CHEMISTRY FOR JEE

1. A student performs a titration with different burettes and finds titre values of \(25.2 \mathrm{~mL}\), \(25.25 \mathrm{~mL}\), and \(25.0 \mathrm{~mL}\). The number of significant figures in the average titre value is

[IIT JEE 2010]

1) 1

2) 2

3) 3

4) 4

2. The correctly reported answer of the addition of \(4.523,2.3\) and 6.24 will have significant figures

[Manipal 2008]

1) Two

2) Three

3) Four

4) Five

3. The least count of an instrument is \(0.01 \mathrm{~cm}\).

Taking all precautions, the most possible error in the measurement can be [Manipal 2004]

1) \(0.005 \mathrm{~cm}\)

2) \(0.01 \mathrm{~cm}\)

3) \(0.0001 \mathrm{~cm}\)

4) \(0.1 \mathrm{~cm}\)

4. Which one of the following set of units represents the smallest and largest amount of energy respectively?

[Kerala CEE 2007]

1)J and erg

2) erg and cal

3) Cal and eV

4) L-atm and J

5) \(\mathrm{eV}\) and L-atm

5. The value of amu is which of the following?

[Guj CET 2007]

1) \(1.57 \times 10^{-24} \mathrm{~kg}\)

2) \(1.66 \times 10^{-24} \mathrm{~kg}\)

3) \(1.99 \times 10^{-23} \mathrm{~kg}\)

4) \(1.66 \times 10^{-27} \mathrm{~kg}\)

6. The mass of \(11.2 \mathrm{~L}\) of ammonia gas at STP is

[Kerala CEE 2004]

1) \(8.5 \mathrm{~g}\)

2) \(85 g\)

3) \(17 \mathrm{~g}\)

4) \(1.7 \mathrm{~g}\)

5) \(4.25 \mathrm{~g}\)

7. Law of multiple proportions is illustrated by one of the following pairs [Kerala CEE 2003]

1) \(\mathrm{H}_{2} \mathrm{~S}\) and \(\mathrm{SO}_{2}\)

2) \(\mathrm{NH}_{3}\) and \(\mathrm{NO}_{2}\)

3) \(\mathrm{Na}_{2} \mathrm{~S}\) and \(\mathrm{Na}_{2} \mathrm{O}\)

4) \(\mathrm{BeO}\) and \(\mathrm{BeCl}_{2}\)

5) \(\mathrm{N}_{2} \mathrm{O}\) and \(\mathrm{NO}\)

8. The number of hydrogen atoms present in 25.6 g of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) which has a molar mass of \(342.3 \mathrm{~g}\) is

[VITEEE 2008]

1) \(22 \times 10^{23}\)

2) \(9.91 \times 10^{23}\)

3) \(11 \times 10^{23}\)

4) \(44 \times 10^{23} \mathrm{H}\) atoms

9. \(80 \mathrm{~g}\) of oxygen contains as many atoms as in

[KCET 2008]

1) 80 g of hydrogen

2) \(1 \mathrm{~g}\) of hydrogen

3) 10 g of hydrogen

4) 5 g of hydrogen

10. Gram molecular volume of oxygen at STP is

1) \(3200 \mathrm{~cm}^{3}\)

2) \(5600 \mathrm{~cm}^{3}\)

3) \(22400 \mathrm{~cm}^{3}\)

4) \(11200 \mathrm{~cm}^{3}\)

[KCET 2007]

11. How many H-atoms are present in \(0.046 \mathrm{~g}\) of ethanol?

[BITSAT 2003]

1) \(6 \times 10^{20}\)

2) \(1.2 \times 10^{21}\)

3) \(3 \times 10^{21}\)

4) \(3.6 \times 10^{21}\)

12. Which has the maximum number of atoms?

[DCE 2003]

1) \(2.0 \mathrm{~mol}\) of \(S_{8}\)

2) \(6.0 \mathrm{~mol}\) of \(S\)

3) 5.5 mol of \(\mathrm{SO}_{2}\)


13. A gas has a vapour density 11.2. The volume occupied by \(1 \mathrm{~g}\) of the gas at NTP is

[BCECE 2004]

1) \(1 \mathrm{~L}\)

2) \(11.2 \mathrm{~L}\)

3) \(22.4 \mathrm{~L}\)

4) \(4 \mathrm{~L}\)

14. The number of atoms in \(4.25 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) is

approximately

[MHT CET 2003]

1) \(6 \times 10^{23}\)

2) \(2 \times 10^{23}\)

3) \(1.5 \times 10^{23}\)

4) \(1 \times 10^{23}\)

15. 0.1 mole of a carbohydrate with empirical formula \(\mathrm{CH}_{2} \mathrm{O}\) contains \(1 \mathrm{~g}\) of hydrogen. What is its molecular formula?

[Kerala CEE 2008]

1) \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{5}\)

2) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

3) \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{4}\)

4) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}\)

5) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\) 16. Law of constant composition is same as the law of

1) Conservation of

2) Conservation of mass energy

3) Multiple proportion 4) Definite proportion

17. One mole of \(\mathrm{CO}_{2}\) contains

[Manipal 2010]

1) 3 g atoms of \(\mathrm{CO}_{2}\)

2) \(\begin{aligned} & 18.1 \times 10^{23} \\ & \text { molecules of } \mathrm{CO}_{2}\end{aligned}\)


18. The number of gram molecules of chlorine in 6. \(02 \times 10^{25}\) hydrogen chloride molecules is

[KCET 2007]

1) 10

2) 100

3) 50

4) 5

19. Which has the maximum number of atoms?

[WB JEE 2007]

1) \(24 g\) of \(C\)

2) \(56 \mathrm{~g}\) of \(\mathrm{Fe}\)

3) \(26 \mathrm{~g}\) of \(\mathrm{Al}\)

4) 108 g of \(\mathrm{Ag}\)

20. The number of formula units of calcium fluoride, \(\mathrm{CaF}_{2}\) present in \(146.4 \mathrm{~g}\) of \(\mathrm{CaF}_{2}\) (the molar mass of \(\mathrm{CaF}_{2}\) is \(78.08 \mathrm{~g} / \mathrm{mol}\) ) is

[VITEEE 2008]

1) \(1.129 \times 10^{24} \mathrm{CaF}_{2}\)

2) \(1.146 \times 10^{24} \mathrm{CaF}_{2}\)

3) \(7.808 \times 10^{24} \mathrm{CaF}_{2}\)

4) \(1.877 \times 10^{24} \mathrm{CaF}_{2}\)

21. How many moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) would be in \(50 \mathrm{~g}\) of the substance? [Jamia Millia Islamia

2006]

1) \(0.083 \mathrm{~mol}\)

2) \(0.952 \mathrm{~mol}\)

3) \(0.481 \mathrm{~mol}\)

4) \(0.140 \mathrm{~mol}\)

22. \(1 \mathrm{~L}\) oxygen gas at STP will weigh [JCECE 2010]

1) 1.43

2) \(2.24 \mathrm{~g}\)

3) \(11.2 \mathrm{~g}\)

4) \(22.4 \mathrm{~g}\)

23. Which has the highest weight?

[Manipal 2010]

1) \(1 \mathrm{~m}^{3}\) of water

2) A normal adult man

3) \(10 \mathrm{~L}\) of Hg

4) All have same weight

24. The mass of 1 mole of electrons is

[UP SEE 2006]

1) \(9.1 \times 10^{-28} \mathrm{~g}\)

2) \(1.008 \mathrm{mg}\)

3) \(0.55 \mathrm{mg}\)

4) \(9.1 \times 10^{-27} g\)

25. The maximum number of molecules are present in

[UP SEE 2007]

1) 15 Lof \(\mathrm{H}_{2}\) gas at

2) 5 Lof \(N_{2}\) gas at STP

3) \(0.5 \mathrm{~g}\) of \(\mathrm{H}_{2}\) gas

4) \(10 \mathrm{~g}\) of \(\mathrm{O}_{2}\) gas

26. Which of the following contains greatest number of oxygen atoms?

[UP SEE 2009]

1) \(1 \mathrm{~g}\) of 0

2) \(1 \mathrm{~g}\) of \(\mathrm{O}_{2}\)

3) \(1 \mathrm{~g}\) of \(\mathrm{O}_{3}\)

4) All have the same number of atoms

27. The numerical value of \(\frac{N}{n}\) (where, \(N\) is the number of molecules in a given sample of gas and \(n\) is the number of moles of the gas) is

[Kerala CEE 2004]

1) 8.314

2) \(6.02 \times 10^{23}\)

3) 0.0821

4) \(1.66 \times 10^{-19}\)

5) \(1.62 \times 10^{-24}\)

28. Number of atoms of oxygen present in \(10.6 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) will be

[J\&K CET 2004]

1) \(6.02 \times 10^{23}\)

2) \(12.04 \times 10^{22}\)

3) \(1.806 \times 10^{23}\)

4) \(31.80 \times 10^{28}\)

29. \(4.6 \times 10^{22}\) atoms of an element weigh \(13.8 \mathrm{~g}\).

The atomic weight of element is

[WB JEE 2007]

1) 290

2) 180

3) 34.4

4) 10.4

30. One gram mole of a gas at NTP occupies \(22.4 \mathrm{~L}\). This fact was derived from

1) Law of gaseous

2) Avogadro's volumes hypothesis

3) Berzelius hypothesis 4) Dalton's atomic theory

31. Weight of an atom of an element is 6. \(644 \times 10^{-23} \mathrm{~g}\). What will be the number of \(g\) atom of that element in \(40 \mathrm{~kg}\) ?

[AMU 2003]

1) \(10^{3}\)

2) \(10^{6}\)

3) \(1.5 \times 10^{3}\)

4) None of these

32. Arrange the following in the order of increasing mass (atomic mass; \(\mathrm{O}=16, \mathrm{Cu}=\) \(63, \mathrm{~N}=14\) )

1. One atom of oxygen

2. One atom of nitrogen

3. \(1 \times 10^{-10}\) mole of oxygen

4. \(1 \times 10^{-10}\) mole of copper

5. [Kerala CEE 2011]

1) \(I I<I<I I I<I V \quad 2) I<I I<I I I<I V\)

3) \(I I I<I I<I V<I\) 4)IV \(<I I<I I I<I\)

5) \(I I<I V<I<I I I\)

33. How many moles of magnesium phosphate, \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) will contain 0.25 mole of oxygen

atoms?

1) 0.02

2) \(3.125 \times 10^{-2}\)

3) \(1.25 \times 10^{-2}\)

4) \(2.5 \times 10^{-2}\)

[AIEEE 2006]

34. The total number of protons in \(10 \mathrm{~g}\) of calcium carbonate is \(\left(N_{0}=6.023 \times 10^{23}\right)\)

1) \(3.01 \times 10^{24}\)

2) \(4.06 \times 10^{24}\)

[WB JEE 2006] 

3) \(2.01 \times 10^{24}\)

4) \(3.02 \times 10^{24}\)

35. The number of molecules of \(\mathrm{CO}_{2}\) present in 44 \(\mathrm{g}\) of \(\mathrm{CO}_{2}\) is

[BCECE 2005]

1) \(6.0 \times 10^{23}\)

2) \(3 \times 10^{23}\)

3) \(12 \times 10^{23}\)

4) \(3 \times 10^{10}\)

36. Which of the following has the smallest number of molecules?

[WB JEE 2007]

1) 0.1 mole of \(\mathrm{CO}_{2}\) gas

2) \(\begin{aligned} & \text { 11.2 L of } \mathrm{CO}_{2} \text { gas at }\end{aligned}\)

3) 22 g of \(\mathrm{CO}_{2}\) gas

4) \(22.4 \times 10^{3} \mathrm{~mL}\) of \(\mathrm{CO}_{2}\)

gas at STP

37. \(2 \mathrm{~g}\) of \(O_{2}\) at \(O^{0} \mathrm{C}\) and \(760 \mathrm{~mm}\) of \(\mathrm{Hg}\) pressure has volume

[BCECE 2005]

1) \(1.4 \mathrm{~L}\)

2) \(2.8 \mathrm{~L}\)

3) \(11.2 \mathrm{~L}\)

4) \(22.4 \mathrm{~L}\)

38. Which one of the following has the maximum number of atoms of oxygen?

[KCET 2007]

1) \(2 \mathrm{~g}\) of carbon

2) \(2 \mathrm{~g}\) of carbon dioxide monoxide

4) \(2 \mathrm{~g}\) of water

3) 2 g of sulphur dioxide

39. Number of atoms of \(\mathrm{He}\) in \(100 \mathrm{u}\) of \(\mathrm{He}\) (atomic weight of \(\mathrm{He}\) is 4 ) are

[BCECE 2008]

1) 25

2) 100

3) 50

4) \(100 \times 6 \times 10^{-23}\)

40. Which of the following is correct for \(C\) (graphite \()+\mathrm{O}_{2}\) (gas \() \rightarrow \mathrm{CO}_{2}\), heat \(=-348\) \(\mathrm{kJ}\) ?

[OJEE 2006]

1) Heat absorbed

2) Mass of product \(>\) Mass of reactant

3) Mass of product \(<\)

4) Mass of product \(=\)

Mass of reactant Mass of reactant

41. A signature, written in carbon pencil weights 1 \(\mathrm{mg}\). What is the number of carbon atoms present in the signature?

[RPET 2005]

1) \(5.02 \times 10^{23}\)

2) \(5.02 \times 10^{20}\)

3) \(6.02 \times 10^{20}\)

4) \(0.502 \times 10^{20}\)

42. Which of the following contains maximum number of molecules?

[Kerala CEE 2004]

1) 100 cc of \(\mathrm{CO}_{2}\) at \(\left.S T P_{2}\right) 150\) cc of \(\mathrm{N}_{2}\) at STP

3) 50 cc of \(\mathrm{SO}_{2}\) at \(S T P\)

4) 150 cc of \(\mathrm{O}_{2}\) at STP

5) 200 cc of \(\mathrm{NH}_{3}\) at STP

43. The mass of \(112 \mathrm{~cm}^{3}\) of \(\mathrm{CH}_{4}\) gas at STP is

[DCE 2006]

1) \(0.16 \mathrm{~g}\)

2) \(0.8 \mathrm{~g}\)

3) \(0.08 \mathrm{~g}\)

4) \(1.6 \mathrm{~g}\)

44. Number of atoms in \(560 \mathrm{~g}\) of \(\mathrm{Fe}\) ( atomic mass \(56 \mathrm{~g} \mathrm{~mol}^{-1}\) ) is

[Jamia Millia Islamia 2005] 1)Twice that of \(70 \mathrm{~g} \mathrm{~N}\) 2) Half that of \(20 \mathrm{~g} \mathrm{H}\)

3) Both are correct

4) None of these

45. Mass of 0.1 mole of methane is [KCET 2008]

1) \(1 \mathrm{~g}\)

2) \(16 \mathrm{~g}\)

3) \(1.6 \mathrm{~g}\)

4) \(0.1 \mathrm{~g}\)

46. \(74.5 \mathrm{~g}\) of a metallic chloride contains \(35.5 \mathrm{~g}\) of chlorine, the equivalent weight of the metal is

1) 19.5

2) 35.5

3) 39

4) 78.0

[WB JEE 2007]

47. \(2 \mathrm{~g}\) of metal carbonate is neutralised completely by \(100 \mathrm{~mL}\) of \(0.1(\mathrm{~N}) \mathrm{HCl}\). The equivalent weight of metal carbonate is

1) 50

2) 100

3) 150

4) 200

[WB JEE 2011]

48. \(\mathrm{KMnO}_{4}\) (mol.wt. \(\left.=158\right)\) oxidizes oxalic acid in acid medium to \(\mathrm{CO}_{2}\) and water as follows \(5 \mathrm{C}_{2} \mathrm{O}_{4}^{2-}+2 \mathrm{MnO}_{4}^{-}+16 \mathrm{H}^{+} \rightarrow 10 \mathrm{CO}_{2}+2 \mathrm{Mn}^{2+}+\) What is the equivalent weight of \(\mathrm{KMnO}_{4}\) ?

[J\&K CET 2006]

1) 158

2) 31.6

3) 39.5

4) 79

49. \(3 \mathrm{~g}\) of an oxide of a metal is converted to chloride completely and it yields \(5 \mathrm{~g}\) of chloride. The equivalent weight of the metal is [OJEE 2007]

1) 33.25

2) 3.325

3) 12

4) 20

50. The formula mass of Mohr's salt is 392. The iron present in it is oxidised by \(\mathrm{KMnO}_{4}\) in acid medium. The equivalent mass of Mohr's salt is [Jamia Millia Islamia 2008]

1) 392

2) 31.6

3) 278

4) 156

51. Dulong and Petit's law is valid only for [KCET 2004]

1) Metals

2) Non-metals

3)Gaseous elements

4) Solid elements

52. A gas is found to have formula \([\mathrm{CO}]_{x}\). Its vapour density is 70, the \(x\) is [BCECE 2007]

1) 3.0

2) 3.5

3) 5.0

4) 6.5

53. An unknown element forms an oxide. What will be the equivalent weight of the element if the oxygen content is \(20 \%\) by weight? [WB JEE 2008]

1) 16

2) 32

3) 8

4) 64

54. A bivalent metal has an equivalent mass of 32 . The molecular mass of the metal nitrate is [Manipal 2009]

1) 182

2) 168

3) 192

4) 188 55. In the disproportionation reaction \(3 \mathrm{HClO}_{3} \rightarrow \mathrm{HClO}_{4}+\mathrm{Cl}_{2}+2 \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}\), the equivalent mass of the oxidising agent is (molar mass of \(\mathrm{HClO}_{3}=84.45\) ) [Kerala CEE

2011]

1) 16.89

2) 32.22

3) 84.45

4) 28.15

5) 29.7

56. The equivalent weight of \(\mathrm{KMnO}_{4}\) for acid solution is [Manipal 2010]

1) 79

2) 52.16

3) 158

4) 31.6

57. If we consider that \(\frac{1}{6}\), in place of \(\frac{1}{12}\), mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of a substance will [AIEEE 2005]

1) Be a function of the 2) Remain unchanged molecular mass or the substance

3) Increase two fold 4) Decrease twice

58. If molecular weight of \(\mathrm{KMnO}_{4}\) is \(M\), then its equivalent weight in acidic medium would be [WB JEE 2007]

1) \(M\)

2) \(\frac{M}{2}\)

3) \(\frac{M}{5}\)

4) \(\frac{M}{3}\)

59. The standard adopted for the determination of atomic weight of elements is based on [Kerala CEE 2003]

1) \(H^{1}\)

2) \(C^{12}\)

3) \(O^{16}\)

4) \(S^{32}\)

5) \(\mathrm{Cl}^{35}\)

60. An alkaloid contains \(17.28 \%\) of nitrogen and it's molecular mass is 162 . The number of nitrogen atoms present in one molecule of alkaloid is [Guj CET 2008]

1) 5

2) 4

3) 3

4) 2

61. The equivalent weight of a solid element is found to be 9 . If the specific heat of this element is \(1.05 \mathrm{Jg}^{-1} \mathrm{~K}^{-1}\), then its atomic weight is [Manipal 2004]

1) 17

2) 21

3) 25

4) 27

62. Of two oxides of iron, the first contained \(22 \%\) and the second contained \(30 \%\) of oxygen by weight. The ratio of weights of iron in the two oxides that combine with the same weight of oxygen, is [J\&K CET 2008]

1) \(3: 2\)

2) \(2: 1\)

3) \(1: 2\)

4) \(1: 1\)

63. \(1.520 \mathrm{~g}\) of hydroxide of a metal on ignition gave \(0.995 \mathrm{~g}\) of oxide. The equivalent weight of metal is [BCECE 2008]

1) 1.52

2) 0.995

3) 190

4) 9

64. The relative abundance of two isotopes of atomic weight 85 and 87 is \(75 \%\) and \(25 \%\) respectively. The average atomic weight of element is [DCE 2003]

1) 75.5

2) 85.5

3) 40.0

4) 86.0

65. The equivalent weight of \(\mathrm{KIO}_{3}\) in the reaction, \(2 \mathrm{Cr}(\mathrm{OH})_{3}+\mathrm{OH}^{-}+\mathrm{KIO}_{3} \rightarrow 2 \mathrm{CrO}_{4}^{2-}+5 \mathrm{H}_{2} \mathrm{O}+\) is [UP SEE 2003]

1) Mol. wt.

2) Mol. wt./ 3

3) Mol. wt./ 6

4) Mol. wt./ 2

66. The electrochemical equivalent of a metal is ' \(x\) ' g coulom \(b^{-1}\). The equivalent weight of metal is [EAMCET 2004]

1) \(x\)

2) \(x \times 96500\)

3) \(\frac{x}{96500}\)

4) \(1.6 \times 10^{-19} \times x\)

67. Camphor is often used in molecular mass determination because [Manipal 2007]

1) It is readily available 2) It has a very high cryoscopic constant

3)It is volatile

4) It is solvent for organic substances

68. In the equation, \(\mathrm{H}_{2} \mathrm{~S}+2 \mathrm{HNO}_{3} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{NO}_{2}+\mathrm{S}\)

The equivalent weight of hydrogen sulphide is [BCECE 2006]

1) 18

2) 68

3) 34

4) 17

69. Given, that the abundances of isotopes \({ }_{54} \mathrm{Fe}\), \({ }_{56} \mathrm{Fe}\) and \({ }_{57} \mathrm{Fe}\) are 5\%, 90\% and \(5 \%\), respectively, the atomic mass of Fe is [IIT JEE 2009]

1) 55.85

2) 55.95

3) 55.75

4) 56.05

70. What is the equivalent weight of \(\mathrm{SnCl}_{2}\) in the following reaction, \(\mathrm{SnCl}_{2}+\mathrm{Cl}_{2} \rightarrow \mathrm{SnCl}_{4} ?\) [KCET 2008]

1) 95

2) 45

3) 60

4) 30

71. If the molecular weight of \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) and \(\mathrm{I}_{2}\) are \(M_{1}\) and \(M_{2}\) respectively, then what will be the equivalent weight of \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) and \(\mathrm{I}_{2}\) in the following reaction? \(2 \mathrm{~S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{I}_{2} \rightarrow \mathrm{S}_{4} \mathrm{O}_{6}^{2-}+2 I^{-}\)[WB JEE 2011]

1) \(M_{1}, M_{2}\)

2) \(M_{1}, M_{2} / 2\) 

3) \(2 M_{1}, M_{2}\)

4) \(M_{1}, 2 M_{2}\)

72. For the reaction, \(\mathrm{Na}_{2} \mathrm{CO}_{3}+2 \mathrm{HCl} \rightarrow \mathrm{NaCl}+\mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2}\)

Equivalent weight of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is [AMU 2007]

1) \(\frac{M}{2}\)

2) \(M\)

3) \(2 M\)

4) \(\frac{M}{4}\)

73. Equivalent weight of a bivalent metal is 37.2. The molecular weight of its chloride is [MHT CET 2003]

1) 412.2

2) 216

3) 145.4

4) 108.2

74. The percentage of an element \(M\) is 53 in its oxide of molecular formula \(\mathrm{M}_{2} \mathrm{O}_{3}\). Its atomic mass is about [Kerala CEE 2008]

1) 45

2) 9

3) 18

4) 36

5) 27

75. The equivalent weight of a certain trivalent element is 20. Molecular weight of its oxide is [RPET 2005]

1) 152

2) 56

3) 168

4) 68

76. \(4 \mathrm{~g}\) of copper was dissolved in concentrated nitric acid. The copper nitrate solution on strong heating gave \(5 \mathrm{~g}\) of its oxide. The equivalent weight of copper is [AMU 2006]

1) 23

2) 32

3) 12

4) 20

77. In acidic medium, the equivalent weight of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{Mol} . \mathrm{wt}\). \(=\mathrm{M})\) is [UP SEE 2009]

1) \(M\)

2) \(\frac{M}{2}\)

3) \(\frac{M}{3}\)

4) \(\frac{M}{6}\)

78. A compound contains \(69.5 \%\) oxygen and \(30.5 \%\) nitrogen and its molecular weight is 92 . The formula of the compound is [DCE 2007]

1) \(\mathrm{N}_{2} \mathrm{O}\)

2) \(\mathrm{NO}_{2}\)

3) \(\mathrm{N}_{2} \mathrm{O}_{4}\)

4) \(\mathrm{N}_{2} \mathrm{O}_{5}\)

79. If two compounds have the same empirical formula but different molecular formulae, they must have [RPET 2008]

1) Different percentage 2) Different molecular composition weights

3) Same viscosity

4) Same vapour density

80. A hydrocarbon contains \(10.5 \mathrm{~g}\) carbon and \(1 \mathrm{~g}\) hydrogen. Its \(2.81 \mathrm{~g}\) has \(1 \mathrm{~L}\) volume at \(1 \mathrm{~atm}\) and \(127^{\circ} \mathrm{C}\), hydrocarbon is [UP SEE 2003]

1) \(\mathrm{C}_{6} \mathrm{H}_{7}\)

2) \({ }_{7} \mathrm{H}_{8}\)

3) \(\mathrm{C}_{5} \mathrm{H}_{6}\)

4) None of the above

81. The empirical formula of a compound is \(\mathrm{CH}_{2}\). One mole of this compound has a mass of \(42 \mathrm{~g}\). Its molecular formula is [Manipal 2006]

1) \(\mathrm{C}_{3} \mathrm{H}_{6}\)

2) \(\mathrm{C}_{3} \mathrm{H}_{8}\)

3) \(\mathrm{CH}_{2}\)

4) \(\mathrm{C}_{2} \mathrm{H}_{2}\)

82. A compound contains \(54.55 \%\) carbon, \(9.09 \%\) hydrogen, \(36.36 \%\) oxygen. The empirical formula of this compound is [UP SEE 2004]

1) \(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}\)

2) \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{2}\)

3) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\)

4) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\)

83. 0.0833 mole of carbohydrate of empirical formula \(\mathrm{CH}_{2} \mathrm{O}\) contain \(1 \mathrm{~g}\) of hydrogen. The molecular formula of the carbohydrate is [RPET 2004]

1) \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{5}\)

2) \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{3}\)

3) \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\)

4) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

84. An organic compound on analysis was found to contain \(10.06 \%\) carbon, \(0.84 \%\) hydrogen and \(89.10 \%\) chlorine. What will be the empirical formula of the substance? [MP PET 2010]

1) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\)

2) \(\mathrm{CHCl}_{3}\)

3) \(\mathrm{CCl}_{4}\)

4) \(\mathrm{CH}_{3} \mathrm{Cl}\)

85. Equivalent weight of an acid [UP SEE 2004]

1) Depends on the

2) Depends upon the reaction involved number of oxygen atoms present

3) Is always constant 4) None of the above

86. An aromatic hydrocarbon with empirical formula \(\mathrm{C}_{5} \mathrm{H}_{4}\) on treatment with concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) gave a monosulphonic acid. \(0.104 \mathrm{~g}\) of the acid required \(10 \mathrm{~mL}\) of \(\frac{N}{20} \mathrm{NaOH}\) for complete neutralisation. The molecular formula of hydrocarbon is [Kerala CEE 2007]

1) \(\mathrm{C}_{5} \mathrm{H}_{4}\)

2) \({ }^{C_{10}} \mathrm{H}_{8}\)

3) \(\mathrm{C}_{15} \mathrm{H}_{12}\)

4) \(\mathrm{C}_{20} \mathrm{H}_{16}\)

5) \(\mathrm{C}_{15} \mathrm{H}_{20}\)

87. In a compound \(\mathrm{C}, \mathrm{H}\) and \(\mathrm{N}\) are present is \(9: 1\) : 3.5 by weight. If molecular weight of the compound is 108 , then the molecular formula of the compound is [BCECE 2008]

1) \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{~N}_{2}\)

2) \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{~N}\)

3) \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{~N}_{2}\)

4) \(\mathrm{C}_{9} \mathrm{H}_{12} \mathrm{~N}_{3}\)

88. An organic compound has an empirical formula \(\left(\mathrm{CH}_{2} \mathrm{O}\right)\) its vapour density is 45 . The molecular formula of the compound is [Manipal 2006]

1) \(\mathrm{CH}_{2} \mathrm{O}\)

2) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{O}\)

3) \(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O}\)

4) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\) 89. An organic compound contains \(49.3 \%\) carbon, \(6.84 \%\) hydrogen and its vapour density is 73 . Molecular formula of the compound is [RPET 2004]

1) \(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}_{2}\)

2) \(\mathrm{C}_{4} \mathrm{H}_{10} \mathrm{O}_{2}\)

3) \(\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{O}\)

4) \(\mathrm{C}_{3} \mathrm{H}_{10} \mathrm{O}\)

90. The empirical formula of a compound is \(\mathrm{CH}_{2}\).

One mole of this compound has a mass of \(56 \mathrm{~g}\). its molecular formula is [MP PET 2006]

1) \(\mathrm{C}_{3} \mathrm{H}_{6}\)

2) \({ }_{4} \mathrm{H}_{8}\)

3) \(\mathrm{CH}_{2}\)

4) \(\mathrm{C}_{2} \mathrm{H}_{2}\)

91. An organic compound containing \(\mathrm{C}\) and \(\mathrm{H}\) has \(92.3 \%\) of carbon, its empirical formula is

[EAMCET 2004]

1) \(\mathrm{CH}\)

2) \(\mathrm{CH}_{3}\)

3) \(\mathrm{CH}_{2}\)

4) \(\mathrm{CH}_{4}\)

92. An aqueous solution containing \(6.5 \mathrm{~g}\) of \(\mathrm{NaCl}\) of \(90 \%\) purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid \(\mathrm{NaOH}\). The volume of 1 \(\mathrm{M}\) acetic acid required to neutralise \(\mathrm{NaOH}\) obtained above is [Manipal 2009]

1) \(1000 \mathrm{~cm}^{3}\)

2) \(2000 \mathrm{~cm}^{3}\)

3) \(100 \mathrm{~cm}^{3}\)

4) \(200 \mathrm{~cm}^{3}\)

93. Excess of carbon dioxide is passed through 50 \(\mathrm{mL}\) of \(0.5 \mathrm{M}\) calcium hydroxide solution. After the completion of the reaction, the solution was evaporated to dryness. The solid calcium carbonate was completely neutralised with 0.1 \(\mathrm{N}\) hydrochloric acid. The volume of

hydrochloric acid required is (Atomic mass of calcium =40) [Manipal 2009]

1) \(300 \mathrm{~cm}^{3}\)

2) \(200 \mathrm{~cm}^{3}\)

3) \(500 \mathrm{~cm}^{3}\)

4) \(400 \mathrm{~cm}^{3}\)

94. Stoichiometric ratio of sodium dihydrogen orthophosphate and sodium hydrogen orthophosphate required for synthesis of \(\mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{11}\) is [Guj CET 2011]

1) \(1.5: 3\)

2) \(3: 1.5\)

3) \(1: 1\)

4) \(2: 3\)

95. The ratio of amounts of \(\mathrm{H}_{2} \mathrm{~S}\) needed to precipitate all the metal ions from \(100 \mathrm{~mL}\) of 1 \(\mathrm{M} \mathrm{AgNO}_{3}\) and \(100 \mathrm{~mL}\) of \(\mathrm{CuSO}_{4}\), will be

\section{[Manipal 2008]}

1) \(1: 1\)

2) \(1: 2\)

3) \(2: 1\)

4) None of these

96. \(x\) grams of calcium carbonate was completely burnt in air. The weight of the solid residue formed is \(28 \mathrm{~g}\). What is the value of \(x\) (in grams)? [EAMCET 2005]

1) 44

2) 200

3) 150

4) 50

97. Sodium nitrate on reduction with \(\mathrm{Zn}\) in presence of \(\mathrm{NaOH}\) solution produces \(\mathrm{NH}_{3}\). Mass of sodium nitrate absorbing 1 mole of electron will be [WB JEE 2008]

1) 7.750

2) 10.625

3) 8.000

4) 9.875

98. The volume of oxygen necessary for the complete combustion of \(20 \mathrm{~L}\) of propane is [WB JEE 2006]

1) \(40 \mathrm{~L}\)

2) \(60 \mathrm{~L}\)

3) \(80 \mathrm{~L}\)

4) \(100 \mathrm{~L}\)

99. What is the volume (in litres) of oxygen required at STP to completely convert 1.5 moles of sulphur into sulphur dioxide?

[EAMCET 2003]

1) 11.2

2) 22.4

3) 33.6

4) 44.8

100.2 g of mixture of \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\) on reaction with excess \(\mathrm{I}_{2} \mathrm{O}_{5}\) produced \(2.54 \mathrm{~g}\) of \(\mathrm{I}_{2}\). What would be the mass \(\%\) of \(\mathrm{CO}_{2}\) in the original mixture? [WB JEE 2007]

1) 60

2) 30

3) 70

4) 35