Basic concept chemistry s2

1.0 Introduction

  1. _ chemistry deals with the chemistry of
    elements other than carbon and of their
    (A) Organic (B) Physical
    (C) Inorganic (D) Bio
  2. The branch of chemistry which deals with the
    separation, identification and quantitative
    determination of the composition of different
    substances is called _ chemistry.
    (A) Organic (B) Inorganic
    (C) Analytical (D) Bio
    1.1 Importance and Scope of Chemistry
  3. Solar energy can be converted into electrical
    energy using
    (A) Daniel cell (B) Lithium ion cell
    (C) Photovoltaic cell (D) Ni cell
  4. _ cannot be carried out in a lab.
    (A) Photosynthesis (B) Reduction
    (C) Oxidation (D) Hydration
  5. The compound which is added to table salt for
    maintaining proper health is
    (A) KCl (B) KBr
    (C) NaI (D) MgBr2
    1.2 Historical Approach to Particulate Nature
    of Matter
  6. SI unit of velocity is
    (A) km s−1
    (B) km hr−1
    (C) m s−2
    (D) m s−1
  7. SI unit of temperature is
    (A) K (B) °C
    (C) °F (D) D
  8. Electrochemical equivalence has unit __.
    (A) kg m s−1
    (B) kg m2
    (C) kg C−1
    (D) kg m−1
  9. Magnitude of ‘pico−’ is _.
    (A) 10−12 (B) 10−15
    (C) 1012 (D) 1015
  10. One atmosphere is equal to
    (A) 101.325 K pa (B) 1013.25 K pa
    (C) 105
    Nm (D) 107
  11. Which of the following elements of matter
    would best convey that there is life on earth?
    (A) Oxygen (B) Hydrogen
    (C) Carbon (D) Iron
  12. Which of the following contains only one
    (A) Marble (B) Diamond
    (C) Glass (D) Sand
  13. Which one of the following is not an element?
    (A) Diamond (B) Graphite
    (C) Silica (D) Ozone
  14. The element similar to carbon is
    (A) Mg (B) Mn
    (C) Sn (D) Pb
    1.3 Laws of Chemical Combination
  15. The law of multiple proportions is illustrated
    (A) Carbon monoxide and carbon dioxide
    (B) Potassium bromide and potassium
    (C) Ordinary water and heavy water.
    (D) Calcium hydroxide and barium
  16. Two elements, X (Atomic mass 16) and Y
    (Atomic mass 14) combine to form
    compounds A, B and C. The ratio of different
    masses of Y which combine with fixed mass
    of X in A, B and C is 1:3:5. If 32 parts by
    mass of X combine with 84 parts by mass of Y
    in B, then in C, 16 parts by mass of X will
    combine with
    (A) 14 parts by mass of Y
    (B) 42 parts by mass of Y
    (C) 70 parts by mass of Y
    (D) 82 parts by mass of Y
  17. The volume of oxygen required for complete
    combustion of 0.25 cm3
    of CH4 at S.T.P is
    (A) 0.25 cm3
    (B) 0.5 cm3
    (C) 0.75 cm3
    (D) 1 cm3
  18. How many litres of ammonia will be formed
    when 2 L of N2 and 2 L of H2 are allowed to
    (A) 0.665 (B) 1.0
    (C) 4.00 (D) 1.33
  19. Two elements, A and B, combine to form a
    compound in which ‘a’ g of A combines with
    ‘b1’ and ‘b2’g of B respectively. According to
    law of multiple proportion _.
    (A) b1 = b2
    (B) b1 and b2 bear a simple whole number
    (C) a1 and b1 bear a whole number ratio
    (D) No relation exists between b1 and b2
    SECTION – 2
  1. 1.0 g of an oxide of A contained 0.5 g of A.
    4.0 g of another oxide of A contained 1.6 g of
    A. The data indicate the law of
    (A) Reciprocal proportions
    (B) Constant proportions
    (C) Conservation of energy
    (D) Multiple proportions
  2. Hydrogen and oxygen combine to form H2O2
    and H2O containing 5.93% and 11.29% of
    hydrogen respectively. The data illustrates
    (A) Law of conservation of mass
    (B) Law of constant proportions
    (C) Law of reciprocal proportions
    (D) Law of multiple proportions
  3. One unit volume of N2 reacts with 3 unit
    volumes of H2 to form 2 unit volumes of NH3.
    This is in accordance with
    (A) Avogadros law
    (B) Gay Lussac’s law
    (C) Law of conservation of mass
    (D) Law of chemical combination
    1.4 Dalton’s Atomic Theory
  4. _ proposed some symbols for some
    common atoms and molecules.
    (A) Democritus (B) Newton
    (C) Thompson (D) Dalton
    1.5 Concepts of Atoms and Molecules
  5. Atoms are the smallest particle of the _.
    (A) Compound (B) Substance
    (C) Mixture (D) Element
  6. Which one of the following properties of an
    element is not variable?
    (A) Valency
    (B) Atomic weight
    (C) Equivalent weight
    (D) Molar mass
    1.6 Atomic and Molecular Masses
  7. Which one of the following is not the
    standard for atomic mass?
    (A) 1
    1H (B) 12
    6 C
    (C) 14
    6 C (D) 16
    8 O
    27 Which of the following weighs the least ?
    (A) 2.0 gram mole of CO2.
    (B) 0.1 mole of sucrose ( C12 H22 O11).
    (C) 1 gram atom of calcium.
    (D) 1.5 mole of water.
  8. From the following masses, the one which is
    expressed nearest to the milligram is
    (A) 16 g (B) 16.4 g
    (C) 16.428 g (D) 1.64284 g
  9. If the equivalent weight of a trivalent metal is
    32.7, the molecular weight of its chloride will
    (A) 68.2 (B) 103.7
    (C) 204.6 (D) 32.7
  10. The mass of 1 × 1022 molecules of
    CuSO4.5H2O is
    (A) 41.59 g (B) 415.9 g
    (C) 4.159 g (D) 42.2 g
  11. The number of atoms in 6 amu of He is
    (A) 18
    (B) 18 × 6.022 × 1023
    (C) 54
    (D) 54 × 6.023 × 1023
    1.7 Avogadro’s Law
  12. The number of molecules in 22.4 dm3
    nitrogen gas at STP is
    (A) 6.023 × 1020 (B) 6.023 × 1023
    (C) 22.4 × 1020 (D) 22.4 × 1023
  13. Number of moles of water in 1 L of water with
    density 1 g/cc are
    (A) 55.56 (B) 45.56
    (C) 56.55 (D) 56.45
  14. 27 g of Al (Atomic mass = 27) will react with
    oxygen equal to
    (A) 24 g (B) 8 g
    (C) 40 g (D) 10 g
  15. The largest number of molecules is present in
    (A) 54 g of nitrogen peroxide
    (B) 28 g of carbon dioxide
    (C) 36 g of water
    (D) 46 g of ethyl alcohol
  16. How many moles of electrons weigh one
    (A) 6.023 × 1023 (B) 1
    × 1031
    (C) 6.023
    × 1054 (D) 1
    9.108 6.023 × × 108
  17. Which of the following has maximum number
    of atoms?
    (A) 18 g of H2O (B) 16 g of O2
    (C) 4.4 g of CO2 (D) 16 g of CH4
    7 Some Basic Concepts of Chemistry
    TARGET Publications Std. XI: Triumph Chemistry
  18. Which of the following contains more
    (A) 1 g CO2 (B) 1 g N2
    (C) 1 g H2 (D) 1 g CH4
  19. 1g-atom of nitrogen represents
    (A) 6.02 × 1023 N2 molecules
    (B) 22.4 L of N2 at N.T.P.
    (C) 11.2 L of N2 at N.T.P.
    (D) 28 g of nitrogen
  20. 1 atom of an element weighs 1.792 × 1022 g.
    The Atomic mass of the element is
    (A) 108 (B) 17.92
    (C) 1.192 (D) 64
  21. The number of sulphur atoms present in
    0.2 moles of S8 molecules is
    (A) 4.82 × 1023 (B) 9.63 × 1022
    (C) 9.63 × 1023 (D) 1.20 × 1023
  22. The mass of 1 atom of hydrogen is
    (A) 1 g (B) 0.5 g
    (C) 1.6 × 10−24 g (D) 3.2 × 10−24 g
  23. 1 mol of CH4 contains
    (A) 6.02 × 1023 atoms of H
    (B) 4 g atom of Hydrogen
    (C) 1.81 × 1023 molecules of CH4
    (D) 3.0 g of carbon
  24. Which of the following has smallest number
    of molecules
    (A) 0.1 mol of CO2 gas
    (B) 11.21 of CO2 gas at NTP
    (C) 22 g of CO2 gas
    (D) 22.4 g 103
    mL of CO2 gas
    1.8 Percentage Composition and Molecular
  25. Which pair of species have same percentage of
    (A) CH3COOH and C6H12O6
    (B) CH3COOH and C2H5OH
    (C) HCOOCH3 and C12H22O11
    (D) C6H12O6 and C12H22O11
  26. Two elements X (Atomic mass 75) and Y
    (Atomic mass 16) combine to give a
    compound having 75.8% X. The formula of
    the compound is
    (A) XY (B) XY2
    (C) X2Y2 (D) X2Y3
  27. The molecular mass of an organic compound
    is 78. Its empirical formula is CH. The
    molecular formula is
    (A) C2H4 (B) C2H2
    (C) C6H6 (D) C4H4
  28. Percentage of nitrogen in urea is about
    (A) 46 % (B) 85 %
    (C) 18 % (D) 28 %
  29. Which of the following has same molecular
    formula and empirical formula?
    (A) CO2 (B) C6H12O6
    (C) C2H2 (D) C2H2O4
  30. The empirical formula of a compound is
    CH2O. 0.0835 moles of the compound
    contains 1.0 g of hydrogen. Molecular formula
    of the compound is
    (A) C2H12O6 (B) C5H10O5
    (C) C4H8O8 (D) C3H6O3
    1.9 Chemical Reactions and Stoichiometry
  31. What mass of CaO will be obtained by heating
    3 mole of CaCO3 [Atomic mass of Ca = 40] ?
    (A) 150 g (B) 168 g
    (C) 16.8 g (D) 15 g
  32. Volume of O2 required to produce 44 g of CO2
    by combustion of carbon is
    (A) 2.24 L (B) 22400 mL
    (C) 22.4 mL (D) 224 mL
  33. 3 g of H2 reacts with 29 g of O2 to yield water.
    Which is the limiting reactant?
    (A) H2 (B) O2
    (C) H2O (D) none of there
  34. The unit J Pa−1 is equivalent to
    (A) m3
    (B) cm3
    (C) dm3
    (D) dm−3
  35. What volume of ammonia would be formed
    when 0.36 dm3
    of nitrogen reacts with
    sufficient amount of hydrogen? (all volumes
    are measured under same conditions of
    temperature and pressure)
    (A) 0.36 dm3
    (B) 0.72 dm3
    (C) 0.18 dm3
    (D) 0.12 dm3
  36. If the law of conservation of mass was to hold
    true, then 20.8 g of BaCl2, on reaction with 9.8 g
    of H2SO4 will produce 7.3 g of HCl and __
    (A) 11.65 g (B) 23.3 g
    (C) 25.5 g (D) 30.6 g
  1. Two containers of the same size are filled
    separately with H2 gas and CO2 gas. Both the
    containers under the same T and P will contain
    the same
    (A) Number of atoms.
    (B) Weight of gas.
    (C) Number of molecules.
    (D) Number of electrons.
  2. A compound made of two elements A and B
    are found to contain 25% A (Atomic mass
    12.5) and 75% B (Atomic mass 37.5). The
    simplest formula of the compound is
    (A) AB (B) AB2
    (C) AB3 (D) A3B
  3. Hydrogen reacts with nitrogen to form
    ammonia as: N2(g) + 3H2(g) ⎯→ 2NH3(g)
    The amount of ammonia that would be
    produced if 200 g of H2 reacts with N2 is
    (A) 1032.2 g (B) 11332 g
    (C) 1133.3 g (D) 8692.6 g

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