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1.

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. \(\mathrm{PH}_3, \mathrm{P}_2 \mathrm{O}_3, \mathrm{P}_2 \mathrm{O}_5\)

2.

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

3.

A 6.85 g sample of the hydrates $\mathrm{Sr}{\left(\mathrm{OH}\right)}_2.{\mathrm{xH}}_2\mathrm{O}$ is dried in an oven to give 3.13 g of anhydrous $\mathrm{Sr}{\left(\mathrm{OH}\right)}_2$. The value of x is - 
(Atomic weights : Sr=87.60, O=16.0, H=1.0)
1.  8
2.  12
3.  10
4.  6

4.

A solution of Na₂S₂O₃ is standardized iodometrically against 0.167 g of KBrO₃. This process requires 50 mL of the ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ solution. What is the normality of the  Na₂S₂O₃?
1. 0.2 N
2. 0.12 N
3. 0.72 N
4. 0.02 N

5.

The ${\mathrm{NH}}_3$ evolved due to complete conversion of N from 1.12 g sample of protein was absorbed in 45 mL of 0.4 N ${\mathrm{HNO}}_3$. The excess acid required 20 mL of 0.1 N $\mathrm{NaOH}$. The % N in the sample is:
1.  8
2.  16
3.  20
4.  25

6.

Rearrange the following (I to IV) in the order of increasing masses:
(I)   0.5 mole of O₃
(II)  0.5 gm atom of oxygen
(III) 3.011$\times$10²³ molecules of O₂
(IV)  5.6 liter of CO₂ at STP

1.	II<IV<III<I	2.	II<I<IV<III
3.	IV<II<III<I	4.	I<II<III<IV

7.

The density of dry air containing only ${\mathrm{N}}_2$ and ${\mathrm{O}}_2$ is 1.15 g/L at 740 mm and 300 K. What is the percentage
composition of ${\mathrm{N}}_2$ by weight in the air?

1.	78.00%	2.	75.50%
3.	70.02%	4.	72.75%

8.

The vapour density of a mixture containing ${\mathrm{NO}}_2$ and ${\mathrm{N}}_2{\mathrm{O}}_4$ is 27.6. The mole fraction of ${\mathrm{N}}_2{\mathrm{O}}_4$ in the mixture is:
1.  0.1
2.  0.2
3.  0.5
4.  0.8

9.

How much volume of 75% alcohol by weight (d=0.80 g/cm³) is required to prepare 150 cm³ of 30% alcohol by weight (density = 0.90 g/cm³)?

1.	67.5 mL	2.	56.25 mL
3.	44.44 mL	4.	None of the above

10.

The average atomic mass of magnesium is 24.31 a.m.u. Magnesium consists of three isotopes: \(^{24}Mg\), \(^{25}Mg \), and \(^{26}Mg\). The mole percentage of \(^{24}Mg\) is 79%, and the remaining 21% is a mixture of \(^{25}Mg \) and \(^{26}Mg\).
Calculate the mole percentage of \(^{26}Mg\).
1.  10 %
2.  11 %
3.  15 %
4.  16 %

11.

Calculate the % of free ${\mathrm{SO}}_3$ in oleum (a solution of ${\mathrm{SO}}_3$ in ${\mathrm{H}}_2{\mathrm{SO}}_4$) that is labelled 109% ${\mathrm{H}}_2{\mathrm{SO}}_4$.
1. 40
2. 30
3. 50
4. None
 

12.

Suppose two elements X and Y combine to form two compounds ${\mathrm{XY}}_2$ and ${\mathrm{X}}_2{\mathrm{Y}}_3$when 0.05 mole of${\mathrm{XY}}_2$ weighs 5 g while 3.011$\times$10²³ molecules of ${\mathrm{X}}_2{\mathrm{Y}}_3$ weighs 85 g. The atomic masses of x and y are respectively:
1.  20, 30
2.  30, 40
3.  40, 30
4.  80, 60

13.

100 mL of 10% NaOH (w/V) is added to 100 mL of 10% HCl (w/V). The resultant solution becomes:
1. Alkaline
2. Strongly alkaline
3. Acidic
4. Neutral

14.

1.44 gram of titanium (At. wt. =48) reacted with excess of ${\mathrm{O}}_2$ and produce x gram of non-stoichiometric compound Ti_1.44 O$$. The value of x is:
1. 2
2. 1.77
3. 1.44
4. None of the above

15. For the reaction

2Fe(NO₃)₃ + 3Na₂CO₃ → Fe₂(CO₃)₃ + 6NaNO₃

2.5 moles of Fe(NO₃)₃ are allowed to react with 3.6 moles of Na₂CO₃. If the actual amount of NaNO₃ produced is 6.3 moles, calculate the percentage yield of the reaction.
1. 50
2. 84
3. 87.5
4. 100

16.

A 6.0 g impure sample of sodium chloride is dissolved in water and reacted with excess silver nitrate solution.
If 14.0 g of silver chloride is formed, determine the percentage purity of NaCl in the sample.
1. 95%
2. 85%
3. 75%
4. 65%

17.

25.4 g of ${\mathrm{I}}_2$ and 14.2 g  of ${\mathrm{Cl}}_2$ are made to react completely to yield a mixture of ICI and ICI₃. The mole of ICI and ICI₃ formed, is respectively -
1. 0.5, 0.2
2. 0.1, 0.1
3. 0.1, 0.3
4. 0.3, 0.4

18.

The vapour density of a mixture containing \(NO_{2}\) and \(N_{2} O_{4}\)  is 38.3. The mole of \(NO_{2}\) in a 100 g mixture is:
[Vapour density = (Molar mass / 2)]
1. 0.437
2. 0.347
3. 0.557
4. 0.663

19.

The average molar mass of the mixture of ${\mathrm{CH}}_4$ $$and ${\mathrm{C}}_2{\mathrm{H}}_4$ present in the mole ratio of a:b is
20 g mol^-1. When the mole ratio is reversed, the molar mass of the mixture will be:

1.	24 gram	2.	42 gram
3.	20 gram	4.	15 gram

20. 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

21.

The vapour density of a volatile chloride of a metal is 95 and the specific heat of the metal is 0.13 cal/g. The equivalent mass of the metal will be:
1.  6 g
2. 12 g
3.  18 g
4.  24 g