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

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:

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

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

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

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

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 % composition of ${\mathrm{N}}_2$ by weight in the air?
1.  78%
2.  75.5%
3.  70.02%
4.  72.75%

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

What volume of 75% alcohol by weight (d=0.80g/$c{m}^3$) must be used to prepare 150 $c{m}^3$ of 30% alcohol by weight (d=0.90 g/$c{m}^3$)?
1. 67.5 mL
2. 56.25 mL
3. 44.44 mL
4. None of these

Average atomic mass of magnesium is 24.31 a.m.u. This magnesium is compound of 79 mole% of ${}_{24}\mathrm{Mg}$ and remaining 21 mole % of ${}_{25}\mathrm{Mg}$ and ${}_{26}\mathrm{Mg}$. Calculate mole% of ${}_{26}\mathrm{Mg}$.
1.  10
2.  11
3.  15
4.  16

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
 

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

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

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

For the reaction; 
\(2Fe{(NO_3)}_3 + 3Na_2CO_3 \rightarrow Fe_2{(CO3)}_3 + 6NaNO_3\)
Initially if 2.5 mole of \(Fe{(NO_3)}_3 \) and 3.6 mole of \(Na_2CO_3\) is taken. If 6.3 mole of \(NaNO_3\) is obtained then % yield of given reaction is:
1.  50
2.  84
3.  87.5
4.  100

The impure 6 g of $\mathrm{NaCl}$ is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of $\mathrm{NaCl}$ solution would be:
1.  95%
2.  85%
3.  75%
4.  65%

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

The vapour density of a mixture containing ${\mathrm{NO}}_2$ and ${\mathrm{N}}_2{\mathrm{O}}_4$  is 38.3. The mole of ${\mathrm{NO}}_2$ in a 100 g mixture is -
[Vapour density = (Molar mass / 2)]
1. 0.437
2. 0.347
3. 0.557
4. 0.663

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:

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):

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