12 (b) 320g of sulphur - iBioKaare · (1) (1) Avogadro’s number represents the number of atoms in...

(1)

(1) Avogadro’s number represents the number of atoms in(a) 12g of C12 (b) 320g of sulphur

(c) 32g of oxygen (d) 12.7g of iodine

(2) The number of moles of carbon dioxide which contain 8 g of oxygen is(a) 0.5 mol (b) 0.20 mol

(c) 0.40 mol (d) 0.25 mol

(3) The total no of ions present in 111 g of cacl2 is(a) One mole (b) Two mole

(c) Three mole (d) Four moles

(4) Which of the following weighs the most ?(a) one g-atom of nitrogen (b) One mole of water

(c) One mole of sodium (d) One molecule of H2So4

(5) 5.0 litre of 0.4 M H2SO4 Contains-(a) 2.0 Mole Of H2So4 (b) 0.4 mole H2So4

(c) 5.0 mole H2So4 (d) 2.0 moles H2O

(6) A symbol not only represents the name of the element but also represents-(a) its atomic no. (b) 1 gm-atom

(c) its atomicity (d) Reactivity.

(7) Which has maximum number of atoms ?(a) 24g of c (12) (b) 56g of Fe (56)

(c) 27g of Al (27) (d) 108g of Ag (108)

(8) Number of atoms of oxygen present in 10.6g Na2Co3 will be-(a) 6.02 × 1022 (b) 12.04 × 1022

(c) 1.806 × 1023 (d) 31.80 × 1023

(9) The maximum no. of molecules is present in(a) 15 L of H2 gas at S.T.P (b) 5 L of N2 gas at S.T.P

(c) 0.5 g of H2 gas (d) 10 g of O2 gas.

(10) The number of g-atom of oxygen in 6.02 × 1024 CO molecules is(a) 1 (b) 0.5

(c) 5 (d) 10

(11) Number of electrons in 1.8 mL of H2O is:(a) 6.02 x 1023 (b) 3.011 x 1023 (c) 0.6022 x 1023 (d) 60.22 x 1023

(12) Which names are associated with 1g / NA ?(a) Rutherford (b) 1 Dalton

(c) 1 Avogram (d) 1 gram

AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB

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(2)

(13) 100 g caco3 is treated with I litre of 1N HCl. What would be the weight of co2libereted after the completion of the reaction ?(a) 5.5 g (b) 11g

(c) 22g (d) 33g

(14) The mass of carbon present in 0.5 mole of K4 [Fe(CN)6] is(a) 1.8 g (b) 18 g

(c) 3.6 g (d) 36 g

(15) Number of water molecules in the drop of water,if 1 ml of water has 20 drops and A isAvogadro’s number, is-(a) 0.5A/18 (b) 0.05A

(C)0.5A (d) 0.05A/18

(16) Volume at N.T.P of 0.22 g of CO2 is same as that of-(a) 0.01 g of hydrogen (b) 0.085 g of NH3

(c) 320 mg of gaseous So2 (d) All the above.

(17) 0.224 L of H2 gas at S.T.P is equivalent to(a) 1 mol (b) 1g

(c) 6.02 × 1022 molecules (d) 0.01 mol

(18) 2.0 g of oxygen contains number of atoms same as in-(a) 4g of s (b) 7g of nitrogen

(c) 0.5 g of H2 (d) 12.3 g of Na.

(19) A sample of phosphrous trichloride(PCl3) contains 1 .4 moles of the substance. howmany atoms are there is the sample ?(a) 5.6 (b) 4

(c) 8.431× 1023 (d)3.372× 1024

(20) Which of the following contains maximum no. of molecules ?(a) 200 cc of NH3 at S.T.P (b) 150 cc of N3 at S.T.P

(c) 50 cc of So2 at S.T.P (d) 150 cc of O2 at S.T.P

(21) Which among the following is the heaviest?(a) One mole is oxygen (b) One molecule of sulphur trioxide

(c) 100 amu of uranium (d) 44 g of carbon dioxide.

(22) 6.02×1022 molecules of N2 at NTP will occupy a volume of(a) 22.4 litres (b) 2.24 litres

(C) 6.02 litres (d) 6.02 mL

(23) How many grams are contained in 1 gram-atom of Na?(a) 13g (b) 23g

(C) 1 g (d) 1/23g

(24) I mole of a compuund contain 1 mole of C and 2 moles of O. The molecular weightof the compound is(a) 3 (b) 12

(C) 32 (d) 44


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CHEMISTRY PATHSHALA

12

(3)

(25) The volume of gas at O.c and 700 mm pressure is 760 cc. The number of moleculespresent in this volume is(a) 1.88 × 1022 (b) 6.022×1023

(C) 18.8×1023 (d) 18.8×1022

(26) I mole of a diatomic element X2contains 34 and 40 moles of electrons and neutronsrespectively.the isotopic formula of the element is

(a) x3474

(b) x1737

(C) x3440

(d) x2040

(27) 2 moles of H atoms at NTP occupy a volume of(a) 11.2 litres (b) 44.8 litres

(C) 2 litres (d) 22.4 litres

(28) How many electron weigh one kilogram ?(a) 6.022×1023 (b)

108.91031

(C) 023.6108.9

101 8

(d) 5410

108.9023.6

(29) 1 amu is equal to

(a) 121

of C-12 (b) 141

of O-16

(C) 1g of H2 (d) 1.66×10-23 kg(30) 5 moles of a gas in closed vessel was heated from 300 K to 600 K. the pressure of

gas doubled The number of moles of the gas will be

(a) 5 (b) 2.5

(C) 10 (d) 20(31) One mole of oxygen gas is the volume of .

(a) 1 litre of oxygen at S.T.P.

(b) 32 litres of oxygen at S.T.P.

(c) 22.4 litres of oxygen at S.T.P.

(d) 6.02 × 1023 molecules of oxygen at any temperature and pressure.

(32) 5.6 litres of gas at N.T.P are found to have a mass of 11 g. The molecular mass ofthe gas is.

(a) 22 (b) 44 (c) 88 (d) 32


(33) The number of atoms of oxygen present in 10.6g of Na2CO3 will be.(a) 6.02 × 1022 (b) 12.04 × 1022 (c)1.806 × 1023 (d) 31.8

(34) Which of the following has the largest number of aloms ?(a) 0.5 g atom of Cu (b) 0.635 g of Cu

(c)0.25 mole of Cu (d) 3.35 × 1020 amu of Cu

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CHEMISTRY PATHSHALA

(4)

(35) The number of molecules present in a drop of water weighing 0.06 g is approxi-mately(a) 1012 (b) 2 × 1012 ( c) 3 × 1021 ( d) 4 × 1021

(36) Which of the following has maximum mass ?(a) 0. g atom of carbon

(b) 0.1 mol of ammonia

(c) 6.02 × 1022 molecules of hydrogen gas

(d)1120 cc of carbon dioxide.

(37) Total number of atoms present 17 g of NH3 is(a) 6.02 × 1023 (b) 2 × 6.02 × 1023 ( c) 3 × 6. 02 ×1023 ( d) 4 × 10-24 g

(38) The mass of one atom of hydrogen is approxmatelya) 1 g (b) 0 . 5 g ( c) 1 . 6 × 10-24 g ( d) 3.2 × 6.02 × 10-24g

(39) A gaseous mixture contains oxygen and nitrogen in the ratio of 1 : 4 by weight.Therefore the ratio of their number of molecules isa) 1 : 4 (b) 1 : 8 ( c) 7 : 32 ( d) 3 : 16

(40) Volume at N.T.P. of 0.22 g of CO2 is same as that of(a) 0.01 g of hydrogen.

(b) 0.085 g of NH3

(c) 320 mg of gaseous So2.

(d) All the the above.

(41) Mass of a mole of electrons is :(a) 0.20mg (b) 0.02mg

(c) 0.55mg (d) 1.00mg(42) 5.6 litres of oxygen at NTP is equivalent of

(a) 1 mole (b) 1/2 mole

(C) 1/4 Mole (d) 1/8 mole

CHEMISTRY PATHSHALA(43) The weight of 350 mL of diatomic gas at 0 C and 2 atm pressure is 1g. The wt. of one

atom is(a) 16/N (b) 32/N

(C) 16 N (d) 32 N (N is the Av. const.)


(a) 5 (b) 12

(C) 6.022 × 1023 (d) 12 × 6.022 × 1023

6C is-(45) Number of atoms in 12 g of 12

(C) 3.01 × 1011.5 (d) 6.02 × 1023

(44) The number of atoms present in 16 g of oxygen is(a) 6.05 × 1011.5 (b) 3.01 × 1023

(46) Which of the following contains the greatest number of oxygen atoms?(a) 1 g of O (b) 1g of O2

(C) 1 g of O3 (d) All have the same number of atoms

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(a) 27 (b) 21

(C) 5 (d) 8

(48) A gaseous oxide contains 30.4 % of nitrogen, one molecule of which contains onenitrogen atom. The density of the oxide relative to oxygen is -(a) 0.94 (b) 1.44

(C) 1.50 (d) 3.0

(49) Number of electrons in 1.8 ml of H2O is-(a) 6.023 × 1023 (b) 0.6022 × 1023

(C) 3.011 × 1023 (d) 6.022 × 1024

(50) 22.4 litres of water vapour at NTP, when condensed to water, occupies an approxi-mate volume of(a) 18 litres (b) 1 litre

(C) 1 mL (d) 18 ml

(51) Which of the following has the highest mass?(a) 1 g-atom of c (d) 3.011×1023 atoms of oxygen

(b) 1/2 mole of CH4 (C) 10 mL of water

(52) If the atomic weight of carbon were set at 24 amu, the value of the Avogadro con-stant would be(a) 6.022×1023 (b) 12.044×1023

(C) 3.011×1023 (d) none of these

(53) If 32 g of O2 contain 6.022×1023 molecules at NTP then 32g of S, under the sameconditions, will contain,(a) 6.022×1023 S (b) 3.011×1023 S (C) 12.044×1023 S (d) 1×1023 S

(54) Which of the following is correct ?(a) g-mol.wt = mol. wt in gm = wt. of 6.02 ×1023 atom

(b) Mole = g-mol.wt

(C) Mole = N molecules = 6.02 ×1023 Molecules

(d) None of the above


(47) The total number of atoms represented by the compound CuS04. 5H20 is -

(55) 11.2 Litres of a gas at STP weighs 14g. The gas could not be :(a) N20 (b) CO

(C) B2H6 (d) N2

(56) Atomic mass of an elements is(a) the actual mass of one atom of the element

(b) the relative mass of an atom of the element

(c) the average relative mass of different atoms of the element

(d) much different from the mass number of the element.

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(6)

(58) One atomic mass unit is equivalent to(a) 1.66 x 10-27 (b) 1.66 x10-27 kg (c) 1.66 x 10-27 (d) 1.66 x10-27 g

(59) The correct value of Avogadro’s number is(a) 6.02 × 1021 (b) 6.02 × 1022 (c) 6.02 × 1023 (d) 6.62 × 10-34

(60) Which one of the following statements is incorect ?.(a) One gram atom of carbon contains avogadro’s number of atoms.

(b) One mole of oxygen gas contains Avogadro’s number of atoms.

(c) One mole of hydrogen contains Avogadro’s number of atoms.

(d) One mole of electrons stands for 6.02x1023 electrons

(c) 1 mg of Na

(d) 1 mL of water(b) 1 mg of N2

(57) The atomic mass of an element is measured relative to the mass of(a) hydrogen atom (b) oxygen atom

(c) carbon-12 (d) isotopic mixture of 12C, 13C and 14C,

(62) Which sample contains the largest number of atoms?(a) 1 mg of C4H10

(c) 236.022 10

41 atoms of p

(d) 24.088 x 1023 atoms of p

(63) One mole of P4 molecules contain:

(a) 1 molecule of p(b) 4 molecules of p

(61) The no. of gram atoms of oxygen present in 0.3 g--- mole of (COOH)2.2H2O is:

(a) 0.6 (b) 1.8 (c) 1.2 (d) 3.6

is:

(a) 1.084 x 1025 (b) 6.022 x 1023 (c) 6.022 x 1022

(64.) The total number of protons, electrons and neutrons in 12 g of 12 c6

(d) 18

(a) N2

(65.) 11.2 litre of a gas at STP weighs 14 g. The gas could not be:(b) CO (c) B2H6 (d) N2O


66) Smallest particle of an element which may or may not have independent existence (a)a molecule (b)an atom (c) an ion (d)an electron

68) The number of atoms present in a molecule determine its (a) molecularity (b) basicity (c)acidity

(d) atomicity 69) When an electron is added to a unipositive ion we get (a)anion (b)cation (c) neutral atom (d) molecule

67) Swedish chemist J. Berzelius determined the (a)atomic no. (b)atomic volume (c)atomic mass (d)atomic density

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75) Simplest formula that gives us information about the simple ratio of atoms in a compound is called (a) structural formula (b) molecular formula (c) empirical formula (d) molar ratio 76) Percentage of oxygen in H2O is (a) 80% (b) 88.8% (c) 8.8% (d) 9.8% 77) More abundant isotope of an element is one with (a) even atomic no. (b) odd atomic no. (c) Even mass no. (d) odd mass no. 78) Large no. of isotopes are known for the elements whose masses are multiple of (a) two (b) four (c) six (d) eight


70) CO+ is an example of: (a) free radical (b) cationic molecular ion (c) an ionic molecular ion (d) stable molecule 71) Relative atomic mass is the mass of an atom of an element as compared to the mass of (a) oxygen (b) hydrogen (c) nitrogen (d) carbon 72) Isotopes are the sister atoms of the same element with similar chemical properties and different (a) atomic number (b) atomic mass (c) atomic volume (d) atomic structure 73) The instrument which is used to measure the exact masses of different isotopes of an element called (a) I.R. Spectrophotometer (b) U.V. Spectrophotometer (c) Mass Spectrometer (d) Colourimeter 74) Mass spectrometer separates different positive isotopic ions on the basis of their (a) mass value (b) m/e value (c) e/m value (d) change value

(d) 224014 dm3

79) When 0.01 kg of CaCO3 is decomposed the CO2 produced occupies a volume at S.T.P. (a) 2.2414 dm3 (b) 22.414 dm3 (c) 22414 dm3

80) The no. of covalent bond in 10gm of NH3 are (a) 6.022 x 1023 (b) 1.062 x 1023 (c) 10.62 x 1024 (d) 1.062 x 1024 81) No. of molecules present in 10gm of water are (a) 3.37 x 1023 (b) 33.7 x 1023 (c) 3.37 x 1024 (d) 3.037 x 1024 82) The no. of covalent bonds present in 10gm of water are (a) 6.074 x 1023 (b) 6.74 x 1023 (c) 6.074 x 1024 (d) 6.74 x 1024 83) The least no. of molecules present in 30 gm of (a) N2O (b) NO (c) NO2 (d) N2O3 84) Which of the following has highest percentage of nitrogen (a) (NH4)2SO4 (b) NH4H2PO4 (c) (NH4)2HPO4 (d) (NH4)3PO4

85) 0.1 mole of Na3PO4 completely dissociates in water to produce Na+ (a) 6.02 x 1022 (b) 6.02 x 1023 (c) 1.806 x 1023 (d) 1.806 x 1022

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(a)reactants (b)products (c) Reactants and products (d)all of above

88) Stoichiometry is the branch of chemistry which deals with the study of quantitative relationship among the various

89) 500 cm3 of H2 gas at STP contradictions of hydrogen (a)6.02 x 1023 b) 3.01 x 1022 (c)2.68 x 1022 (d) 1.34 x 1022

90) Largest number of H+ ions are produced by complete ionization of


100) The mass of one mole of electron is (a) 1.008 mg (b) 0.184 mg (c) 1.673 mg (d) 0.55 mg

99) The largest number of molecules are presenting (a) 3.6 gram of H2O (b) 4.8 gram of C2H5OH

98) Mole of SO2 contains

91) The Avogadro’s number is (a) 6.02 x 1024 (b) 6.02 x 10–24 (c) 6.02 x 10–23 (d) 6.02 x 1023 92) The largest number of H+ are produced by complete ionization of (a) 0.100 2 moles of HCl (b) 0.051 moles of H2SO4 (c) 0.0334 moles of H3PO4 (d) All of the above 93) A sample of pure matter is (a) element (b) compound (c) substance (d) mixture 94) nm stands for (a) Newton meter (b) Nanometer (c) Newton square meter (d) none of the above 95) One calorie is equal to (a) 4.184 J (b) 41.84 J (c) 0.4184 J (d) 0.04184 J 96) The number of moles of CO2 which contains 8.0 gm of oxygen (a) 0.25 (b) 0.50 (c) 1.0 (d) 1.50 97) 27 grams of Al will react completely with how much mass of O2 to produce Al2O3 (a) 8 gm of oxygen (b) 16 gm of oxygen (c) 32 gm of oxygen (d) 24 gm of oxygen

(a) 6.02 x 1023 atoms of oxygen (b) 18.1 x 1023 molecules of SO2 (c) 6.023 x 1023 atom of sulphur (d) 4 gram of SO2

(c) 2.8 gm of CO (d) 5.4 gms of N2O5

(a) 0.01 mole of HCl (b) 0.0050 mole of H2SO4 (c) 0.000334 moles of H3PO4 (d) all above

(c)which produces maximum no. of moles of product

(d)does not effect the amount of product

87) A limiting reactant is one

(a)which is present in least amount

(b)which produces minimum no. of moles of product

86) Efficiency of chemical reaction can be checked by calculating (a) amount of limiting reactant (b) amount of the reactant in excess (c) amount of the product formed (d) amount of the reactant unused w

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(1) a

(2) d

(3) c

(4) c

(5) a

(6) b

(7) a

(8) c

(9) a

(10) c

(11) a

(12) c, b

(13) c

(14) d

(15) d

(16) d

(17) d

(18) a

(19) d

(20) a

(21) d

(22) b

(23) b

(24) d

(25) a

(26) b

(27) d

(28) d

(29) a

(30) a

(31) c

(32) b

(33) c

(34) a

(35) c

(36) d

(37) d

(38) c

(39) c

(40) d

(41) c

(42) c

(43) a

(44) d

(45) c

(46) b

(47) b

(48) b

(49) a

(50) d

(51) a

(52) b

(53) a

(54) c

(55) a

(56) c

(57) c

(58) b

(59) c

(60) b

(61) b

(62) d

(63) d

(64) a

(65) d

66 67 68 69 70 b C d c b

71 72 73 74 75

d b c b c

76 77 78 79 80

b c b a d

81 82 83 84 85 a b d d c

86 87 88 89 90 c b d c d

91 92 93 94 95

d d a b a

96 97 98 99 100 a d c a d

Answer


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12 (b) 320g of sulphur - iBioKaare · (1) (1) Avogadro’s number represents the number of atoms in...

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