure and 270C. It is heated to 3270C. As a result, 20% of N2O4(g) by mass decomposed to NO2(g). The resultant pressure is:

(a) 1 atm (b) 1.2 atm (c) 2.4 atm (d) 3.6 atm

72. Hydrogen gas diffuses from two different vessels X and Y. Vessel X has a circular orfice while vessel Y has a square orfice of length equal to the radius of the orfice vessel X. Assuming same temperature and pressure, the ratio of the rates of diffusion of H2 gas from vessel X to vessel Y is :

(a) 1 : 1 (b) 1 : 2 (c) 1 (d) ππ

73. The molecules of gas X more 3 times faster than those of gas Y at the same temperature. The ratio of the molecular weights Mx will be : My

(a) 1/10 (b) 1/9 (c) 1/8 (d) 7/1

74. Which of the following statement is false?

(a) The difference between rms velocity and mean velocity at any temperature for different gases diminishes as larger and yet larger molar masses are considered.(b) The square of the mean velocity of molecules is equal to square of the rms velocity at a certain temperature.(c) The ratio of the mean velocity to the rms velocity is independent of temperature.(d) The mean K.E. of the gas molecules at any given temperature does and depend on the mean velocity.

75. For identical conditions of temperature, the density of a gas A is three times that of gas B but the molar mass of gas B is two times that of gas A. The ratio of pressure of gases A and B is:

(a) 3 (b) 1 (c) 6 (d) 1 3 6

76. Pressure remaining constant, at what temperature, the volume of a gas at 00 C will be double of the volume?

(a) 1000C (b) 5460C (c) 273 K (d) 546 K

77. T = 550K, V=49.8 litre, n=2 mol, then the pressure will be (atm) :

(a) 2 (b) 4 (c) 1.5 (d) 2.5

78. If rms = 1000, the average velocity is :

(a) 920 (b) 820 (c) 1000 (d) 1020

79. Iodised table salt contains 7.6x10¯5 g of KI per gram of NaCI. The concentration in ppm in KI is :

(a) 76 (b) 152 (c) 500 (d) 760

80. 10 litre solution of urea contains 240 g urea. The active mass of urea will be :

(a) 0.02 (b) 0.04 (c) 0.2 (d) 0.4

81. For an ideal gas, number of moles per litre in terms of its pressure P, gas constant R and temperature T is :

(a) PT (b) RT (c) P (d) PRT R P RT

82. If 0.44 g of a colourless oxide of nitrogen occupies 224 mL at 1520 mm Hg and 2730C, then the compound is :

(a) NO (b) NO2 (c) N2O3 (d) N2O83. If the density of air at 298 K and 101.325 kPa is 1.161kg m¯3, then the average molar mass of air, assuming air behaves as an ideal gas is :

(a) 18 g mol¯ (b) 28 g mol¯ (c) 32 g mol¯ (d) 2 g mol¯

84. If the value of critical pressure and critical temperature are 72 atm and 300C respectively, the value of Vander Waal constant ‘a’ will be :

(a) 0.0432 L mol¯ (b) 3.628 L2atm mol¯2

(c) 0.0216 L mol¯ (d) 0.06 atm L2 mol¯2

85. The value of Vander Waal’s constant b for CO2 gas having critical pressure and critical temperature values 72.9 atm and 31.20C is :

(a) 0.342 L mol¯ (b) 0.342 L2 atm mol¯2

(c) 0.0428 L mol¯ (d) 0.0214 L mol¯

86. A real gas is supposed to obey the gas equation, P(V-b)=nRT at NTP. If one mole of a gas occupies 24 dm3 volume at NTP, the compressibility factor for the gas will be :

(a) 1.071 (b) 5.8 x 10¯3 (c) 2.9 x 10¯3 (d) 2

87. The temperature at which 2.5 mol of SO2 obeying the Vander Waal equation will occupy a volume of 12 litre at a pressure of 16 atm is :

(a) 788.69 K (b) 1061.690C (c) 2730C (d) 1061.69 K

88. The reduced temperature of oxygen at 370C if critical temperature of this gas is 155 K, will be :

(a) 0.2167 (b) 2 (c) 0.5167 (d) 48

89. The reduced pressure of a gas is 0.1604. If critical pressure is 45.6 atm, its pressure will be : (a) 3.5 x 10¯3 atm (b) 45.76 atm (c) 7.31 atm (d) None of these90. The number of potassium atoms required for the preparation of 0.2 MKMnO4 are:

(a) 2.408 x 1023 (b) 1.408 x 1023 (c) 2.4 x 1022 (d) 1.204 x 1023

91. The number of molecules in 4.49 L of a gas at 00C and 1 atmospheric pressure is approximately :

(a) 12.06 x 1023 (b) 12.06 x 1022 (c) 24.12 x 1022 (d) 24.12 x 1023

92. The percentage of sodium present is the cereal served in breakfast which is labeled to contain 110 mg of sodium per 100 g of cereal, is :

(a) 2% (b) 3% (c) 1% (d) 0.11%

93. The number of gram atoms of oxygen (atomic mass, 16 a.m.u.) in 8 g of oxygen, is

(a) 0.1 (b) 0.3 (c) 0.5 (d) 5.0

94. 0.01 mol of a compound weighs 1 g . The molecular mass of the compound is :

(a) 20 a.m.u. (b) 50 a.m.u. (c) 100 a.m.u. (d) 2.0 a.m.u.

95. Volume occupied by one molecule of water (density = 1 g cm¯3 ) is :

(a) 3.0 x 10¯23 cm3 (b) 5.5 x 10¯23 cm3 (c) 9.0 x 10¯23 cm3 (d) 6.023 x 10¯23 cm3

96. The number of atoms (x) of oxygen present in 88g of CO2 and (y) the mass of CO having same no. of oxygen atoms are :

(a) (x) 1024 (y) 100 g (b) (x) 2.408 x 1024 (y) 105g.(c) (x) 2.408 x 1024 (y) 112g. (d) None of these

97. The molecular mass of hydrogen chloride (HCI) having absolute density 1.63 g L¯, is :

(a) 3.651 g (b) 36.51 g (c) 18 g (d) 9 g

98. The weight of one litre of an unknown gas is 1.25 g at N.T.P. Which of the following gas pertains to the given data?

(a) N2 (b) N2O (c) N2O2 (d) N2O4

99. The minimum molecular weight of insulin containing 3.4% sulphur is :

(a) 941.176 g. mol¯ (b) 4703 g. mol¯ (c) 10.625 g. mol¯ (d) 106.25 g. mol¯

100. How many moles of lead (II) chloride will be formed from a reaction between 6.5 g of PbO and 3.2 g HCI?

(a) 0.011 (b) 0.029 (c) 0.044 (d) 0.333

101. If three elements, A, B and C crystallised in cubic solid lattice with A atoms at corners, B atoms at cube centre and C atoms at the edges, which formula of the compound is expected out of : (a) ABC3’ (b) ABC2’ (c) ABC, (d) AB3C,

102. The radius of A+ in ionic compound AB is 0.225 A. If AB has ZnS structure, the ideal radius of B- will be :

(a) 5.06 pm, (b) 50.6 pm, (c) 100 pm, (d) 150.6 pm,

103. A substance crystallises to f.c.c. lattice having 6Å edge length. If the density of unit cell is 2kg dm¯3, the molar mass of substance is :

(a) 51.65 g mol¯ (b) 25.8 g mol¯ (c) 76.4 g mol¯ (d) 65.04 g mol¯

104. An ionic compound AB crystallieses in b.c.c. lattice. If its unit cell edge length is 412 pm and radius of B¯ is 181 pm, the radius of A+ is :

(a) 200 pm (b) 175.8 pm (c) 351.6 pm (d) 100 pm

105. An XY ionic compound has zinc sulphide type structure. If the radius of Y ¯ is 100 pm, the radius of X+ will be :

(a) 45 pm (b) 0.225 Å (c) 120 pm (d) 2.25 Å

106. The number (n) of atoms in a cube when atoms are given on its own diagonal are :

(a) n (b) 2n (c) 3n (d) 4n

107. The number of atoms in a cubic based unit cell having one atom on each corner and two atoms on each body diagonal are :

(a) 1 (b) 2 (c) 3 (d) 4

108. How many unit cells are present in a cube shaped ideal crystal of NaCI of mass 1.00 g? (atomic masses, Na = 23, CI = 35.5).

(a) 1.71 x 1021 unit cells (b) 2.57 x 1021 unit cells (c) 5.14 x 1021 unit cells (d) 1.28 x 1021 unit cells

109. A binary solid (A+B-) has a zinc blende structure with B¯ ions constituting the lattice and A+ ions occupying 25% tetrahedral holes. The formula of solid is :

(a) AB3 (b) AB2 (c) AB4 (d) AB

110. The percentage of free space is a body centred unit cell is :

(a) 34% (b) 28% (c) 30% (d) 32%

111. The limiting radius ratio for tetrahedral shape is :

(a) 0.155 to 0.225 (b) 0.225 to 0.414 (c) 1.0 to 1.55 (d) 1.55 to 0.225

112. The number of octahedral sites for sphere in a cubic closest-packed (face-centred cubic) structure are :

(a) One (b) Two (c) Three (d) Four

113. A metal of atomic mass = 75 forms a cubic lattice of edge length 5Å and density 2 g cm¯3. The radius of atom (Avogadro’s number, NA = 6 x 1023) is :

(a) 217 pm (b) 100 pm (c) 217 Å (d) None of these

114. The volume of O2 required for the complete combustion of 120 cm3 of methane gas in a eudiometer tube will be :

(a) 60 cm3 (b) 120 cm3 (c) 240 cm3 (d) 360 cm3

115. The volume of Oxygen gas required for the complete combustion of 1.12 litre of ethene at 270C and 750 mm pressure will be :

(a) 1L (b) 2L (c) 2.3 L (d) 3.03 L116. A mixture of 25 mL nitric oxide and 25 mL of oxygen was sparked in a eudiometer tube. The volume of the gas left behind after treated with KOH solution would be : (a) 12.5 mL O2 (b) 25 mL O2 (c) 2.5 mL O2 (d) 2.5 mL NO2

117. 45 cm3 of O2 was mixed with 6 cm3 of a gaseous hydrocarbon and exploded in a eudiometer tube. After explosion, the volume was found to be 36 cm3 . After treatment with KOH solution, the volume was left as 18 cm3. The molecular formula of the hydrocarbon is :

(a) CH4 (b) C2H4 (c) C2H2 (d) C3H6

118. Of the following, the electromagnetic radiation with maximum wavelength is :

(a) Ultraviolet (b) Radiowaves (c) X-ray (d) Infra-red

119. Radius of second Bohr orbit of H-atom is …… times the first Bohr orbit of H-atom :

(a) 4 times (b) 2 times (c) 5 times (d) 3 times

120. Maximum number of orbitals in h subshell are :

(a) 16 (b) 11 (c) 13 (d) 10

121. For azimuthal quantum number, 1 = 2, the maximum number of electrons will be :

(a) 0 (b) 5 (c) 10 (d) 14

122. The radius of fifth orbit of the hydrogen atom is :

(a) 6.612 Å (b) 13.225 Å (c) 26.45 Å (d) None of these

123. The molarity of the original H3PO4 solution if 18.0 mL of H3PO4 solution is required to completely neutralise 35.0 mL of 0.045 M Ba(OH)2 is :

(a) 5.8 M (b) 0.058 M (c) 1.58 M (d) 2 M

124. The number of electrons in sulphur atom having n+1 = 3 are :

(a) 8 (b) 6 (c) 4 (d) 2

125. The orbital that has two angular nodal planes is :

(a) f (b) d (c) p (d) s

126. The ion which has the maximum magnetic moment is :

(a) Na+ (b) Fe3+ (c) Cr3+ (d) Sc3+

127. The wave number of the shortest wavelength transition in Lyman series of atomic hydrogen will be :

(a) 3647 Å (b) 109678 cm (c) 9.1x10¯6cm (d) 9.1 Å

128. When the frequency of light incident on a metallic plate is doubled, the kinetic energy of the emitted photoelectron will be :

(a) halved (b) unchanged (c) increase but more than double of the previous K.E. (d) doubled

129. The light energy required by the interior of human eye to see an object is 10¯17J. The number of photons of green light (λ=550 nm) required to see the object will be :

(a) 25 (b) 26 (c) 28 (d) 30

130. The number of d-electrons retained in Fe2+ (at. no. of Fe=26) ion is:

(a) 6 (b) 3 (c) 4 (d) 5

131. Assuming the velocity to be same, which of the following is associated with smallest de-Broglie wavelength?

(a) An electron (b) A proton (c) An alpha particle(d) All will have same wavelength

132. The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is : (a) 2 (b) 6 (c) 10 (d) 14

133. Least paramagnetic property is shown by :

(a) Fe (b) Mn (c) Ni (d) Cu

134. Which of the following is not permissible?

(a) n=4, 1=3, m=0 (b) n=4, 1=2, m=1(c) n=4, 1=4, m=1 (d) n=4, 1=0, m=0

135. Effective magnetic moment of Sc3+ ion is :

(a) 1.73 (b) 0 (c) 5.92 (d) 2.83 (d) 3.87

136. The ratio of charge and mass would be greater for :

(a) proton (b) electron (c) neutron (d) alpha particle

137. The number of radial nodes of 3s and 2p orbitals are respectively: (a) 2, 0 (b) 0, 2 (c) 1, 2 (d) 2, 1

138. Experimental dipole moment of HBr is 0.263 x 10─29 C.m. If bound length of H-Br is 1.41 Aº, the percentage of ionic character in H-Br is :

(a) 5.8% (b) 11.63% (c) 23.26% (d) 90%

139. The percentage ionic character of C-H bond in CH4 assuming the Pauli’s electronegativity value of C and H to be 2.5 and 2.1 respectively is :

(a) 3.34% (b) 6.68% (c) 4.99% (d) 6.96%

140. The covalent radius of double bonded oxygen atoms in CO2 is :

(a) 0.98 Aº (b) 0.32 Aº (c) 0.49 Aº (d) 4.9 Aº

141. The number of period to which an element with atomic number 21 belongs is :

(a) 1 (b) 2 (c) 3 (d) 4

142. The number of π electrons present in 2.6 g of ethyne are :

(a) NA (b) 2NA (c) 0.4 NA (d) 4 NA

143. Energy needed to convert 5.75 g Na-atom is gaseous state to form Na+ (g) is :

(a) 2829 kj (b) 28.29 kj (c) 123 kj (d) 282.9 kj

144. The hydrogen ion concentration of a solution having a pH value of 4.32 is :

(a) 4.79 x 10¯5 (b) 3.8 x 102 (c) 2 x 10¯6 (d) 11 x 10¯9

145. The electron affinity of CI when 1.0g of CI-atom is converted to CI ֿ (g) liberate 9.83 kj energy is :

(a) -349 kj (b) +349 kj (c) 35.5 kj (d) -35.5 kj

146. The bond length in CO is 1.128 Aº. What will be the bond length of CO in Fe(CO)5?

(a) 1.158 Aº (b) 1.128 Aº (c) 1.178 Aº. (d) 1.118 Aº.

147. Among the following, the paramagnetic compound is :(a) Na2O2 (b) O3 (c) N2 O (d) KO2

148. A 35.0 mL of sodium chloride solution is treated with excess of AgNO3 solution. As a result, 1.1 g of AgCl precipitate is formed. The molar concentration of NaCl is : (a) 0.44 M (b) 0.22 M (c) 0.11 M (d) 0.011M

(at.wt. Ag = 108, Cl 35.5)

149. The volume of 0.5 N HCI to react completely with 20 mL of 0.1 N NaOH will be :

(a) 40 mL (b) 4 L (c) 4.7 mL (d) 0.004 L

150. Volume of HBr required to neutralize 20 mL of 0.015 M Ca(OH)2 completely is : (a) 15 mL (b) 30 mL (c) 40 mL (d) 45 mL

151. Volume of 4.0 MHCI required to react completely with 25.2 g sodium bicarbon is : (a) 0.75 L (b) 0.075 mL (c) 75 mL (d) 7.5 mL

152. The final concentration of HCI if 0.15 mol HCI is added to a beaker containing 1.6 L of 1.75 M HCI and enough water to give a final volume of 3.5 L, is : (a) 0.84 M (b) 0.42 M (c) 0.21 M (d) 0.2 M

153. The weight of AgNO3 required to prepare 250 mL of a solution containing 50 mg of AgNO3 per mL will be : (a) 1.5 g (b) 11.5 g (c) 12.5 g (d) 25 g

154. How many g of concentrated nitric acid, containing 37.9% HNO3 by weight, will contain, 6.0 g HNO3 ? : (a) 6.6 g (b) 13.2 g (c) 19.8 g (d) 15.83 g

155. The mass of anhydrous HCI in 8.0 mL concentrated HCI [density 1.19 g (mL)¯ containing 37.9% HCI by weight will be : (a) 3.6 g (b) 7.2 g (c) 2.7 g (d) 36 g

156. The extent to which a solution of concentration 30 mg NaCI per mL be diluted to yield one mL of concentration of 12 mg NaCI per mL is : (a) 5 mL (b) 0.5 mL (c) 0.4 mL (d) 2.5 mL

157. The volume of dil. HCI (density 1.11 g/mL) and 18% HCI by weight and containing 8.0 g HCI, will be : (a) 30 mL (b) 1.29 mL (c) 40 mL (d) 30.3 mL

158. An ammonia solution (density 0.928 g/ml) containing 19% ammonia by weight was obtained when NH3 (g) was passed through water. The mass of ammonia per cm³ will be :

(a) 4.88 g (b) 0.18 g (c) 0.09 g (d) 2.44 g

159. The weight of NaCI required to make 50.0 mL of an aqueous solution containing 60.0 mg Na+ per mL will be :

(a) 76 g (b) 0.076 g (c) 7.6 g (d) None of these

160. The extent to which a solution containing 60 mg KCI per mL be diluted to give a solution of concentration 10 mg KCI per mL will be :

(a) 4 times (b) 5 times (c) 6 times (d) 600 times

161. 100 g CaCO3 is treated with 1 litre of 1NHCI. What would be the weight of CO2

liberated after the completion of the reaction.

(a) 5.5 g (b) 11 g (c) 22 g (d) 33 g (e) 44 g

162. The mass of carbon anode consumed (giving only carbon dioxide) in the production of 270 kg of aluminium metal from bauxite by Hall process is :

(a) 270 kg (b) 540 kg (c) 90 kg (d) 180 kg(at. mass. AI = 27)

163. Cyclohexanol is dehydrated to cyclohexene on heating with conc. H2SO4. If the yield of the reaction is 60%, the amount of cyclohexene obtained from 80 g of cyclohexanol will be :

(a) 0.4 g (b) 3.936 g (c) 393.6 g (d) 39.36 g

164. The volume in litre of CO2 produced at NTP when 8.4 g of 80% pure solution bicarbonate is heated completely is :

(a) 1.792 L (b) 0.896 L (c) 0.448 L (d) 0.224 L

165. Select the correct answer for the following : 27 g of AI will react completely with :

(a) 8 g (b) 16 g (c) 24 g (d) 32 g (e) 40 g of oxygen(AI = 27, O = 16)

166. What volume of oxygen gas (O2) measured at 0ºC and 1 atm, is needed to burn completely 1 L of propane gas (C3H8) measured under the same conditions :

(a) 5 L (b) 10 L (c) 7 L (d) 6 L

167. When 50 J heat is supplied to a system, the increase in internal energy of the system is 38 J. The work done by the system is :

(a) 98 J (b) + 12 J (c) - 12 J (d) None of these

168. An electric motor generates 20 kj energy per second as mechanical work. If 1.5 kj heat is lost to the surrounding, the change in internal energy of the motor will be :

(a) + 21.5 kj (b) - 21.5 kj (c) + 18.5 kj (d) 30 kj

169. 2 mol of a gas is allowed to expand freely in vacuum. The work done during the process will be :

(a) 2 kj (b) zero kj (c) - 2 kj (d) 4 kj

170. On supplying 250 j heat to a gas, its 2L volume at N.T.P. becomes 2.2 L at one atmosphere. The change in its internal energy would be :

(a) 302 J (b) 272.75 J (c) 229.75 J (d) 292.75 J

171. The work done to expand isothermally 1.6 g oxygen at 27ºC and 5 atmospheric pressure, against a constant external pressure of one atmosphere, is

(a) 99.76 J (b) -49.88 J (c) 49.88 J (d) -99.76 J

172. When work done by a system was 10 J, the increase in the internal energy of the system was 30 J. The heat ‘q’ supplied to the system was :

(a) - 40 J (b) + 20 J (c) 40 J (d) - 20 J

173. The work done when 10g of zinc reacts with dil H2SO4 in a closed vessel of fixed volume is :

(a) 10 J (b) 1.0 J (c) zero J (d) none of these

174. The work done when 6.5 g of zinc reacts with dil. HCI is an open beaker at 298 K is :

(a) - 495.52 J (b) 247.76 J (c) - 247.76 J (d) - 123.88 J

175. The work done in heating one mol of an ideal gas as constant pressure from 15ºC to 25ºC is :

(a) 1.987 cal (b) 198.7 cal (c) 9.935 cal (d) 19.87 cal

176. One mol of a gas was expanded isothermally and reversibly at 17ºC from 2 atm to some other pressure P. If 200 cal work is used in causing reversible isothermal expansion then final pressure P will be :

(a) 2.84 atm (b) 1.42 atm (c) 4.26 atm (d) none of these

177. If specific heat, heat of fusion and heat of vaporisation of water are 1 cal g¯, 80 cal g¯ and 540 cal g¯ respectively then heat required to concert 5.0 g of ice at 0ºC to steam at 100ºC would be nearly :

(a) 7.53 J (b) 7.53 kj (c) 15.06 kj (d) 30.12 kj

178. The entropy change to expand 2 mol of an ideal gas at 27ºC, reversibly 6 times of its initial volume is :

(a) 14.9 JK¯ (b) 29.8 JK¯ (c) 44.77 JK¯ (d) 20 JK¯

179. The entropy change during heating of 50g water (sp. heat = 4200 J kg¯K¯) from 20ºC to 40 ºC will be :

(a) 13.83 JK¯ (b) - 13.83 JK¯ (c) 27.66 JK¯ (d) 55.32 JK¯

180. The heat capacities of water and pressure cooker metal are 1k cal(kg)¯K¯ and 0.09 k cal (kg)¯K¯ respectively. The actual heat required to raise the temperature of water (750g) from 27ºC to 110ºC in this cooker weighing 5 kg is :

(a) 58.59 k cal (b) 55.59 k cal (c) 1.2 k cal (d) 117.18 k cal

181. One mole of an ideal gas is allowed to expand reversibly and adiabetically from temperature of 27ºC. If the work done during the process is 3 kJ, the final temperature will be equal to (Cv = 20 JK¯

(a) 100 K (b) 150 K (c) 295 (d) 26.85ºC

182. The heat of combustion of solid benzoic acid at constant volume is – 312.30kJ at 27ºC. The heat of combustion at constant pressure is :

(a) 100 - R (b) 200 – 2R (c) – 321.3 – 150 R (d) 321.3 + 150R

183. Work done on a system when one mole of an ideal gas at 500 K is compressed isothermally and reversibly to 1/10th of its original volume (R=2 cal).

(a) 1 kJ (b) 2.303 kJ (c) 4.606 kJ (d) 2.303 J

184. The heat of neutralization of a strong base and strong acid is 57.0 kJ. The heat released when 0.5 mol of HNO3 solution is added to 0.2 mol of NaOH solution is :

(a) 5.7 kJ (b) 5.7 J (c) 11.4 kJ (d) 11.4 J

185. One mole of an ideal gas freely and isothermally at 300 K from 5 litre to 10 litre if ∆E = 0, the ∆H is :

(a) 1 (b) 2 (c) 3 (d) zero

186. Two moles of an ideal gas at 2 atmospheric pressure and 27ºC is compressed isothermally to half its volume by external pressure of 4 atmosphere. The work done is : :

(a) 2.345 kJ (b) 2.456 J (c) 4.985 kJ (d) 7 kJ

187. For equilibrium reaction, value of Gibb’s free energy change is :

(a) > 0 (b) < 0 (c) = 0 (d) ≠ 0

188. The sublimation energy of I2(s) is 57.3 kJ/mol and the enthalpy of fusion is 15.5 kJ/mol. The enthalpy of vaporisation of I2 is :

(a) 41.8 kJ/mol (b) - 41.8 kJ/mol (c) 72.8 kJ/mol (d) -72.8 kJ/mol

189. What would be the heat released when an aqueous solution containing 0.5 mole of HNO3 is mixed with 0.3 mol of OH¯ (enthalpy of neutralisation = - 57.1 kJ ) ?

(a) 28.5 kJ (b) 17.1 kJ (c) 45.7 kJ (d) 1.7 kJ (e) 2.85 kJ

190. Which of the following is always negative for exothermic reaction ?

(a) ∆H (b) ∆S (c) ∆G (d) None of these

191. Given the bond energies of N≡N, H-H, N-H bonds are 945, 436 and 391 kJ/mol respectively. The enthalpy of the reaction, N2(g) + 3H2(g) → 2NH3(g) is :

(a) -93 kJ (b) 102 kJ (c) 90 kJ (d) 105 kJ

192. If heats of combustion of red phosphorus and yellow phosphorus are – 8.78 kJ and – 9.19 kJ respectively, then heat of transition of yellow phosphorus to red phosphorus will be :

(a) 17.97 kJ (b) - 17.97 kJ (c) - 1.13 kJ (d) + 1.13 kJ

193. Heat capacity of liquid water at constant pressure, Cp is 18 cal deg¯ mol¯. The value of heat capacity of water at constant volume, Cv is approximately:

(a) 18 cal deg¯ mol¯ (b) 16 cal deg¯ mol¯(c) 10.8 cal deg¯ mol¯ (d) cannot be predicted

194. The enthalpy and entropy change for the reaction Br2(l) + Cl2(g) → 2BrCl(g) are 30 kJ mol¯ and 105 J mol¯ respectively. The temperature at which the reaction will be in equilibrium is :

(a) 300 K (b) 285.7 K (c) 273 K (d) 450 K

195. In alkaline medium,ClO2 oxidises H2O2 to O2 and itself gets reduced to Cl¯ . How many moles of H2O2 are oxidized by 1 mole of CIO2?

(a) 1.0 (b) 1.5 (c) 2.5 (d) 3.5 (e) 5.0

196. The oxidation state of chromium in the final product formed by the reaction between KI and acidified potassium dichromate solution is :

(a) +4 (b) +6 (c) +2 (d) +3

197. Oxidation state of oxygen in potassium superoxide is :

(a) -1/2 (b) -1 (c) -2 (d) 0

198. The oxidation number of carbon in carbon suboxide is :

(a) +2/3 (b) +4/3 (c) +4 (d) -4/3

199. In rhombic sulphur, the oxidation number, atomicity and valency of sulphur are :

(a) 0, 2, 8 (b) 0,8,2 (c) 2, 8,2 (d) 2, 1,8

200. In the reaction, Cu + 2H2SO4→ CuSO4 + SO2 + 2H2O, H2SO4 acts as :

(a) Catalyst (b) reductant (c) oxidant (d) oxidant as well as an acid

201. The oxidation number of N in hydrazine is : (a) +2 (b) 0 (c) -1 (d) -2

202. A metal ion M3+ after loss of three electrons in a reaction will have an oxidation number equal to :

(a) zero (b) +2 (c) +3 (d) +6

203. Oxidation number of O in O3 is :

(a) 3 (b) -2 (c) zero (d) -6 204. The oxidation number of H in CaH2 is :

(a) +2 (b) -2 (c) +1 (d) -1

205. The oxidation number of Nitrogen in N3H is :

(a) +1/2 (b) +3 (c) -1 (d) -1/3

206. Oxidation number of oxygen is potassium Peroxide is :

(a) zero (b) -1/2 (c) -1 (d) -2 207. Oxidation number of Mn in KMnO4 is :

(a) +7 (b) -7 (c) +1 (d) -1 208. Oxidation state of chlorine in perchloric acid is :

(a) -1 (b) 0 (c) -7 (d) +7 209. The oxidation number of carbon in CH2O is :

(a) -2 (b) +1 (c) 0 (d) +4

210. 0.1M NH4OH solution is 1.34% dissociated. Its Kb value will be :

(a) 1.8 x 10¯4 (b) 2.9 x 10¯5 (c) 1.8 x 10¯5 (d) 1.8 x 10¯12

211. Oxidation state of oxygen in hydrogen peroxide is :

(a) -1 (b) +1 (c) 0 (d) -2

212. The oxidation state of Cr is K2Cr2O7 is :

(a) +6 (b) -7 (c) +2 (d) -2

213. Oxygen has an oxidation state of + 2 ins :

(a) H2O2 (b) H2O (c) OF2 (d) SO2

214. The oxidation number of phosphorus in Ba(H2PO2) 2 is :

(a) +3 (b) +2 (c) +1 (d) -1215. Consider a titration of potassium dichromate solution will acidified Mohr’s salt solution using diphenylamine as indicator. The number of moles of Mohr’s salt required per mole of dichromate is :

(a) 3 (b) 4 (c) 5 (d) 6

216. In a 0.2 molal aqueous solution of a weak acid HX, the degree of ionisation is 0.3. Taking Kf for water as 1.85, the freezing point of the solution will be nearest to :

(a) + 0.480 °C (b) - 0.481 °C (c) - 0.360 °C (d) - 0.260 °C

217. A solution of urea (mol mass 56 g mol¯) boils at 100.18 °C at the atmospheric pressure. If Kf and Kb for water are 1.86 and 0.512 K kg mol¯ respectively, the above solution will freeze at :

(a) 0.654 °C (b) - 0.654 °C (c) 6.54 °C (d) - 0.6.54 °C218. The vapour pressure of two liquids P and Q are 80 and 60 torr, respectively. The total vapour pressure of solution obtained by mixing 3 mol of P and 2 mol of Q are :

(a) 72 torr (b) 140 torr (c) 68 torr (d) 20 torr

219. The mole fraction of the solute in one molal aqueous solution is :

(a) 0.009 (b) 0.018 (c) 0.027 (d) 0.036

220. A solution is prepared by dissolving 17.1 g of sucrose to make 1000 mL of solution in water. The osmotic pressure of the solution at 20 °C is :

(a) 1.203 atm (b) 1.203 mm (c) 1.203 cm (d) 20 atm

221. The number of equivalents in 1 mol of H2SO4 are : 20

(a) 0.01 (b) 0.1 (c) 0.05 (d) 0.5

222. The number of equivalents in 250 mL of N H2SO4 are : 20

(a) 1.25 (b) 0.125 (c) 12.5 (d) 0.0125

223. The number of equivalents in 125 milliequivalents of HNO3 are : (a) 125 (b) 12.5 (c) 1.25 (d) 0.125

224. The molarity of N sodium bicarbonate solution is : 10

(a) 0.1 (b) 0.2 (c) 0.01 (d) 0.02

225. Number of millilitre of 0.25 M H2SO4 required to dissolve 2.1 g magnesium carbonate (at.wt.,Mg = 24, C=12, O=16) is : (a) 200 mL (b) 100 mL (c) 50 mL (d) 20.0 mL

226. The boiling point of an aqueous solution containing 10 g of urea (molar mass = 60) in 250 g of water (Lv = 539 cal g ¯), will be : (a) 373.34 K (b) 350.17 0C (c) 273 0C (d) 274 K

227. 10 g of glucose are dissolved in 150 g of water. The mass percentage of glucose is : (a) 2.25% (b) 6.25% (c) 7.50% (d) 2.22%

228. The number of moles of H2SO4 in which mole fraction of water is 0.85 are :

(a) 8.9 (b) 9.8 (c) 8 (d) 9

229. Which has minimum osmotic pressure?

(a) 200 mL of 2 M NaCI solution (b) 200 mL of 1 M glucose solution(c) 200 mL of 2 M Urea solution (d) All have same

230. If a is the degree of dissociation of Na2SO4 , the Van’t Hoff’s factor (i) used for calculating the molecular mass is :

(a) 1 + α (b) 1 – α (c) 1 + 2 α (d) 1 – 2 α

231. The mass of NaOH in its 40 milliequivalents is :

(a) 6.1 g (b) 1.6 g (c) 6.2 g (d) 2.6 g

232. One atom of an element weighs 3.819 x 10¯23 g. The number of gram atoms in 46 kg of it will be :

(a) 500 g atom (b) 1000 g atom (c) 2000 g atom (d) 3000 g atom

233. The milliliter of 0.4M H2SO4 used to dissolve 1.2 g of CuCO3 will be :

(a) 2.01 (b) 4.001 (c) 28.1 (d) 24.3

234. The number of oxalic acid molecules in 250 cm3 of 0.02N oxalic acid will be :

(a) 2.5 x 1022 (b) 3.0 x 1023 (c) 2.1 x 1020 (d) 1.5 x 1021

235. 25 mL of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a titre value of 35 mL. The molarity of Ba (OH) 2 solution was :

(a) 0.35 (b) 0.07 (c) 0.14 (d) 0.28

236. A 0.01 molar solution of KI is found to be isotonic with 0.019 molar solution of urea. The apparent degree of ionization of KI will be :

(a) 70% (b) 80% (c) 90% (d) 45%

237. 0.1 molar solution of phenol in water exhibits an osmotic pressure of 1.88 atm at 27 °C. The degree of association of phenol in water, if it is assumed that phenol forms a double molecule in water is :

(a) 23.67% (b) 11.84% (c) 47.34% (d) 94.68%

238. What is the normality of 1 M solution of H3PO4 ?

(a) 0.33 N (b) 1.0 N (c) 2.0 N (d) 3.0 N

239. The osmotic pressure of 1 M sodium chloride solution at 27 °C is :

(a) 12.3 atm (b) 24.6 atm (c) 39.8 atm (d) 49.2 atm

240. The concentration of glucose solution in molality which boils at 100.01 °C (Kb for water is 0.5 °C kg mol¯) is :

(a) 0.01 (b) 0.02 (c) 0.03 (d) 0.04

241. A solution containing 10 g per dm3 of urea (molecular mass = 60 g mol¯) is isotonic with a 5% solution of a non volatile solute whose molar mass is :

(a) 200 g mol¯ (b) 250 g mol¯ (c) 300 g mol¯ (d) 350 g mol¯

242. The osmotic pressure of a 0.10 M solution of a non – electrolyte at 0 °C is :

(a) 1.12 atm (b) 2.24 atm (c) 3.36 atm (d) 3.36 mm

243. Density of a 2.05 M solution of acetic acid in water is 1.02 g/mL. The molality of the solution is :

(a) 1.14 mol kg¯ (b) 3.28 mol kg¯ (c) 2.28 mol kg¯ (d) 0.44 mol kg¯

244. 18 g of glucose (C6H12O6) is added to 178.2 g of water. The vapour pressure of this water for this aqueous solution at 100 °C :

(a) 759.00 torr (b) 7.60 torr (c) 76.00 torr (d) 752.3 torr

245. At some temperature, which pair of the following solutions are isotonic solutions?

(a) 0.2 M BaCI2 and 0.2 M urea (b) 0.1 M urea and 0.1 M NaCI(c) 0.1 M NaCI and 0.1 M K2SO4 (d) 0.1 M Ba(NO3)2 and 0.1 M Na2SO4

246. When 20 g of naphthoic acid (C11 H8O2) is dissolved in 50 g of benzene (KF = 1.72 K kg mol¯), a freezing point depression of 2 K is observed. The Van’t Hoff factor (i) is :

(a) 0.5 (b) 1 (c) 2 (d) 3

247. If the conductance and specific conductance of a solution is same, then its cell constant is equal to :

(a) Zero (b) 1 (c) 2 (d) 3

248. The specific conductance of a salt of 0.01 concentration is 1.061 x 10¯4. Molar conductance will be : (a) 1.061 x 10¯4 (b) 1.061 (c) 10.61 (d) 106.1

249. The resistance of a cell (cell constant = 1.1 cm¯1) containing N KCI was found to be 400 50

ohms. The equivalent conductivity of KCI at this dilution is :

(a) 68.75 ohm¯ (b) 437.5 ohm¯ (c) 200 cm¯ (d)137.5 ohm¯ cm2 (g.equiv)¯

250. When an electric current is passed through dil. H2SO4, the gases liberated at anode and cathode are :

(a) H2 and O2 respectively (b) O2 and H2 respectively (c) SO2 and O2 respectively (d) SO2 and O2 respectively

251. The coulombs of electricity consumed when 60 mA current is passed through a solution of silver nitrate for 20 minutes are :

(a) 2 C (b) 6 C (c) 72 C (d) None of these

252. Being unstable, Cu+ undergoes disproportionation. E0 for Cu+ disproportionation is :

(a) - 0.367 V (b) + 0.377 V (c) - 0.726 V (d) + 0.666 V

253. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is :

(a) 150 (b) 100 (c) 50 (d) 5.0

254. In a solution of CuSO4’ how much time will be required to precipitate 2g copper by 0.5 ampere current?

(a) 12100 sec (b) 12157.48 sec (c) 104 sec (d) 105 sec.

255. The volume of H2 gas at N.T.P. obtained by passing 4 amperes through acidified H2O for 30 minutes is : (a) 0.0836 L (b) 0.0432L (c) 0.1672 L (d) 0.836 L

256. Conductance (unit siemen’s S) is directly proportional to area of the vessel and the concentration of the solution in it and is inversely proportional to the length of the vessel, then the unit of constant of proportionality is :

(a) Sm mol¯ (b) S2m2 mol¯2 (c) Sm¯2 mol¯ (d) S¯2m2 moL.

257. How many coulombs of electricity are consumed when a 100 mA current is passed through a solution of AgNO3 for half an hour during an electrolysis experiment?

(a) 108 (b) 18,000 (c) 180 (d) 3000

258. How much silver will be displaced by that quantity of current which displaces 5.6 L of H2 :

(a) 13.5 g (b) 20 g (c) 54 g (d) 168 g

259. What is the number of coulombs required for the conversion of one mol of MnO¯4 to one mol of Mn

2+ ?

(a) 96500 (b) 96500 x 3 (c) 96500 x 5 (d) 96500 x 7

260. When electricity is passed through aqueous solution of aluminium chloride, 13.5 g of AI are deposited. The number of Faradays of electricity passed must be : (a) 2.0 (b) 1.5 (c) 1.0 (d) 0.5

261. What would be the weight of deposited silver on passing 965 coulombs of electricity in a solution of silver nitrate?

(a) 1.08 g (b) 2.16 g (c) 0.54 g (d) 0.27 g

262. What is the amount of chlorine evolved when 2 amperes of current is passed for 30 minutes in an aqueous solution of NaCI ?

(a) 66 g (b) 1.32 g (c) 33 g (d) 99 g

263. A galvanic cell was set up from zinc rod (= 100 g) and 1L of 1 M CuSO 4 solution. If the cell delivers a steady current of one ampere, the time for which the cell would work is :

(a) 5.36 hr (b) 2.68 hr (c) 26.8 hr (d) 53.6 hr

264. How many grams of copper will be deposited from a solution of CuSO4 by passing 0.5 F of electric current?

(a) 31.75 (b) 63.5 (c) 15.875 (d) 127

265. How many electrons are in one coulomb?

(a) 6.023 x 1023 (b) 1.64 x 10¯24 (c) 6.24 x 1018 (d) 6.24 x 10¯24

266. The value of potential of a hydrogen electrode, pH = 10 is :

(a) 0.4 V (b) - 0.4 V (c) - 0.3 V (d) - 0.591 V

267. When 9.65 coulombs of electricity is passed through a solution of silver nitrate (at. Mass of Ag = 108 amu), the amount of silver deposited is :

(a) 10.8 mg (b) 5.4 mg (c) 16.2 mg (d) 21.2 mg

268. 1A current is supplied for 30 minutes through NaCL. How much chlorine will be liberated ?

(a) 0.66 gm (b) 0.66 mol (c) 0.33 g (d) 0.33 mol

269. The current strength in amperes that is required to liberate 10 g of iodine from KI solution in 1 hour will be :

(a) 1.05 (b) 2.1 (c) 13.9 (d) 1.12

270. Specific conductance has the unit

(a) Ohm¯ cm (b) Ohm¯ cm2 (c) Ohm¯ cm¯ (d) Ohm cm

271. The rate of reaction, A + B → products is given by the equation, r = k[A][B]. If B is taken in large excess, the order of reaction would be :

(a) 1.5; (b) 2.5; (c) 1; (d) unpredictable

272. For a first order reaction A → B, the reaction rate at reactant concentration of 0.01 M is found to be 2.0 x 10¯5 mol L¯s¯ . The half-life period of the reaction is :

(a) 30s; (b) 220s; (c) 300s; (d) 347s

273. The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is :

(a) 2; (b) -2; (c) 1; (d) -1

274. For the reaction A → B, the rate of reaction is quadrupled when the concentration of A is doubled. The rate expression of the reaction is r = k[A]n when the value of n is :

(a) 1 (b) zero (c) 3 (d) 2

275. For a first order reaction, we have k = 100 sec¯. The time for completion of 50% reaction is :

(a) 1 m sec; (b) 4 m sec; (c) 7 m sec; (d) 10 m sec

276. The rate of reaction between A and B increases by a factor of 100, when the concentration of A is increased 10 folds. The order of reaction with respect to A is:

(a) 10; (b) 1; (c) 3; (d) 2

277. If a plot of log10(t1/2) Vs log10a gives a straight line with a slope of -1, the order of reaction would be:

(a) 0; (b) 1; (c) 2; (d) 3

278. Plot of log C (concentration) as a function of time gives a straight line for a first order reaction. The slope of this line gives:

(a) k; (b) 1/k; (c) -k; (d) -1/k

279. A reaction that is of first order with respect to reactant A has rate constant 6min¯. If we start with [A]=0.5 mol L¯, when would [A] reach the value 0.05 mol L¯?

(a) 0.15min; (b) 0.384min; (c) 3.84min; (d) 3min

280. A reaction was found to be of second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled with everything else kept the same, the rate of reaction will:

(a) remain unchanged; (b) be tripled; (c) increase by a factor of 4; (d) be doubled

281. Consider a reaction a G + b H→ Products. When concentration of both the reactants G and H is doubled , the rate increases eight times. However, when concentration of G is doubled, keeping the concentration of H fixed, the rate is doubled . The overall order of the reaction is:

(a) 0; (b) 1; (c) 2; (d) 3

282. An element E has a half-life of 10 years. The time taken to reduce its activity to about 1/8 of its original value will be:

(a) 80 years (b) 1.25 years (c) 10 years (d) 30 years

283. One of the following is not an isoelectronic species:

(a) Ar, K+ (b) H¯ , He (c) CO2 , CN¯ (d) CNO¯ , N2O

284. A substance has half-life period of 4 sec. After t=20sec, how much percentage of substance is destroyed?

(a) 96.87 (b) 3 (c) 40 (d) 50

285. A radioactive isotope having a half-life of 3 days was received after 12 days. It was found that there were 3g of the isotope in the container. The initial weight of the isotope when packed was :

(a) 48g (b) 36g (c) 24g (d) 12g

286. If the mass of Co-59 = 58.9332, the value of its packing fraction will be:

(a) +11.322 (b) -11.322 (c) +5.661 (d) -5.661

287. The mass number of a nucleide is 64. What is its nuclear radius in Fermi?

(a) 2.8 Fermi (b) 1.4 Fermi (c) 5.6 Fermi (d) 11.2 Fermi

288. A radioactive isotope decays at such a note that after 90 minutes, only 1/16 th of the original amount is left behind. The half-life of this nucleide is :

(a) 33 min (b) 66 min (c) 23.1 min (d) 46.2 min

289. The loss in mass accompanying combustion of one mol of fuel to release 900 kj heat energy is :

(a) 2 x 109 kg (b) 2 x 1011 kg (c) 3 x 1011 kg (d) 1011 kg

290. The half-life of a radioactive element in 4.8 min. The time taken by a given sample of the element to reduce to 1/4th of its initial activity will be :

(a) 4.8 min (b) 9.6 min (c) 19.2 min (d) 1 hour

291. A radioactive substance decays at such a rate that after 35 minutes, only a quarter of the original substance is left behind. The disintegration constant and half-life of the radio-isotope are :

(a) 0.0396 min¯, 17.5 min (b) 1.2 min¯, 10 min (c) 2.4 min¯, 20 min (d) 0.003 min¯, 1 min

292. The half-life of a radioactive isotope is three hours. If the initial mass of the isotope was 256 g, the mass of it remaining undecayed after 18 hours would be :

(a) 16.0 g (b) 4.0 g (c) 8.0 g (d) 12.0 g

293. In the first order reaction, the concentration of the reactants is reduced to 25% in one hour. The half-life period of the reaction is :

(a) 30 seconds (b) 30 minutes (c) 1.5 hr (d) 2.5 hr

294. The half-life of a first order reaction is 60 sec. The percentage of reactant left after 3 minutes is :

(a) 2.5 (b) 25 (c) 12.5 (d) 1.25

295. The half-life period of polonium is 140 days. If one starts with 1 g of polonium, 75% of it would have undergone disintegration in :

(a) 28 days (b) 280 days (c) 560 days (d) 1 year

296. The radius of nucleus of fluorine-19 is :

(a) 3.7 x 10¯15 m (b) 7.6 x 10¯12 m (c) 2.1 x 10¯15 m (d) 7.6 x 10¯10 m

297. The loss in mass accompanying the combustion of one mol of a given fuel that yields 800 kj of heat energy is :

(a) 4.4 x 10¯12 kg (b) 2.2 x 1011 kg (c) 8.89 x 10¯12 kg (d) 3.2 x 10¯13 kg

298. If the amount of radioactive substance is increased three times, the number of atoms disintegrated per unit time would :

(a) be doubled (b) be tripled (c) remain one-third (d) not change

299. The half-life of a radioactive element is 30 minutes. One sixteenth of the original quantity of the element will remain unchanged after :

(a) One hour (b) 16 hours (c) 4 hours (d) 2 hours

300. A radioactive sample has half-life of 1500 years. A sealed tube containing 1 g of the sample will contain after 3000 years :

(a) 1 g of the sample (b) 0.5 g of the sample (c) 0.25 g of the sample (d) 0.00 g of the sample

301. The half-life of a radionucleide ‘X’ is 24 hours. The time required for 12.5% of the original X to remain is :

(a) 1 day (b) 2 days (c) 3 days (d) 4 days

302. 1.0 g of radioactive isotope was found to reduce to 125 mg after 24 hours. The half-life of the isotope is :

(a) 8 hrs (b) 24 hrs (c) 6 hrs (d) 4 hrs

303. The half-life of a radioisotope is four hours. If the initial mass of the isotope was 200 g, the mass remaining after 24 hours undecayed is :

(a) 1.042 g (b) 2.084 g (c) 3.125 g (d) 4.167 g

304. The half-life of a radioactive isotope is three hours. If the initial mass of isotope was 300 g, the mass that remained undecayed in 18 hours would be :

(a) 2.34 g (b) 1.17 g (c) 9.36 g (d) 4.68 g

305. A human body required 0.01 M activity of a radioactive substance after 24 hours. Half-life of the radioactive substance is 6 hours. The injection of maximum activity of the radioactive substance that can be injected to :

(a) 0.08 (b) 0.04 (c) 0.16 (d) 0.32

306. A radioactive isotope decays at such a rate that after 192 minutes only 1/16 of the original amount remains. The half-life of the radioactive isotope is :

(a) 32 min (b) 48 min (c) 12 min (d) 24 min

307. What is the half-life of a radioactive substance if 87.5% of any given amount of the substance disintegrates in 40 minutes?

(a) 10 min (b) 20 min (c) 160 min (d) 13 min 20 sec.

308. The half-life of an isotope is 10 hrs. How much will be left after 4 hrs in one gram mole sample?

(a) 45.6 x 1023 atoms (b) 4.56 x 1023 atoms(c) 4.56 x 1021 atoms (d) 4.56 x 1020 atoms

309. Which of the following has maximum N/p ratio ?

(a) 16 Ne (b) 16 O (c) 16 F (d) 16 N

310. A first order reaction is 10% complete in 20 minutes. The time taken for 19% completion is :

(a) 30 min (b) 40 min (c) 50 min (d) 38 min (e) 45 min

311. The equivalent weight of N/1.75 H2SO4 solution containing 3.5 g/125 mL is :

(a) 98 (b) 49 (c) 24.5 (d) 12.75

312. The strength of 1.5 N HNO3 in gram equivalents per litre is :

(a) 0.152 (b) 1.68 (c) 6.1 (d) 1.5

313. The number of gram mol of 2.0 L of 3 M H2SO4 are :

(a) 2.0 (b) 3.0 (c) 6.0 (d) None of these

314. The molarity of sulphuric acid [sp. gr. 1.249 g (mL)¯] containing 98% by weight of sulphuric acid is :

(a) 1.4 M (b) 2.8 M (c) 6.245 M (d) 12.49 M

315. The normality of a solution prepared by diluting 100 cm3 of 0.25 N H2SO4 with 1000 cm3

of water would be :

(a) 0.0227 N (b) 1.12 N (c) 0.09 N (d) none of these

316. 10 mL of 1 M NaOH solution will neutralise :

(a) 2.5 mL (b) 5 mL (c) 10 mL (d) 20 mL of 1 M H2SO4

317. The equivalent weight of a metal carbonate, 0.84 g of which react exactly with 40 mL of N/2 sulphuric acid is :

(a) 21 (b) 42 (c) 84 (d) 8.4

318. A 1.0 g sample of H2O2 solution containing x per cent H2O2 by weight requires x mL of a KMnO4 solution for complete oxidation under acidic conditions. The normality of KMnO4

solution is :

(a) 0.588 N (b) 1.16 N (c) 0.244 N (d) 0.1 N

319. The amount of NaOH required to neutralize 25 Meq of the following :

(i) CO2 (ii) HCl (iii) NaHSO4 is :

(a) 0.5g (b) 1.0 g (c) 1.5 g (d) 2.0 g

320. If density of water is 1000 kg m¯3 , the molarity of water will be :

(a) 18 (b) 5.6 (c) 55.6 (d) none of these

321. An aqueous solution of KOH (6.9 M) contains 30% KOH by weight. The density of solution will be :

(a) 0.6 g (mL)¯ (b) 2.4 g mL¯ (c) 0.23 g (mL)¯ (d) 1.288 g (mL)¯

322. The volume of a solution of HCI containing 73 g of acid per litre that would suffice for the exact neutralization of sodium hydroxide obtained by allowing 0.46 g of metallic sodium to act upon water is :

(a) 2 mL (b) 5 ml (c) 10.0 mL (d) 15.0 mL

323. A sample of Na2CO3H2O weighing 0.62 g is added to 100 mL of 0.1 N H2SO4. The resulting solution will be :

(a) Acidic (b) Basic (c) neutral

324. 0.1 M KMnO4 is used for the following titration. The volume of solution in mL required to react with 0.158 g of Na2S2O3 will be :

(a) 26.67 mL (b) 2.4 mL (c) 24 mL (d) 2.7 mL

325. The magnitude of equilibrium constant, K for any reaction is affected by changing: -

(a) Catalyst (b) Concentration of reactant species(c) Temperature (d) Concentration of products.

326. If Henry’s law constant for O2 is 1.28 x 10¯3 mol L¯ atm¯, the solubility of O2 in water at a partial pressure of O2 of 190 torr at 298 K will be :

(a) 1.6 x 10¯4 mol L¯ (b) 3.2 x 10¯4 mol L¯(c) 4.8 x 10¯6 mol L¯ (d) 10¯5 mol L¯ only

327. One mol of NH3 was heated in presence of a catalyst in a half-litre capacity vessel to get equilibrium. The resultant mixture contained 0.7 mol of NH3. The equilibrium constant at the temperature of experiment will be :

(a) 0.1 (b) 0.2 (c) 0.8 (d) 0.33

328. 1 mol of N2O4 is heated in a flask with a volume of 10 dm3. At equilibrium, 1.708 mol of NO2 and 0.146 mol of N2O4 were found at 407 K. The equilibrium constant value will be :

(a) 200 mol¯3 dm (b) 2.0 mol dm¯3

(c) 100 mol dm ¯3 (d) 50 mol dm ¯3

329. A closed vessel contains one mol of N2O4(g) at 270C and one atmospheric pressure. On heating to 3270C, 20% by mass of this gas decomposed to brown coloured NO2 (g). The resultant pressure will be :

(a) 0.24 atm (b) 2.4 atm (c) 0.024 atm (d) 0.48 atm

330. The dissociation constant of N2O4 if it dissociates to the extent of 53% at 600C and one atmospheric pressure will be :

(a) 2.39 (b) 9.32 (c) 239 (d) 23.9

331. One mol of acetic acid and one mol of ethyl alcohol were mixed at 298 K. At equilibrium, 0.333 mol of acetic acid was found unreacted. The value of equilibrium constant will be :

(a) 2.006 (b) 4.012 (c) 12.036 (d) 1.003

332. 0.12 mol of PCl3 are mixed with 0.9 mol of PCI5 in a one litre vessel. The vessel contains 0.72 mol of PCI5 at equilibrium. The value of Kc for the reaction is : (a) 0.1 mol L¯ (b) 0.04 mol L¯ (c) 0.075 mol L¯ (d) 0.75 mol L¯

333. Phosphorus penta chloride is 82% dissociated into phosphorus trichloride and chlorine, all gaseous at 2500C and 1 atmospheric pressure. The equilibrium constant of dissociation is :

(a) 2.577 (b) 3.577 (c) 0.202 (d) 2.05

334. A container contains CO2 gas at 0.5 atm pressure and 1000K. On the addition of some graphite, some of the CO2(g) converted into carbon monoxide. If total pressure at equilibrium is 0.8 atm, the value of equilibrium constant will be :

(a) 0.8 atm (b) 1.8 atm (c) 2.8 atm (d) None of these

335. 4 moles of CO2 were heated in 1 dm3 vessel under conditions which produced at equilibrium 25% dissociation into carbon monoxide and oxygen. The number of moles of carbon monoxide produced was :

(a) 0.5 (b) 1.0 (c) 1.5 (d) 2.0

336. A mixture of NO2 and N2O4 has vapour density 38.5. How many mol of NO2 are present in 100 g of mixture :

(a) 0.42 (b) 4.4 (c) 33.4 (d) 3.34

337. 2.5 mL of 2/5 M weak monoacidic base (Kb=1x10¯12 at 250C) is titrated with 2/15 % M

HCl in water at 250C. The concentration of H+ at equivalence point is (Kw = 1 x 10¯14 at 250C) is:

(a) 3.7 x 10¯13 M (b) 3.2 x 10¯7 M (c) 3.2 x 10¯2 M (d) 2.7 x 10¯2 M

338. The dissociation constant of an acid, the pH of whose molar solution in 5, is :

(a) 10¯7 (b) 10¯8 (c) 10¯9 (d) 10¯10

339. The pH of a lemon juice solution at 298 K is 2.32. The OH¯ ion concentration in this solution in mol L¯ is :

(a) 10¯12 (b) 2.09 x 10¯12 (c) 10¯14 (d) 10¯8

340. At a certain temperature, the value of Kw is 9.55 x 10¯14 . So the pH value of water will be :

(a) 7 (b) 7.9 (c) 6.51 (d) 8.51

341. The pH of a solution that contains 6.02 x 10¯11 H+ ions per mL solution is : :

(a) 7 (b) 8 (c) 9 (d) 10

342. Assume that the dissociation constant for ammonia and acetic acid are same. The pOH of an ammonia solution, when that of acetic acid of equal strength is 3.27, would be :

(a) 3.27 (b) 10.8 (c) 7 (d) 1.6635

343. The pH value of Ba(OH) 2 is 12. Its solubility product value will be :

(a) 10¯7 M3 (b) 3 x 10¯7 M3 (c) 5 x 10¯7 M3 (d) 0.3 x 10¯6 M3

344. At 298 K, an aqueous has thrice as many OH¯ ions as pure water. Its pOH will be :

(a) 7 (b) 6.5229 (c) 7.312 (d) 4.921

345. 10¯3 mol of KOH was added to 10 litre of water. The pH of the solution will change by :

(a) 1 (b) 2 (c) 3 (d) 4

346. The pH of a solution having [H3O+] equal to 4 x 10¯2 g ion L¯ is :

(a) - 1 (b) 2.7 (c) 1.3983 (d) None of these

347. The [H+] of a solution having pH 10.7 is :

(a) 5 (b) 7 (c) 3 (d) 1.99 x 10¯11

348. Let the solubility of an aqueous solution of Mg (OH) 2 be x, then its Ksp is :

(a) 9x (b) 27x4 (c) 4x3 (d) 108x5

349. The pH of 10¯10 molar solution of HCl solution at 250C is approximately:

(a) 6 (b) 5 (c) 11 (d) 7

350. The pH of a solution is 6. If H+ ion concentration is reduced by 100, the resulting solution will be :

(a) more acidic (b) less acidic (c) neutral (d) can not say

351. The % age ionisation of 0.2 M CH3COOH will be :

(a) 1 (b) 0.8 (c) 0.95 (d) 6.7

352. The pH value of 102 M HCl is :

(a) -4 (b) 2 (c) 12 (d) None of these

353. Solution of 0.8 M NH4 Cl and 0.1M Mg2+ ions when mixed in equal volumes, just gave precipitate. The concentration of NH3 in solution will be :

(a) 0.74 (b) 0.37 (c) 1.11 (d) 2.0

354. The value of pH at which the 1.2 x 10¯3 M solution of an indicator having Kb value 10¯10

will change colour is :

(a) 2 (b) 3 (c) 4 (d) 5

355. The pH of a solution, one litre of which contains 0.1 mol CH3COOH and 0.1 mol HCOOH is :

(a) 4.1 (b) 2.36 (c) 3.7 (d) 1.43

356. The pH of a 0.56 mol dm¯3 aqueous solution of KOH (assuming ideal behavior) will be :

(a) 13.75 (b) 12.75 (c) 13.25 (d) 14

357. At 200C, 0.016N solution of acetic acid is 4% ionized. The ionisation constant of acetic acid will be :

(a) 2.66 x 10¯5 (b) 10¯5 (c) 5.32 x 10¯5 (d) 10¯6

358 The degree of dissociation of 0.1 M NH4 OH solution will be :

(a) 34% (b) 3.4% (c) 1.34% (d) 1.8%

359. The hydroxyl ion concentration in a solution having pH value 3 will be :

(a) 10¯11 (b) 10¯7 (c) 10¯3 (d) 10¯14

360. By adding 20 mL of 0.1 N HCl to 20mL of 0.001N KOH, the pH of the obtained solution will be :

(a) 1.3 (b) 2 (c) 7 (d) 0

361. The dissociation constant of two acids HA1 and HA2 are 3.4.x 10¯14 and 1.8 x 10¯5

respectively. The relative strength of the acids will approximately be :

(a) 1:4 (b) 4:1 (c) 1:16 (d) 16:1

362. Two mol of PCl5 are heated in a closed vessel of 2 litre capacity. When the equilibrium is attained, 40% of it has been found to be dissociated. What is the value of Kc in mol/dm3?

(a) 0.532 (b) 0.266 (c) 0.133 (d) 0.174 (e) 0.25

363. Given pH of a solution in 3 and it is mixed with another solution B having pH 2. If both mixed, the resultant pH of the solution will be :

(a) 3.2 (b) 1.96 (c) 3.4 (d) 3.5

364. The pH value of 0.001 M HCl is :

(a) + 1 (b) + 2 (c) + 3 (d) None of these

365. In a Liebig’s method to estimate carbon in an organic compound, 0.2 g of the latter produced 0.532g CO2 . The percentage of carbon in this compound is :

(a) 36.27 (b) 72.54 (c) 90 (d) 45

366. 0.316g of an organic compound containing-hydrogen and carbon produced 0.272g water. The % age of hydrogen in the compound is :

(a) 9.56 (b) 4.78 (c) 2.39 (d) 19.12

367. An organic compound weighing 0.2562 g gave 0.2998g of silver bromide. The percentage of bromide in this compound is :

(a) 36.36 (b) 18.18 (c) 40.34 (d) 49.79

368. In a carius determination of sulphur, 0.16g of an organic compound gave 0.4908g of barium sulphate. The % age of sulphur in the compound is :

(a) 42.13 (b) 84.26 (c) 60.1 (d) 17.98

369. The percentage composition of a compound is C = 90% and H=10%. The probable formula of the compound is :

(a) C8H10 (b) C15H20 (c) C15H20 (d) C15H30

370. An aromatic compound ‘Y’ having molecular formula C7H7NO produces ammonia on heating with alkali. When ‘Y’ is treated with bromine and alkali, the product will be :

(a) Aniline (b) Benzonitrile (c) Benzoic acid (d) Benzamide

371. When 32.25g of ethyl chloride is subjected to dehydrohalogenation reaction, the yield of the alkene formed is 50%. The mass of product formed is (atomic mass of chlorine is 35.5):

(a) 14g (b) 28g (c) 64.5g (d) 56g (e) 7g

372. A compound of the formula C4H10O reacts with sodoum and undergoes oxidation to give a carbonyl compound which does not reduce Tollen’s reagent. The original compound is :

(a) Diethyl ether (b) n-Butyl alcohol(c) Isobutyl alcohol (d) Sec. butyl alcohol

373. Which of the following gives iodoform test ?

(a) CH3CH2(OH) (b) C2C5CHO (c) (CH2OH) 2 (d) none of these

374. Which of the following does not undergo Cannizzaro’s reaction ?

(a) benzaldehyde (b) 2-methyl propanal(c) p- methoxybenzaldehyde (d) 2, 2-dimethyl propanal (e) formaldehyde

375. An aromatic hydrocarbon of molecular formula C8H10 forms only one mononitroderivative. The hydrocarbon is :

(a) 1, 4-dimethyl benzene (b) 1, 2-dimethyl benzene(c) 1, 3-dimethyl benzene (d) ethyl benzene

376. The total number of optical isomers in CH2 CHOH. CHOH. COOH are :

(a) 1 (b) 2 (c) 3 (d) 4

377. The total number of optical isomers in CO2H.CHOH.CHOH,CO2H. are :

(a) 1 (b) 4 (c) 3 (d) 2

378. The hardness of water containing 24 ppm of MgSO4 is :

(a) 10 ppm (b) 20 ppm (c) 30 ppm (d) 40 ppm

379. The temporary hardness of water containing 20 ppm of Ca(HCO3)2 and 10 ppm of MgSO4

is :

(a) 8.2 ppm (b) 9.2 ppm (c) 12.3 ppm (d) 24.6 ppm

380. The permanent hardness of water containing 12 mg of MgCl2 and 24 ppm of Mg(HCO3)2

per ½ kg of water is :

(a) 25.2 ppm (b) 12.6 ppm (c) 126 ppm (d) 1.26 ppm

381. The volume strength of 1.5 N H2O2 solution is :

(a) 4.8 (b) 8.4 (c) 3.0 (d) 8.0

382. The amount of H2O2 present in one litre of 2.2 N H2O2 solution is :

(a) 74.8 (b) 37.4 (c) 18.7 (d) 9.35

383. 20 volume of H2O2 solution has a strength of about :

(a) 30% (b) 6% (c) 3% (d) 10%

384. Commercially 10 volume H2O2 is a solution with strength of approximately :

(a) 30 gL¯ (b) 6 gL¯ (c) 3 gL¯ (d) 10 gL¯

385. The present strength (W/V) and normality of 15 mL of a 40 volume H2O2 solution is respectively:

(a) 6%, 6.1 N (b) 7%, 9.2 N (c) 12.13 %, 7.14 N (d) 20%, 2N

386. The number average molecular mass and mass average molecular mass of a polymer are respectively 30,000 and 40,000. The polydispersity index of the polymer is :

(a) < 1 (b) > 1 (c) 1 (d) 0 (e) - 1

387. Which of the following complexes exhibits the highest paramagnetic behaviour ?

(a) [Co(ox)2 (OH) 2]¯ (b) [Ti (NH3)6]3+

(c) [V(gly)2 (OH)2NH3]2]+ (d) [Fe (en) (bpy) (NH3)2]2+

388. 1 g of charcoal adsorbs 100 mL 0.5M CH3COOH to form a monolayer, and thereby the molarity of CH3COOH reduces to 0.49. The surface area of charcoal is 3.01 x 102 m2/g. The surface area of the charcoal adsorbed by each molecule of acetic acid is :

(a) 2.5 x 10¯19 (b) 5.0 x 10¯19

(c) 13.2 x 10¯18 (d) 1.32 x 10¯19

389. The concentration of iodine between CCl4 and water solvents in g/200 mL are 10.2 and 0.12 respectively. The value of partition co-efficient in favour of water will be :

(a) 85 (b) 0.01176 (c) 42.5 (d) 21.25

390. The partition co-efficient of I2 in-between CCl4 and H2O in 85 in favour of CCl4 solvent at 298 K. If solubility of I2 in CCl4 at 298 K is 28.05 gL¯ , the solubility of I2 in water at 298 K will be :

(a) 33.0 gL¯ (b) 0.66 gL¯ (c) 0.33 gL¯ (d) 66 gL¯

391. The distribution co-efficient of lactic acid between water and chloroform in favour of chloroform is 0.02. Half litre of aqueous solution of lactic acid in water having 25 g was mixed with 250 ml of chloroform. The concentration of lactic acid in gram in chloroform will be :

(a) 0.02 (b) 0.01 (c) 1.5 (d) 0.247

392. The distribution co-efficient of an organic compound in ethoxyethane and water is 3:1. The weight of organic compound extracted from 200 mL of aqueous solution containing 20 g of organic compound by 100 mL ethoxyethane is :

(a) 0.0012 g (b) 1.2 g (c) 6 g (d) 12 g

393. 100 mL of an aqueous solution contains 5.6 g of an organic compound. The partition co-efficient of this compound between water and CHCl3 is 1:5. The weight of organic compound extracted by 120 mL of CHCl3 in four separate extractions using 30 ml of CHCl3 for each extraction will be x:

(a) 5.6 g (b) 4.6 g (c) 5.46 (d) 1.2 g

394. The partition co-efficient of iodine between CCl4 and H2O in favour of CCl4 is 85. When 15 g of I2 is shaken with the mixed solvents. The approximate ratio between the volumes of CCl4 and H2O if 8 g of I2 is left in aqueous layer will be :

(a) 85:1 (b) 1:85 (c) 97:1 (d) 1:97

395. The volume of H2 gas at N.T.P. obtained by passing 4 amperes through acidified H2O for 30 minutes is :

(a) 0.0836 L (b) 0.0432 L (c) 0.1672 L (d) 0.836 L

396. An electrolytic cell contains a solution of Ag2SO4 and has Pt electrodes. A current is passed till 1.6 g O2 has been liberated at anode. The amount of silver deposited at cathode will be:

(a) 107.88 g (b) 1.6 g (c) 0.8 g (d) 21.60 g

397. Density of oxygen will be the highest under one of the following conditions :

(a) 273 K and 2 atm (b) NTP (c) 546 K and 1 atm (d) 546 K and 2 atm

398. The largest number of molecules will be present in :

(a) 9 g. H2O (b) 4.6 g. C2H5OH(c) 8 g. O2 (d) 7.6 g. N2O

399. The average life period of a radioactive element is the reciprocal of its :

(a) half-life period (b) disintegration constant (c) number of atoms present at any time (d) number of neutrons

400. The strength of N/50 potassium bicarbonate in gram per litre is :

(a) 2.0 (b) 3.0 (c) 4.0 (d) 1.5

ANSWER SHEET CHEMESTRY-1

1 b 21 a 41 b 61 b 81 c2 b 22 c 42 b 62 c 82 d3 c 23 a 43 b 63 c 83 b4 d 24 b 44 c 64 c 84 b5 a 25 c 45 b 65 a 85 c6 b 26 b 46 c 66 a 86 a7 a 27 b 47 a 67 a 87 a8 b 28 d 48 a 68 c 88 b9 c 29 d 49 c 69 a 89 c10 b 30 c 50 b 70 b 90 d11 c 31 b 51 b 71 c 91 b12 b 32 a 52 b 72 d 92 d13 c 33 a 53 c 73 b 93 c14 a 34 b 54 d 74 d 94 c15 c 35 d 55 c 75 c 95 a16 c 36 a 56 d 76 d 96 c17 b 37 c 57 b 77 a 97 b18 a 38 b 58 a 78 a 98 a19 c 39 c 59 c 79 a 99 a20 d 40 a 60 d 80 d 100 b

ANSWER SHEET CHEMESTRY-2

101 a 121 c 141 d 161 c 181 b102 c 122 b 142 c 162 c 182 c103 d 123 b 143 c 163 d 183 b104 b 124 a 144 a 164 b 184 c105 b 125 b 145 a 165 c 185 d106 a 126 b 146 d 166 a 186 c107 c 127 c 147 d 167 c 187 c108 b 128 c 148 b 168 b 188 a109 b 129 c 149 d 169 b 189 b110 d 130 a 150 b 170 c 190 a111 a 131 c 151 c 171 d 191 a112 a 132 b 152 a 172 c 192 c113 a 133 d 153 c 173 c 193 b114 c 134 c 154 d 174 c 194 b115 d 135 b 155 a 175 d 195 c116 a 136 b 156 d 176 b 196 d117 d 137 a 157 c 177 c 197 a118 b 138 b 158 b 178 b 198 b119 a 139 d 159 c 179 c 199 b120 b 140 c 160 c 180 d 200 d

ANSWER SHEET CHEMESTRY-3

201 d 221 b 241 c 261 a 281 d202 d 222 d 242 b 262 b 282 d203 c 223 d 243 c 263 d 283 c204 d 224 a 244 d 264 c 284 a205 d 225 b 245 d 265 c 285 a206 c 226 a 246 a 266 d 286 b207 a 227 b 247 b 267 a 287 c208 d 228 b 248 c 268 a 288 c209 c 229 b 249 d 269 b 289 d210 c 230 c 250 b 270 c 290 b211 a 231 b 251 c 271 c 291 a212 a 232 c 252 b 272 d 292 b213 c 233 d 253 c 273 b 293 b214 c 234 d 254 b 274 d 294 c215 d 235 b 255 d 275 c 295 b216 b 236 c 256 c 276 d 296 a217 a 237 c 257 b 277 c 297 c218 a 238 d 258 c 278 c 298 b219 b 239 b 259 c 279 b 299 d220 a 240 b 260 b 280 c 300 c

ANSWER SHEET CHEMESTRY-4

301 c 321 d 341 c 361 b 381 b302 a 322 c 342 b 362 b 382 b303 c 323 c 343 c 363 b 383 b304 d 324 a 344 b 364 c 384 a305 c 325 c 345 c 365 b 385 c306 b 326 b 346 c 366 a 386 b307 d 327 d 347 d 367 d 387 d308 b 328 b 348 c 368 a 388 b309 d 329 b 349 d 369 c 389 b310 b 330 a 350 b 370 a 390 c311 b 331 b 351 c 371 e 391 d312 d 332 c 352 d 372 c 392 d313 c 333 d 353 b 373 a 393 c314 d 334 b 354 c 374 b 394 d315 a 335 b 355 b 375 a 395 d316 b 336 a 356 a 376 d 396 d317 b 337 c 357 a 377 c 397 a318 a 338 d 358 c 378 b 398 a319 b 339 b 359 a 379 c 399 b320 c 340 c 360 a 380 a 400 a