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1.

At STP, the density of CCl₄ vapour in g/L will be closest to: 
1. 8.67
2. 6.87
3. 3.67
4. 4.26

2.

The molarity of a H₂SO₄ solution that has a density 1.84 g/cc at $35°\mathrm{C}$ and contains 98% H₂SO₄ by weight is:
1. 1.84 M
2. 81.4 M
3. 18.4 M
4. 184 M

3. 6.02 × 10²⁰ molecules of urea are present in 100 mL of its solution. The concentration of the solution is:
1. 0.01 M
2. 0.001 M
3. 0.1 M
4. 0.02 M

4.

25.3 g of Sodium carbonate Na₂CO₃ is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ion, Na⁺ and carbonate ion ${\mathrm{CO}}_3^{2-}$ are respectively (Molar mass of Na₂CO₃ = 106 g mol^-1)
1. 0.955 M and 1.910 M
2. 1.910 M and 0.955 M
3. 1.90 M and 1.910 M
4. 0.477 M and 0.477 M

5.

The molality of a 20% (by mass) CaCO₃ solution is : 
(Given: Density of solution is 1.2 gm/ml)

1.	1.25 m	2.	2.5 m
3.	2.08 m	4.	1.5 m

6.

Equal volumes of 0.1 M AgNO₃ and 0.2 M NaCl are mixed. The concentration of N${\mathrm{O}}_3^{-}$ ions in the mixture will be:

1.	0.1M	2.	0.05M
3.	0.2M	4.	0.15M

7.

1cc N₂O at STP contains: 

1.	\({1.32 \over 224} \times10^{23}~\text{electrons}\)	2.	\({6.02 \over 22400} \times10^{23}~\text{molecules}\)
3.	\({1.8 \over 224} \times10^{22}~\text{atoms}\)	4.	All of the above

8.

The haemoglobin from the red blood corpuscles contains approximately 0.33%  iron
by mass. The molar mass of haemoglobin is 67,200. The number of iron atoms in each molecule of haemoglobin is :
(atomic mass of iron=56):

1.	2
2.	3
3.	4
4.	5

9.

What is the number of moles of O-atom in 126 amu of ${\mathrm{HNO}}_3$?
1.  2
2.  $\frac{2}{{\mathrm{N}}_{\mathrm{A}}}$
3.  6
4.  $\frac{6}{{\mathrm{N}}_{\mathrm{A}}}$

10.

The formula of an acid is ${\mathrm{HXO}}_2.$ The mass of 0.0242 moles of the acid is 1.657 g.
The atomic weight of X is:

1.	35.5	2.	28.1
3.	128	4.	19.0

11.

Volume occupied by one molecule of water (density = 1g cm^-3) is:
1. 9.0 x 10^-23 cm³
2. 6.023 x 10^-23 cm³
3. 3.0 x10^-23 cm³
4. 5.5 x10^-23 cm³

12.

The number of atoms in 0.1 mole of a triatomic gas is: 
(N_A=6.02 x10²³mol^-1)

1.	6.026 x 1022	2.	1.806x1023
3.	3.600 x 1023	4.	1.800 x 1022

13.

4.4 g of an unknown gas occupies 2.24 litres of volume at NTP. The gas may be: 

1.	Carbon dioxide	2.	Carbon monoxide
3.	Oxygen	4.	Sulphur dioxide

14.

Oxygen contains 90% O¹⁶ and 10% O¹⁸. Its atomic mass is
(1) 17.4
(2) 16.2
(3) 16.5
(4) 17