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1.

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

2.

Which of the following combinations illustrates the law of reciprocal proportions?
1. \(\mathrm{N}_2 \mathrm{O}_3, \mathrm{~N}_2 \mathrm{O}_4, \mathrm{~N}_2 \mathrm{O}_5 \)
2. \(\mathrm{NaCl}, \mathrm{NaBr}, \mathrm{Nal}\)
3. \(\mathrm{CS}_2, \mathrm{CO}_2, \mathrm{SO}_2 \)
4. \(\mathrm{PH}_3, \mathrm{P}_2 \mathrm{O}_3, \mathrm{P}_2 \mathrm{O}_5\)

3.

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

4.

Calculate the mole fraction of the solute in a 1.00 m aqueous solution.

1.	0.177	2.	0.771
3.	0.0534	4.	0.0177

5. The number of water molecules are maximum in:
1. 18 molecules of water
2. 1.8 g of water
3. 18 g of water
4. 18 moles of water

6.

Concentrated aqueous sulphuric acid is 98% H₂SO₄ by mass and has a density of 1.80 g mL^-1.
The volume of acid required to make one litre of 0.1 M H₂SO₄ solution is:

1.	11.10 mL	2.	16.65 mL
3.	22.20 mL	4.	5.55 mL

7.

A gaseous mixture of ${\mathrm{H}}_2$ and ${\mathrm{CO}}_2$ gas contains 66 mass % of ${\mathrm{CO}}_2$. The vapour density of the mixture is:
1.  6.1
2.  5.4
3.  2.7
4.  10.8

8.

The percentage of oxygen present in the compound ${\mathrm{CaCO}}_3.3{\mathrm{Ca}}_3<mspace\; width="1em"></mspace>{\left({\mathrm{PO}}_4\right)}_2$ is-
1.  23.3%
2.  45.36%
3.  41.94%
4.  17.08%

9. The iron content of haemoglobin is 0.33% by mass. Given that the molar mass of haemoglobin is 67,200 g mol⁻¹, determine the number of iron atoms present in each haemoglobin molecule.
(Atomic mass of Fe = 56)

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

10.

Which mixture is lighter than humid air?
1.  ${\mathrm{N}}_2+{\mathrm{O}}_2+{\mathrm{SO}}_2$
2.  ${\mathrm{N}}_2+{\mathrm{O}}_2+{\mathrm{CO}}_2$
3.  ${\mathrm{N}}_2+{\mathrm{O}}_2+{\mathrm{C}}_2{\mathrm{H}}_6$
4.  ${\mathrm{N}}_2+{\mathrm{O}}_2+\mathrm{He}$

11.

At 100 ºC and 1 atm, if the density of liquid water is 1.0 g cm^–3 and that of water vapor is 0.0006 g cm^-3, then the volume occupied by water molecules in 1 litre of steam at that temperature will be:

1.	6 cm3	2.	60 cm3
3.	0.6 cm3	4.	0.06 cm3

12.

 The maximum number of molecules is present in which of the following? 
1. 15 L of $H_2$ gas at STP
2. 5 L of $N_2$ gas at STP
3. 0.5 g of $H_2$ gas
4. 10 g of $O_2$ gas

13.

The number of  moles  present in 2.5 litres of 0.2 M  ${\mathrm{H}}_2{\mathrm{SO}}_4$ are:
1. 0.25
2. 0.5
3. 0.75
4. 0.2

14.

The weight of one molecule of a compound C₆₀H₁₂₂ is
1. $5.005\times {10}^{23<mspace\; width="1em"></mspace>}\mathrm{g}$
2. $6.023\times {10}^{23}<mspace\; width="1em"></mspace>\mathrm{g}$
3. $4.1\times {10}^{-21}<mspace\; width="1em"></mspace>\mathrm{g}$
4. $1.4\times {10}^{-21}\mathrm{g}$
 

15.

Determine the mass percentage of urea in a solution prepared by mixing equal moles of urea and water.
 
1. 22.086
2. 11.536
3. 46.146
4. 76.92

16.

The number of valence electrons present in 0.53 grams of Na₂CO₃ is:
1. $3.01\times {10}^{23}$
2. $7.22\times {10}^{22}$
3. $12.046\times {10}^{23}$
4. $6.023\times {10}^{23}$

17.

The molality of 0.01 M Na₂CO₃ solution is:
(The density of the solution is 1.1 g/ml)
1. $9\times {10}^{-3}$
2. $1.8\times {10}^{-3}$
3. $4.5\times {10}^{-3}$
4. $1.1\times {10}^{-3}$

18.

lf N_A is Avogadro's number, then the number of valence electrons in 4.2 g of nitride ions (N${}^{3-}$) will be:

1.	3.2 NA	2.	1.6 NA
3.	2.4 NA	4.	1.2 NA

19.

What is the molarity of ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution that has a density of 1.84 g/cc at 35°C and contains 98% ${\mathrm{H}}_2{\mathrm{SO}}_4$ by weight? 
1. 1.84 M 
2. 81.4 M 
3. 18.4 M
4. 184 M

20.

Calculate the number of moles of oxygen (O) atoms in 126 amu of HNO₃. 
1.  2
2.  $\frac{2}{{\mathrm{N}}_{\mathrm{A}}}$
3.  6
4.  $\frac{6}{{\mathrm{N}}_{\mathrm{A}}}$