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Atoms and Molecules Test - 52

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Atoms and Molecules Test - 52
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Weekly Quiz Competition
  • Question 1
    1 / -0
    A piece of aluminum foil has a mass of 27 grams. About how many atoms does this foil contain?
    Solution
    The atomic mass of Al is 27 g/mol.

    Hence, 27 g of Al corresponds to 1 mole.

    1 mole of any element contains Avogadro's number of atoms.

    Hence, 27 g ( 1 mole ) of Al contains  6.02×1023\displaystyle  6.02 \times 10^{23} atoms.

     Hence the correct option is B.
  • Question 2
    1 / -0
    Which law states that in a chemical reaction, the total mass of the products is equal to the total mass of the reactants?
    Solution
    The law which states that in a chemical reaction, the total mass of the products is equal to the total mass of the reactants is known as the "Law of conservation of mass".
  • Question 3
    1 / -0
    An atom differs from its ion in:
    Solution
     An atom differs from its ion in number of electrons. For example, H\displaystyle H atom has 1 electron. Whereas H+\displaystyle H^+ ion has 0 electrons. On the other hand, H\displaystyle H^- ion has 2 electrons.
  • Question 4
    1 / -0
    The size of the nucleus is measured in _______ units.
    Solution
    The size of the nucleus is measured in fermi units.
     1 fermi =1015 m\displaystyle \ 1 \ fermi  = 10^{-15} \ m .
  • Question 5
    1 / -0
    Barium chloride reacts with sodium sulfate to form barium sulfate and sodium chloride. Then, according to the law of conservation of mass:
    Solution
    BaCl2+Na2SO4BaSO4+2NaClBaCl_2 + Na_2SO_4 \rightarrow BaSO_4 + 2NaCl
    The total mass of the reactants is equal to the total mass of products.
    Hence, option C is correct.
  • Question 6
    1 / -0
    The symbols of lead and mercury are _________ respectively.
    Solution

    Lead is a chemical element with atomic number 82 and symbol Pb comes from the Latin word plumbumplumbum. It is a soft and malleable metal with a density exceeding that of most common materials. Mercury is a chemical element with symbol Hg and atomic number 80. It is commonly known as quicksilver and was formerly named hydrargyrumhydrargyrum.

  • Question 7
    1 / -0
    A balanced chemical equation  supports
    Solution
    A balanced chemical equation supports "Law of conservation of mass". Law of conservation of mass states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations. According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.
  • Question 8
    1 / -0
    1 amu=1121\ amu = \dfrac{1}{12} the mass of one:
    Solution

    An atomic mass unit (symbolized amu) is defined as precisely 1/12 the mass of an atom of carbon-12. The carbon-12 (C12C-12) atom has six protons and six neutrons in its nucleus. In imprecise terms, one amu is the average of the proton rest mass and the neutron rest mass.

    Hence, the correct option is A\text{A}

  • Question 9
    1 / -0
    Nitrogen reaction with oxygen to form nitrous oxide.

    What will be the volume ratio of the reactants and products of the given reaction?
    2N2+O22N2O2N_{2}+O_{2}\rightarrow 2N_{2}O
    Solution
    2N2+O22N2O2N_{2}+O_{2}\rightarrow 2N_{2}O

    The Law of chemical combination states that the Ratio of reactants & products are Reactions coefficients or stoichiometry coefficients.
    Ratio =2:1:2= 2:1:2

    Hence, the correct option is (D)(D).
  • Question 10
    1 / -0
    The mass of 5 moles of H2SO4H_2SO_4 is:
    Solution

    The molar mass of hydrogen (HH) is 11

    Molar mass of sulphur (SS) is 3232

    Molar mass of oxygen (OO) is 1616

    We can calculate the molar mass of H2SO4H_2SO_4 by adding the molar masses of all the atoms in the molecule.

    So, 

    molar mass of H2SO4=(2×molar mass of H)+(molar mass of S)+(4×molar mass of O)molar\ mass\ of\ H_2SO_4 = (2 \times molar\ mass\ of\ H) + (molar\ mass\ of\ S) + (4 \times molar\ mass\ of\ O) 

    = (2×1)+(32)+(4×16)(2 \times 1) + (32) + (4 \times 16) 

    = 9898

    We know that molar mass of a substance is defined as the mass of 11 mol of that substance. So, we can write it as follows:

    Mass of 11 mol of H2SO4H_2SO_4 = Molar mass of H2SO4H_2SO_4 = 9898

    Hence, mass of 55 moles of H2SO4H_2SO_4 = 5×985 \times 98 = 490490

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