: EXERCISE :
1.
A sample of ammonium phosphate (NH4)3PO4
contains 6.36 mol of hydrogen atoms. The number of moles of oxygen atom in the
sample : (atomic mass of N = 14.04, H = 1, P = 31, O=16)
(a) 0.265 (b) 0.795 (c) 2.12 (d) 4.14
(a) 0.265 (b) 0.795 (c) 2.12 (d) 4.14
2.
The number of sulphate ions in 1000 mL of 0.001 M H2SO4
is :
(a) 6.023 ´ 1023 (b) 6.023 ´ 1022 (c) 6.023 ´ 1021 (d) 6.023 ´ 1020
(a) 6.023 ´ 1023 (b) 6.023 ´ 1022 (c) 6.023 ´ 1021 (d) 6.023 ´ 1020
3.
30 mL of a gaseous hydrocarbon requires 90 mL of O2
for complete combustion and 60 mL of CO2 is formed in the process.
The molecular formula of hydrocarbon will be :
(a) C2H2 (b) CH4 (c) C2H4 (d) C2H6
(a) C2H2 (b) CH4 (c) C2H4 (d) C2H6
4.
A sample of mixture of CaCl2 and NaCl weighing
4.22 g was treated to precipitate all the Ca as CaCO3. This CaCO3
is then heated and quantitatively converted into 0.959 g of CaO. Calculate the
percentage of CaCl2 in the mixture : (Automic mass of Ca = 40, O =
16, C = 12, and Cl = 35.5)
(a) 31.5% (b) 21.5% (c) 45.04% (d) 68.48%
(a) 31.5% (b) 21.5% (c) 45.04% (d) 68.48%
5.
A metal oxide is reduced by heating it in a stream of
hydrogen. It is found that after complete reduction,3.15 g of oxide yielded
1.05 g of metal. From the above data we can say that :
(a) the atomic weight of metal is 8 (b) the atomic weight of metal is 4
(c) the equivalent weight of metal is 4 (d) the equivalent weight of metal is 8
(a) the atomic weight of metal is 8 (b) the atomic weight of metal is 4
(c) the equivalent weight of metal is 4 (d) the equivalent weight of metal is 8
6.
Cyclohexanol is dehydrated to cyclohexene on heating with
conc. H2SO4. The cyclohexene obtained from 100 g
cyclohexanol will be : (If yield of reaction is 375%)
(a) 61.5 g (b) 75.0 g (c) 20.0 g (d) 41.0 g
(a) 61.5 g (b) 75.0 g (c) 20.0 g (d) 41.0 g
7.
The composition of residual mixture will be if 30 g of Mg
combines with 30 g of oxygen :
(a) 40g MgO + 20g O2 (b) 45g MgO + 15g O2
(c) 50g MgO + 10g O2 (d) 60g MgO only
(a) 40g MgO + 20g O2 (b) 45g MgO + 15g O2
(c) 50g MgO + 10g O2 (d) 60g MgO only
8.
A metal oxide has the formula A2O3. It
can be reduced by hydrogen to give free metal and water. 0.1596 g of the metal
oxide requires 6 mg of hydrogen for complete reduction. What is the atomic
weight of metal?
(a) 52.3 (b) 57.5 (c) 55.8 (d) 59.3
(a) 52.3 (b) 57.5 (c) 55.8 (d) 59.3
9.
The simplest formula of a compound containing 50% of element
X (at. Wt 10) and 50% of element Y (at wt 20) is -
(a) XY (b) X2Y (c) XY2 (d) X2Y3
(a) XY (b) X2Y (c) XY2 (d) X2Y3
10.
An organic compound has an empirical formula CH2O,
its vapour density is 45. The molecular formula of the compound is.
(a) CH2O (b) C2H5O (c) C2H2O (d) C3H6O3
(a) CH2O (b) C2H5O (c) C2H2O (d) C3H6O3
11.
An oxide of metal (M) has 40% by mass of oxygen. Metal M has
relative atomic mass of 24. The empirical formula of the oxide is.
(a) M2O (b) M2O3 (c) MO (d) M3O4
(a) M2O (b) M2O3 (c) MO (d) M3O4
12.
If a mixture containing 3 moles of hydrogen and 1 mole of
nitrogen is converted completely into ammonia, the ratio of initial and final
volumes under the same temperature and pressure would be.
(a) 3 : 1 (b) 1 : 3 (c) 2 : 1 (d) 1 : 2
(a) 3 : 1 (b) 1 : 3 (c) 2 : 1 (d) 1 : 2
13.
18 g of water contains -
(a) 1 g atom of hydrogen (b) 2 g atoms of hydrogen (c) 3 g atoms of hydrogen (d) None
(a) 1 g atom of hydrogen (b) 2 g atoms of hydrogen (c) 3 g atoms of hydrogen (d) None
14.
40 ml of H2S and 40 ml Cl2 are mixed
together. The volume of the resulting gas at the same temperature and pressure
will be -
(a) 40 ml (b) 80 ml (c) 120 ml (d) 160 ml
(a) 40 ml (b) 80 ml (c) 120 ml (d) 160 ml
15.
How many gram atoms of S are present in 80.25 g of S.
(a) 2.5 (b) 32 (c) 5 (d) 80.25 ´ 32
(a) 2.5 (b) 32 (c) 5 (d) 80.25 ´ 32
16.
The weight of 350 ml of diatomic gas at 0 °C and 2 atm pressure is 1 gm. What is the atomic weight of
the substance.
(a) 17.7 (b) 15.99 (c) 0.05 M. NaCl (d) 6 M H+
(a) 17.7 (b) 15.99 (c) 0.05 M. NaCl (d) 6 M H+
17.
What will be present in the solution when 50 ml. Of 0.1 (M)
HCl is mixed with 50 ml. of 0.1 (M) NaOH.
(a) 4.5 mol of H+ (b) 0.05 mol of OH- (c) 40 (d) 52
(a) 4.5 mol of H+ (b) 0.05 mol of OH- (c) 40 (d) 52
18.
0.2 mole of HCl and 0.1 mole of barium chloride were
dissolved in water to produce a 500-ml solution. The molarity of the Cl- ions is.
(a) 0.06 M (b) 0.09 M (c) 0.12 M (d) 0.80 M
(a) 0.06 M (b) 0.09 M (c) 0.12 M (d) 0.80 M
19.
How many moles of potassium chlorate is to be heated to
produce 11.2 litre oxygen.
(a)
(b) 
(c) 
(d) 
(a)
(b) (c) (d)
20.
4.4 gm of an unknown gas occupies 2.24 litre of volume of
STP. The gas may be.
(a) Carbon dioxide (b) Carbon monoxide (c) Oxygen (d) Sulpur dioxide
(a) Carbon dioxide (b) Carbon monoxide (c) Oxygen (d) Sulpur dioxide
21.
What quantity of limestone (CaCO3) on heating will
give 56 Kg of CaO.
(a) 1000 kg (b) 10 kg (c) 50 kg (d) 100 kg
(a) 1000 kg (b) 10 kg (c) 50 kg (d) 100 kg
22.
Calculate the weight of lime (CaO) obtained by heating 200 kg
of 95% pure lime stone (CaCO3).
(a) 104.0 kg (b) 105.4 kg (c) 212.8 kg (d) 106.4 kg
(a) 104.0 kg (b) 105.4 kg (c) 212.8 kg (d) 106.4 kg
23.
100 ml of PH3 when decomposes produced phosphorus
and hydrogen. The change in volume is.
(a) 50 ml increase (b) 500 ml decrease (c) 900 ml decrease (d) None
(a) 50 ml increase (b) 500 ml decrease (c) 900 ml decrease (d) None
24.
A metal oxide is reduced by passing H2 gas. 3.15
gm of oxide on complete reduction gives 1.05 gm. metal. We concluded that -
(a) atomic weight of metal is 4 (b) eqvivalent weight of metal is 8 (c) eqvivalent weight of metal is 4 (d) atomic weight of metal is 8
(a) atomic weight of metal is 4 (b) eqvivalent weight of metal is 8 (c) eqvivalent weight of metal is 4 (d) atomic weight of metal is 8
25.
A sample of calcium carbonate is 80% pure. 25 gm of this
sample is treated with excess of HCl. How much volume of CO2 will be
obtained at NTP -
(a) 4.48 litre (b) 5.6 litre (c) 11.2 litre (d) 2.24 litre
(a) 4.48 litre (b) 5.6 litre (c) 11.2 litre (d) 2.24 litre
26.
What is the molarity of 36% by strength of HCl (Given sp.
Gravity of pure HCl is 1.5).
(a) 16 M (b) 36 M (c) 14.79 M (d) 15.88 M
(a) 16 M (b) 36 M (c) 14.79 M (d) 15.88 M
27.
Mass of H2O in 1000 kg CuSO4. 5H2O
is.
(a) 360.5 kg (b) 36.05 kg (c) 3605 kg (d) 3.605 kg
(a) 360.5 kg (b) 36.05 kg (c) 3605 kg (d) 3.605 kg
28.
1 gm. Metal carbonate requires 200 ml. of 0.1 N HCl for
complete neutralization. What is the equivalent weight of metal carbonate -
(a) 50 (b) 40 (c) 20 (d) 100
(a) 50 (b) 40 (c) 20 (d) 100
29.
In an experiment 10 ml of AgNO3 (0.1N) solution is
added to 20 ml of decinormal HCl. After the precipitation of AgNO, excess
of HCl is titrated with decinormal NaOH solution. What is the volume of NaOH
used in the titration -
(a) 10 ml (b) 20 ml (c) 5 ml (d) 30 ml
(a) 10 ml (b) 20 ml (c) 5 ml (d) 30 ml
30.
The volume of water added to 50 ml. 0.5 M NaOH so that its
strength becomes 10 mg NaOH per ml. -
(a) 100 ml (b) 200 ml (c) 250 ml (d) 500 ml
(a) 100 ml (b) 200 ml (c) 250 ml (d) 500 ml
31.
The molarity of a solution made by mixing 50 ml of conc. H2SO4(36N)
with 50 ml. of water,is
(a) 36 M (b) 18 M (c) 9 M (d) 6 M
(a) 36 M (b) 18 M (c) 9 M (d) 6 M
32.
Molarity of 720 g of pure water -
(a) 40 M (b) 4 M (c) 55.5 M (d) Unpredictable
(a) 40 M (b) 4 M (c) 55.5 M (d) Unpredictable
33.
A certain aqueous
solution of FeCl3 (formula mass = 162) has a density of 1.1 g/ml and
contains 20.0% FeCl3. Molar concentration of this solution is -
(a) 0.028 (b) 0.163 (c) 1.35 (d) 1.47
(a) 0.028 (b) 0.163 (c) 1.35 (d) 1.47
34.
The density of liquid ethanol is 0.7893 g mL-1 at
20° C. If 1.2 mol of ethanol are needed for a particular
experiment, what volume of ethanol should be measured out -
(a) 55 mL (b) 58 mL (c) 70 mL (d) 79 mL
(a) 55 mL (b) 58 mL (c) 70 mL (d) 79 mL
35.
The most abundant element dissolved in sea water is Cl at a
conc. of 19 gm/kg of sea water. The volume of earth’s ocean is 1.4 ´ 1021 litre. How many gm atoms of Cl are
potentially available from the oceans (density of sea water is 1 gm/cc) -
(a) 7.6 ´ 1020 (b) 27 ´ 1021 (c) 27 ´ 1024 (d) 96 ´ 1023
(a) 7.6 ´ 1020 (b) 27 ´ 1021 (c) 27 ´ 1024 (d) 96 ´ 1023
36.
A mole of any substance is related to :
(a) number of particles (b) volume of gaseous substances (c) mass of a substances (d) all of these
(a) number of particles (b) volume of gaseous substances (c) mass of a substances (d) all of these
37.
2 g of O2 at NTP occupies the volume :
(a) 2.4 litre (b) 4.8 litre (c) 1.4 litre (d) 1.2 litre
(a) 2.4 litre (b) 4.8 litre (c) 1.4 litre (d) 1.2 litre
38.
Normally of 0.3 M H3PO4 solution is:
(a) 0.3 N (b) 0.4 N (c) 0.6 N (d) 0.9 N
(a) 0.3 N (b) 0.4 N (c) 0.6 N (d) 0.9 N
39.
The volume of 1.0 g of hydrogen in litres at NTP is :
(a) 6.8 litre (b) 10.44 litre (c) 11.2 litre (d) 14.56 litre
(a) 6.8 litre (b) 10.44 litre (c) 11.2 litre (d) 14.56 litre
40.
4 g caustic soda is dissolved in 100 cc of solution. The normality of solution is :
(a) 0.2 (b) 0.5 (c) 1.0 (d) 1.5
(a) 0.2 (b) 0.5 (c) 1.0 (d) 1.5
41.
The vapour density of a gas A is four times than that of B.
If molecular mass of B is 1, then molecular mass of A is :
(a) 1 (b) 2 (c) ¼ (d) 4
(a) 1 (b) 2 (c) ¼ (d) 4
42.
The number of atoms present in10.8 g of silver is [atomic
weight of silver = 108]
(a) 6.123 x 1023 (b) 6.312 x 1022 (c) 6.023 x 1022 (d) 6.076 x 1023
(a) 6.123 x 1023 (b) 6.312 x 1022 (c) 6.023 x 1022 (d) 6.076 x 1023
43.
The correct relationship between molecualr mass and vapour
density is :
(a) V.D. = 2M (b) V.D. = M/2 (c) M = (V.D.)½ (d) V.D. = M2
(a) V.D. = 2M (b) V.D. = M/2 (c) M = (V.D.)½ (d) V.D. = M2
44.
0.30 g of a volatile liquid displaces 90.0 cm3 of
air at STP in the Victor Meyer’s method. The molecular mass of the liquid is :
(a) 54.44 g (b) 62.64 g (c) 68.76 g (d) 74.66 g
(a) 54.44 g (b) 62.64 g (c) 68.76 g (d) 74.66 g
45.
The specific heat of metal is 0.16. Its atomic weight is :
(a) 8 (b) 16 (c) 32 (d) 40
(a) 8 (b) 16 (c) 32 (d) 40
46.
A metal oxide contains 20% oxygen by weight. Its equivalent
weight is :
(a) 32 (b) 40 (c) 64 (d) 72
(a) 32 (b) 40 (c) 64 (d) 72
47.
From the complete decomposition of 20 g CaCO3 at
STP the volume of CO2 obtained is :
(a) 2.24 litre (b) 4.48 litre (c) 20 litre (d) 22.4 litre
(a) 2.24 litre (b) 4.48 litre (c) 20 litre (d) 22.4 litre
48.
One mole of a substance present in 1 kg of solvent. The
correct statement regarding above solution is :
(a) strength g/g (b) molar concentration (c) molal concentration (d) normality
(a) strength g/g (b) molar concentration (c) molal concentration (d) normality
49.
0.25 mol of P4 molecules contains atoms :
(a) 1.764 (b) 3.448 (c) 6.023 x 1023 (d) 8.086 x 1023
(a) 1.764 (b) 3.448 (c) 6.023 x 1023 (d) 8.086 x 1023
50.
800 g of a 40% solution by weight was cooled. 100 g of solute
precipitated. The percentage composition of remaining solution is :
(a) 31.4% (b) 55.6% (c) 67.8% (d) 69.9%
(a) 31.4% (b) 55.6% (c) 67.8% (d) 69.9%
ANSWER KEY :
QUE.
|
1
|
2
|
3
|
4
|
5
|
6
|
7
|
8
|
9
|
10
|
ANS.
|
c
|
d
|
c
|
c
|
c
|
a
|
c
|
c
|
b
|
d
|
QUE.
|
11
|
12
|
13
|
14
|
15
|
16
|
17
|
18
|
19
|
20
|
ANS.
|
c
|
c
|
b
|
b
|
a
|
b
|
c
|
d
|
b
|
a
|
QUE.
|
21
|
22
|
23
|
24
|
25
|
26
|
27
|
28
|
29
|
30
|
ANS.
|
d
|
d
|
a
|
c
|
a
|
c
|
a
|
a
|
a
|
d
|
QUE.
|
31
|
32
|
33
|
34
|
35
|
36
|
37
|
38
|
39
|
40
|
ANS.
|
c
|
c
|
c
|
c
|
a
|
d
|
c
|
d
|
c
|
c
|
QUE.
|
41
|
42
|
43
|
44
|
45
|
46
|
47
|
48
|
49
|
50
|
ANS.
|
d
|
c
|
b
|
d
|
b
|
a
|
b
|
c
|
c
|
a
|
