M.C.Qs on Introduction to Fundamental Concepts of Chemistry..... Unit # 1

1.      Which one of the following statements is incorrect regarding mole concept?
(a)
A mole is the gram atomic or gram molecular mass or gram formula mass of a substance.
(b)
1 mole of all elements contains 6.02 x 1023 particles irrespective of their states.
(c)
1 mole of all gases at s.t.p. occupies 22.4 m3.
(d)
11.2 dm3 of hydrogen gas at s.t.p. weighs 1 g.

2.      Which one of the following statements is incorrect regarding empirical formula?
(a)
It shows the simplest atomic ratio.
(b)
Empirical formula of acetic acid and glucose is CH2O.
(c)
Ionic or inorganic compounds are usually represented by their empirical formulae.
(d)
It is an integral multiple of molecular formula.

3.      Which one of the following statements is false regarding molar volume?
(a)
It is the volume occupied by 1 mole of any gas at s.t.p.
(b)
Its value is same at all temperature and pressures.
(c)
Its value is 22.4 dm3 (liter) or 22400 cm3 (ml) or 0.0224 m3.
(d)
Its value is computed by using expression RT/P.

4.      An element has an atomic number of 11, the element is:
(a)
A metal with oxidation number of +1.
(b)
A metal with an oxidation number of +2.
(c)
An inert gas.
(d)
A non-metal with oxidation number of -1.

5.      Isotopes differ in:
(a)
Arrangement of electrons in orbitals.
(b)
The extent to which they may be affected in electromagnetic field.
(c)
Properties which depend upon mass
(d)
Chemical properties.

6.      Which one of the following statements is not true?
(a)
Isotopes with even atomic masses are comparatively abundant.
(b)
Isotopes with odd atomic masses are comparatively abundant.
(c)
Isotopes with even atomic masses and even atomic numbers are comparatively abundant.
(d)
Isotopes with even atomic masses and odd atomic numbers are comparatively abundant.

7.      Many elements have fractional atomic masses. This is because:
(a)
The mass of the atom is itself fractional.
(b)
Atomic masses are average masses of isobars.
(c)
Atomic masses are average masses of isotopes.
(d)
Atomic masses are average masses of isotopes proportional to their relative abundance.

8.      A limiting reactant is the one which:
(a)
Is taken lesser quantity in volume compared to the other reactants.
(b)
Is taken in lesser quantity grams as compared to other reactants.
(c)
Produces the minimum amount of the product under consideration.
(d)
Gives the maximum amount of the product which is required.

9.      Which one of the following statement is not true?
(a)
The empirical and molecular formulae of some compound are same.
(b)
Stoichiometric calculations can only be done if no side reaction occurs.
(c)
A limiting reactant is consumed at the end of the reaction.
(d)
Actual yield is always greater than the theoretical yield.

10.    Which one of the following statement is not true?
(a)
In stoichiometric calculations, low of definite proportions is definitely obeyed.
(b)
Isotopes of an element differ in number of protons and so their masses are different.
(c)
Stoichiometric amounts are the amounts of reactants and products in a balanced chemical equation.
(d)
Isotones are atoms of the element having same number of neutrons.

11.    A quantity containing Avogadro’s number of particles is called:
(a)
Gram atom
(b)
Gram molecule
(c)
Mole
(d)
Gram formula

12.    One mole of hydrogen gas at s.t.p. contains how many atoms?
(a)
6.02x1023
(b)
3.01x1024
(c)
1.2x1024
(d)
12.04x1046

13.    how many significant figures are contained in 0.00050890400?
(a)
6
(b)
4
(c)
8
(d)
11

14.    16 g of oxygen has a volume of:
(a)
22.4 dm3
(b)
11.2 dm3
(c)
5.6 dm3
(d)
22400 cm3

15.    11.2 dm3 of Cl2 gas at s.t.p. weighs:
(a)
71g
(b)
17 g
(c)
35.5 g
(d)
37 g

16.    Which one of the following represents the value of 1 a.m.u.?
(a)
1.667x10-24 g
(b)
1.667x10-23 g
(c)
1.667x10-27 g
(d)
1.667x10-28 g

17.    What is the ratio of the weight of water formed to the weight of Hydrogen used in the formation of water?
(a)
1 : 8
(b)
1 : 9
(c)
8 : 1
(d)
9 : 1

18.    The percentage of which of the following element in an organic compound cannot be measured directly?
(a)
Carbon
(b)
Hydrogen
(c)
Oxygen
(d)
Sulphur

19.    Stoichiometric calculation of a reaction gives us …………yield.
(a)
Actual
(b)
Theoretical
(c)
Both a and b
(d)
None of the above

20.    Actual yield is always …………. than the theoretical yield.
(a)
More
(b)
Less
(c)
Both a and b
(d)
None of the above

21.    The mass of one mole of electrons is:
(a)
1.008 mg
(b)
0.55 mg
  (c)
0.184 mg
(d)
1.673 mg

22.    The number of moles of CO2 which contain 8.0 g of oxygen:
(a)
0.25
(b)
0.50
(c)
1.0
(d)
1.50

23.    The largest number of molecules are present in:
(a)
3.6 g of water
(b)
4.8 g of C2H5OH
(c)
2.8g of CO
(d)
5.4 g of N2O5

24.    One mole of SO2 contains:
(a)
6.02 x 1023 atoms of oxygen
(b)
6.02 x 1023 atoms of sulphur
(c)
18.1 x 10 23 molecules of SO2
(d)
4 gram atoms of SO2

25.    The formula of KAl(SO4)2 represents a total of:
(a)
6 atoms
(b)
7 atoms
(c)
12 atoms
(d)
14 atoms

26.    How many neutrons are contained in the nucleus of an element with Z=27 and A= 59:
(a)
27
(b)
32
(c)
59
(d)
86
27.    How many gram of NaOH are needed to make 1000g of a 5% solution?
(a)
5g
(b)
500g
(c)
40g
(d)
50g

28.    Chlorine atom and chloride ions
(a)
Have same number of protons
(b)
Have same number of electrons
(c)
Are allotropes of chlorine
(d)
Are chemically identical

29.    Which of the following formula represents an acid anhydride?
(a)
CaO
(b)
H2O
(c)
H2SO4
(d)
SO3

30.    Which of the following formula represents a basic anhydride?
(a)
MgO
(b)
CrO3
(c)
CO
(d)
NO

31.    The basic oxide in the given list is:
(a)
N2O5
(b)
P4O6
(c)
Sb4O6
(d)
Bi2O3

32.    If an element M forms an oxide with formula MO, which of the following is a correct formula:
(a)
MCl
(b)
MS
(c)
MCl2
(d)
 Both b and c

33.    nm is …………. than μm.
(a)
Equal to
(b)
Less
(c)
Greater
(d)
All of the above

34.    Which one is large than dm3?
(a)
cm3
(b)
Liter
(c)
m3
(d)
ml

35.    The decimal equivalent of 1/60 to three significant figures is:

(a)
0.156
(b)
0.0166
(c)
0.00166
(d)
1.666 x10−2

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