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Which of The following has a maximum number of molecules?
1. 7g N₂ 
2. 2g H₂ 
3. 16g NO₂ 
4. 16g O₂ 

How much oxygen gas (O₂) at standard temperature (0°C) and pressure (1 atm) is required to completely combust 1 liter of propane gas (C₃H₈) under the same conditions?

The product of atomic mass and specific heat of metal is approximately 6.4. This was given by:
1. Dalton's law
2. Avogadro's law
3. Newton's law
4. Dulong Petit's law

A gas is found to have the formula (CO)_x. Its VD is 70. The value of x must be:
1. 7 
2. 4
3. 5
4. 6

2 gm Iron pyrite (FeS₂) is burnt with O₂ to form Fe₂O₃ and SO₂. The mass of SO₂ produced is (Fe=56, S=32, O=16)
1. 2 gm
2. 2.13 gm
3. 4 gm
4. 4.26 gm

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

KClO₃ on heating decomposes to KCl and O₂. The volume of O₂ at STP liberated by 0.1 mole KClO₃ is
1. 4.36 L
2. 3.36 L
3. 2.36 L
4. None of these

At S.T.P. the density of CCl₄ vapour in g/L will be nearest to [CBSE PMT 1988]
(1) 6.84
(2) 3.42
(3) 10.26
(4) 4.57

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

The mass of carbon present in 0.5 mole of K₄[Fe(CN)₆] is:
1. 1.8 g
2. 18 g
3.  3.6 g
4.  36 g

The number of moles of oxygen in one litre of air containing 21% oxygen by volume under standard conditions is [CBSE PMT 1995]
(1) 0.186 mole
(2) 0.21 mole
(3) 0.0093 mole
(4) 2.10 mole

The empirical formula of an organic compound containing carbon and hydrogen is CH₂. The mass of one litre of this organic gas at STP  is exactly equal to that of one litre of N₂ at STP. Therefore, the molecular formula of the organic gas is:
1. C₂H₄
2. C₃H₆
3. C₆H₁₂
4. C₄H₈

An organic compound containing C, H, and N gave the following on analysis: C = 40%, H = 13.3% and N = 46.67%. Its empirical formula would be:
1. CHN
2. C₂H₂N
3. CH₄N
4. C₂H₇N

At standard temperature and pressure (STP), the volume of oxygen required to completely combust 30 ml of acetylene under similar conditions is:
1. 100 ml
2. 75 ml
3. 50 ml
4. 25 ml

If the Avogadro number N_A, is changed from 6.022 x 10²³ mol^-1 to 6.022 x 10²⁰ mol^-1 this would change: 
1. The definition of mass in units of grams.
2. The mass of one mole of carbon.
3. The ratio of chemical species to each other in a balanced equation.
4. The ratio of elements to each other in a compound.

6.02 x 10²⁰ molecules of urea are present in 100 mL of its solution. The concentration of the solution is: 

The maximum amount of BaSO₄ precipitated on mixing 20mL of 0.5 M BaCl₂ with 20 mL of 1 M H₂SO₄ is:
1. 0.25 mole
2. 0.5 mole
3. 1 mole 
4. 0.01 mole

Insulin contains 3.4% sulphur: The minimum molar mass of insulin is:
1. 941 g
2. 1000 g
3. 841 g
4. 1041 g

1.60 g of a metal were dessolved in HNO₃ to prepare its nitrate. The nitrate on strong heating gives 2 g oxide. The equvalent mass of metal is:
1. 16
2. 32
3. 48
4. 12

100 ml each of 0.5 N NaOH, N/5 HCl and N/10 H₂SO₄ are mixed together. The resulting solution will be 
1. Acidic
2. Alkaline
3. Neutral
4. Can't be determine

An element A (at. wt. = 75) and B (at. wt. = 25) combine to form a compound that contains 75% A by weight. The formula of the compound will be:

The ratio of number of atoms in 4.4 gm CO₂ and 1.7 gm NH₃ is
1. 1:1
2. 3:4
3. 4:3
4. 1:2

$2{\mathrm{SO}}_2<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{O}}_2<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>2{\mathrm{SO}}_3$, 6.4 gm SO₂ and 3.2 gm O₂ to form SO₃. How much maximum mass of SO₃ is formed?
1. 32 gm
2. 16 gm
3. 8 gm
4. 4 gm

A metallic nitride(M₃N₂) contains 20% nitrogen. Equivalent weight of metal is 
1. 37.33
2. 18.67
3. 112
4. 56

The weight of iron which will be converted into oxide (Fe₃O₄) by the action of 18 gm of steam of it will be (at. wt. of Fe = 56)
1. 168 gm
2. 84 gm
3. 42 gm
4. 21 gm

Calculate the molality of 20% CaCO₃ solution is (by mass). The density of solution is 1.2 gm/ml
1. 1.25 m
2. 2.5 m
3. 2.08 m
4. 1.5 m

A mixture of methane and ethene in the molar ratio of x : y has a mean molar mass of 20. What would be the mean molar mass. if the gases are mixed in the molar ratio of y : x?
(1) 22                               
(2) 24
(3) 20.8                           
(4) 19

The volume of a drop of water is 0.0018 mL then the number of water molecules present in two drop of water at room temperature is:
1.  $12.046\times {10}^{19}$
2.  $1.084\times {10}^{18}$
3.  $4.84\times {10}^{17}$
4.  $6.023\times {10}^{23}$

Carbon and oxygen form two oxides, carbon monoxide and carbon dioxide, where the weight ratios of carbon to oxygen are 12:16 and 12:32, respectively. These ratios demonstrate:
1. Law of multiple proportions
2. Law of reciprocal proportions
3. Law of conservation of mass
4. Law of constant proportions

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 sample of phosphorus that weights 12.4 g exerts a pressure 8 atm in a 0.821 litre closed vessel at 527$°$C. The molecular formula of the phosphorus vapour is:
1.  ${\mathrm{P}}_2$
2.  ${\mathrm{P}}_4$
3.  ${\mathrm{P}}_6$
4.  ${\mathrm{P}}_8$

Phosphoric acid $\left({\mathrm{H}}_3{\mathrm{PO}}_4\right)$ prepared in a two step process.
(1) ${\mathrm{P}}_4+5{\mathrm{O}}_2<mspace\; width="1em"></mspace>\stackrel{}{\to }<mspace\; width="1em"></mspace>{\mathrm{P}}_4{\mathrm{O}}_{10}$
(2) ${\mathrm{P}}_4{\mathrm{O}}_{10}+6{\mathrm{H}}_2\mathrm{O}<mspace\; width="1em"></mspace>\stackrel{}{\to }<mspace\; width="1em"></mspace>4{\mathrm{H}}_3{\mathrm{PO}}_4$
We allow 62g of phosphorus to react with react with excess oxygen which form ${\mathrm{P}}_4{\mathrm{O}}_{10}$ in 85% yield. In the step (2) reaction 90% yield of ${\mathrm{H}}_3{\mathrm{PO}}_4$ is obtained. Produced mass of ${\mathrm{H}}_3{\mathrm{PO}}_4$ is:
1.  37.485 g
2.  149.949 g
3.  125.47 g
4.  564.48 g

What volume of HCl solution of density 1.2 g/cm³ and containing 36.5% by weight HCl, must be allowed to react with zinc(Zn) in order to liberate 4.0 g of hydrogen?
1.  333.33 mL
2.  500 mL
3.  614.66 mL
4.  None of these

The molar mass of diacidic organic Lewis base (B), if 12 g of chloroplatinate salt $\left({\mathrm{BH}}_2{\mathrm{PtCl}}_6\right)$ on ignition produced 5 gm residue of Pt,will be -
1.  52
2.  58
3.  88
4.  None of these

What volume of ${\mathrm{O}}_2\left(\mathrm{g}\right)$ measured at 1 atm and 273 K will be formed by the action of 100 mL of 0.5 N KMnO₄ on hydrogen peroxide in an acid solution?
The skeleton equation for the reaction is
${\mathrm{KMnO}}_4+{\mathrm{H}}_2{\mathrm{SO}}_4+{\mathrm{H}}_2{\mathrm{O}}_2<mspace\; width="1em"></mspace>$$\to {\mathrm{K}}_2{\mathrm{SO}}_4+{\mathrm{MnSO}}_4+{\mathrm{O}}_2+{\mathrm{H}}_2\mathrm{O}$
1.  0.12 litre
2.  0.028 litre
3.  0.56 litre
4.  1.12 litre

Cisplatin, an anticancer drug, has the molecular formula $\mathrm{Pt}{\left({\mathrm{NH}}_3\right)}_2<mspace\; width="1em"></mspace>{\mathrm{Cl}}_2$. What is the mass (in gram) of one molecule? (Atomic weights : Pt=195, H=1.0, N=14, Cl=35.5)
1.  $4.98\times {10}^{-21}$
2.  $4.98\times {10}^{-22}$
3.  $6.55\times {10}^{-21}$
4.  $3.85\times {10}^{-22}$

The conversion of oxygen to ozone occurs to the extent of 15% only. The mass of ozone that can be prepared from 67.2 L oxygen at 1 atm and 273 K will be:
1. 14.4 gm
2. 96 gm
3. 640 gm
4. 64 gm

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 %

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

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%

60 mL of a mixture of nitrous oxide and nitric oxide was exploded with excess of hydrogen. If 38 mL of ${\mathrm{N}}_2$ was formed, calculate the volume of each gas in the mixture. All measurements are made at constant P and T.
1.20 ml +30 ml
2. 44 ml + 16 ml
3. 10 ml+40 ml
4 .25 ml +25 ml

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):

Volume strength of 1 M solution of ${\mathrm{H}}_2{\mathrm{O}}_2$ is:
1.  11.2         2.  22.4
3.  10.8         4.  21.6