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Q.1 Four one litre flasks are separately filled with the gases
hydrogen, helium, oxygen and
ozone at the same room temperature and pressure. The ratio of total number of atoms of
these gases present in the different flasks would be -
ozone at the same room temperature and pressure. The ratio of total number of atoms of
these gases present in the different flasks would be -
(A) 1 : 1 : 1 : 1 (B)
1 : 2 : 2 : 3
(C) 2 : 1 : 2 : 3 (D)
3 : 2 : 2 : 1
Q.2 The atomic masses of
two elements A and B are 20 and 40 respectively,
if x gm of A contains y atoms, how many atoms are present in 2x gm of B ?
if x gm of A contains y atoms, how many atoms are present in 2x gm of B ?
(A) y (B) 2y
(C) y/2 (D)y/4
Q.3 If mole percentage of C–12 and C–14 in nature is 98% and 2%
respectively,
then the number of C–14 atoms in 12 g of carbon is -
then the number of C–14 atoms in 12 g of carbon is -
(A) 1.2 × 1022 (B) 3.01 × 1022
(C) 5.88 × 1023 (D) 6.02 × 1023
Q.4 A vessel contains 8 gram TiO2,
2.4 gram carbon and 28.4 gram Cl2.
Maximum mass of TiCl4 which can be produced is -
Maximum mass of TiCl4 which can be produced is -
3TiO2(s)
+ 4C(s) + 6Cl2(g) ® 3TiCl4(g) + 2CO2(g)
+ 2CO(g)
(Consider reaction goes to completion ; atomic mass of Ti
= 48)
(A) 1.90 gram (B)
28.5 gram
(C) 19 gram (D)
38 gram
Q.5 Total number
of atoms of all elements present in 1 mole of ammonium dichromate is ?
(A) 14 (B)
19
(C) 6 x 1023 (D) 114 x 1023
Q.6 25 grams of oleum
contains 30% free SO3. Strength of oleum is -
(A) 130% (B)
106.75 %
(C) 115% (D) 110
Q.7 25 gram of A
sample of oleum is labelled as 110%. The amount of H2O
which should be added to this sample to get 50 % H2SO4(w/w) is -(assuming densily of H2O = 1 g/ml)
which should be added to this sample to get 50 % H2SO4(w/w) is -(assuming densily of H2O = 1 g/ml)
(A) 25 gram (B)
20 gram
(C) 30 gram (D)
27.5 gram
Q.8 The
number of atoms contained in 11.2 L of SO2 at N.T.P. are -
(A) 3/2 x
6.02 x 1023 (B) 2 x 6.02 x
1023
(C) 6.02 x 1023 (D) 4 x 6.02 x 1023
Q.9 The vapour
density of gas A is four times that of B. If molecular mass of B is M,
then molecular mass of A is -
then molecular mass of A is -
(A) M (B) 4M
(C) 1/4 M (D)
2M
Q.10 On analysis, a certain compound
was found to contain iodine and oxygen in the
ratio of 254 gm of iodine (at. mass 127) and 80 gm oxygen (at. mass 16).
What is the formula of the compound -
ratio of 254 gm of iodine (at. mass 127) and 80 gm oxygen (at. mass 16).
What is the formula of the compound -
(A) IO (B) I2O
(C) I5O3 (D) I2O5
Q.11 The hydrated
salt Na2SO4.nH2O,
undergoes 55% loss in weight on
heating and becomes anhydrous. The value of n will be
heating and becomes anhydrous. The value of n will be
(A) 5 (B) 3 (C) 7 (D)
10
Q.12 The mass of oxygen that would
be required to produce enough CO,
which completely reduces 1.6 kg Fe2O3 (at. mass Fe = 56) is -
which completely reduces 1.6 kg Fe2O3 (at. mass Fe = 56) is -
(Fe2O3 + 3CO ® 2Fe + 3CO2)
(A) 240 gm (B)
480 gm
(C) 720 gm (D)
960 gm
Q.13 12g of Mg (atm. mass 24) will
react completely with acid to give -
(A) One mol of H2
(B) 1/2 mol of H2
(C) 2/3 mol of O2
(D) Both 1/2 mol of H2 and 1/2 mol of O2
Q.14 If one mole
of ethanol (C2H5OH) completely burns to carbon
dioxide
and water, the weight of carbon dioxide formed is about -
and water, the weight of carbon dioxide formed is about -
(C2H5OH + 3O2 ® 2CO2 + 3H2O)
(A) 22g (B) 45g (C) 66g (D)
88g
Q.15 Calculate the weight of lime
(CaO) obtained by heating 200 kg
of 95% pure lime stone (CaCO3).
of 95% pure lime stone (CaCO3).
(A) 104.4 kg (B)
105.4 kg
(C) 212.8 kg (D)
106.4 kg
Q.16 The mass of 70% H2SO4 required for
neutralisation of 1 mol of NaOH
(A) 49 gm (B)
98 gm
(C) 70 gm (D)
34.3 gm
Q.17 12 litre of H2 and 11.2 litre of Cl2 are mixed and exploded.
The composition by volume of mixture is -
The composition by volume of mixture is -
(A) 24 litre of HCl
(B) 0.8 litre Cl2 and 20.8 lit HCl.
(C) 0.8 litre H2 & 22.4
litre HCl
(D) 22.4 litre HCl
Q.18 What
volume of 0.4-M FeCl3.6H2O will contain 600 mg of Fe3+ ?
(A) 49.85 mL (B)
26.78 mL
(C) 147.55 mL (D)
87.65 mL
Q.19 The mole
fraction of a given sample of I2 in C6H6 is 0.2.
The molality of I2 in C6H6 is -
The molality of I2 in C6H6 is -
(A) 0.32 (B)
3.2
(C) 0.032 (D)
0.48
Q.20 1 mol of N2 and 4 mol of H2 are allowed to react in a
vessel and after
reaction, H2O is added. Aqueous solution required 1 mol of HCl. Mol fraction
of H2 in the remaining gaseous mixture after reaction is -
reaction, H2O is added. Aqueous solution required 1 mol of HCl. Mol fraction
of H2 in the remaining gaseous mixture after reaction is -
(A) 1/6 (B) 5/6
(C) 1/3 (D)
None of these
Q.21 Calculate the
weight of BaCl2 needed to
prepare 250 mL of a solution
having the same concentration of Cl– ions as in a solution of
KCl of concentration 80 g/L. (Ba = 137.4, Cl = 35.5) -
having the same concentration of Cl– ions as in a solution of
KCl of concentration 80 g/L. (Ba = 137.4, Cl = 35.5) -
(A) 27.92 g (B)
14.50 g
(C) 22.52 g (D)
11.46 g
Q.22 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 -
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
Q.23 A sample of H2SO4 (density 1.8
g/ml) is 90% by weight.
What is the volume of the acid that has to be used to make 1 litre of 0.2-M H2SO4?
What is the volume of the acid that has to be used to make 1 litre of 0.2-M H2SO4?
(A) 16 mL (B)
10 mL
(C) 12 mL (D)
18 mL
Q.24 A sample of
Na2CO3. H2O
weighing 1.24 g is added to 200 mL of a
0.1-N H2SO4 solution. The resulting solution becomes -
0.1-N H2SO4 solution. The resulting solution becomes -
(A) acidic (B)
strongly acidic
(C) alkaline (D)
neutral
Q.25 125 mL of 10%
NaOH (w/V) is added to 125 mL of 10% HCl (w/V).
The resultant solution becomes-
The resultant solution becomes-
(A) alkaline (B)
strongly alkaline
(C) acidic (D)
neutral
Q.26 Equal volumes
of 0.50 M of HCl, 0.25 M of NaOH and 0.75 M of NaCl
are mixed. The molarity of the NaCl solution is -
are mixed. The molarity of the NaCl solution is -
(A) 0.75 M (B)
1/3 M
(C) 0.50 M (D)
2.00 M
Q.27 How many
grams of copper will be replaced in 2 L of a 1.50-M CuSO4
solution if the latter is made to react with 27.0 g of aluminium ?
(Cu = 63.5, Al =27.0)
solution if the latter is made to react with 27.0 g of aluminium ?
(Cu = 63.5, Al =27.0)
(3CuSO4 + 2Al ® Al2(SO4)3 + 3Cu)
(A) 190 g (B)
95.25 g
(C) 48 g (D)
10 g
Q.28 The ratio of the molar amounts
of H2S needed to precipitate the metal
ions from 20 ml each of 1M Cd(NO3)2 and 0.5 M CuSO4 is-
ions from 20 ml each of 1M Cd(NO3)2 and 0.5 M CuSO4 is-
(Cd(NO3)2 + H2S ® CdS¯ + 2HNO3)
(A) 1 : 1 (B)
2 : 1
(C) 1 : 2 (D)
Indefinite
Q.29 In
which mode of expression, the concentration of a solution remains
independent of temperature -
independent of temperature -
(A)
Molarity (B) % w/V
(C)
Formality (D) Molality
Q.30 The largest
number of molecules is in -
(B.H.U. 1997)
(A) 36 g of
water (B) 28 g of CO2
(C) 46 g of CH3OH (D) 58 g of N2O5
Q.31 Which has the
highest weight?(A.F.M.C. 1997)
(A) 1 m3 water
(B) 10 litre of Hg
(density of Hg = 13.6 gm/mL)
(C) A normal adult man
(D) All have same weight
Q.32 The number
of atoms of Cr and O are 4.8 × 1010 and 9.6 × 1010 respectively.
Its empirical formula is - (CPMT 1997)
Its empirical formula is - (CPMT 1997)
(A) Cr2O3 (B) CrO2
(C) Cr2O4 (D) None of these
Q.33 Volume of a
gas at NTP is 1.12 × 10–7 c.c.
The number of molecules in it will be -
The number of molecules in it will be -
(B.H.U.
1997)
(A) 3.1 × 1020 (B) 3.01 × 1012
(C) 30.1 × 1023 (D) 3.01 × 1024
Q.34 Haemoglobin
contains 0.33% of iron by weight. The molecular weight
of haemoglobin is approximately 67200. The number of iron atoms
(at wt. of Fe = 56) present in one molecule of haemoglobin are -
of haemoglobin is approximately 67200. The number of iron atoms
(at wt. of Fe = 56) present in one molecule of haemoglobin are -
(A) 1 (B) 2 (C)
4 (D) 6
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