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If mass of one atom is $3.32\times {10}^{-23}$g, then calculate number of nucleons (neutrons and protons) present in 2 atoms of the element:
1.  40
2.  20
3.  10
4.  40 N_A

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.  $\frac{6}{{\mathrm{N}}_{\mathrm{A}}}$

What is the charge of 96 amu of S^2-?
1.  2C
2.  3.2$\times$10^-19C
3.  9.6$\times$10^-19C
4.  6C

The total no. of neutrons present in 54 mL ${\mathrm{H}}_2\mathrm{O}$ (l) are:
1.  $3 {\mathrm{N}}_{\mathrm{A}}$
2.  $30 {\mathrm{N}}_{\mathrm{A}}$
3.  $24 {\mathrm{N}}_{\mathrm{A}}$
4.  none of these

20 g of an ideal gas contains only atoms of S and O occupies 5.6 L at 1 atm and 273 K. What is the mol. wt. of gas?
1.  64
2.  80
3.  96
4.  None of these

Total number of moles of oxygen atoms in 3 litre ${\mathrm{O}}_3$(g) at 27$°$C and 8.21 atm are:
1.  3
2.  4
3.  1
4.  none of these

Rearrange the following (I to IV) in the order of increasing masses:
(I) 0.5 mole of ${\mathrm{O}}_3$
(II) 0.5 gm atom of oxygen
(III) 3.011$\times$10²³ molecules of ${\mathrm{O}}_2$
(IV) 5.6 litre of ${\mathrm{CO}}_2$ at STP
1.  II < IV < III < I
2.  II < I < IV < III
3.  IV < II < III < I
4.  I < II < III < IV

Common salt obtained from sea-water contains 8.775% NaCl by mass. The number of formula units of NaCl present in 25 g of this salt is:
1.  $3.367\times {10}^{23} \mathrm{formula} \mathrm{units}$
2.  $2.258\times {10}^{22} \mathrm{formula} \mathrm{units}$
3.  $3.176\times {10}^{23} \mathrm{formula} \mathrm{units}$
4.  $4.73\times {10}^{25} \mathrm{formula} \mathrm{units}$

Caffeine has a molecular weight of 194. If it contains 28.9% by mass of nitrogen, number of atoms of nitrogen in one molecule of caffeine is:
1.  4
2.  6
3.  2
4.  3

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. 80.5%
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

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

Hydrogen and oxygen combine to form  ${\mathrm{H}}_2{\mathrm{O}}_2$ and ${\mathrm{H}}_2\mathrm{O}$ containing 5.93% and 11.2% hydrogen, respectively. This data illustrates:
1.  Law  of conversation of mass
2.  Law of constant proportion
3.  Law  of reciprocal proportion
4.  Law of multiple proportions

One mole of elements X has 0.44 times the mass of one mole of element Y. One atom of elements X has 2.96 times the mass of one atom of $\raisebox{1ex}{$12$}\!\left/ \!\raisebox{-1ex}{$\mathrm{C}$}\right.$. What is the atomic weight of Y?
1.  80
2.  15.77
3.  46.67
4.  40.0

What is the empirical formula of vanadium oxide, if 2.74 g f the metal oxide contains 1.53 g of metal:
1.  ${\mathrm{V}}_2{\mathrm{O}}_3$
2.  VO
3.  ${\mathrm{V}}_2{\mathrm{O}}_5$
4.  ${\mathrm{V}}_2{\mathrm{O}}_7$

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

A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound:
1.  ${\mathrm{C}}_2{\mathrm{H}}_2$
2.  ${\mathrm{C}}_2{\mathrm{H}}_4$
3.  ${\mathrm{C}}_4{\mathrm{H}}_8$
4.  ${\mathrm{C}}_4{\mathrm{H}}_{10}$

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

Nitric acid can be produced ${\mathrm{NH}}_3$ in three steps process
(I) $4{\mathrm{NH}}_3\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right) \stackrel{}{\to } 4\mathrm{NO}\left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$
(II) $2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right) \stackrel{}{\to } 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$
(III) $3{\mathrm{NO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) \stackrel{}{\to } 2{\mathrm{HNO}}_3\left(\mathrm{aq}\right)+\mathrm{NO}\left(\mathrm{g}\right)$
percent yield of I^st, II^nd and III^rd are respectiveky 50%, 60% and 80% respectively then what volume of ${\mathrm{NH}}_3\left(\mathrm{g}\right)$ at 1 atm and $0°\mathrm{C}$ required to produced 1575 g of ${\mathrm{HNO}}_3$.
1.  156.25
2.  350 L
3.  3500 L
4.  None of these

M NaOH solution was slowly added into 1000 mL of 183.75 g impure ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution and the following plot was obtained. The percentage purity of ${\mathrm{H}}_2{\mathrm{SO}}_4$ sample and slope of the curve respectively are:
                                     
1.  $75\%, -\frac{1}{3}$
2.  $80\%, -\frac{1}{2}$
3.  $80\%, -1$
4.  None of these

A metal M forms the sulphate ${\mathrm{M}}_2{\left({\mathrm{SO}}_4\right)}_3$. A 0.596 gram sample of the sulphate reacts with excess ${\mathrm{BaCl}}_2$ to give 1.220 g ${\mathrm{BaSO}}_4$. What is the atomic weight of M?     (Atomic weights : S=32, Ba=137.3)
1.  26.9
2.  69.7
3.  55.8
4.  23

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 of oxygen at 1 atm and 273 K will be:
1.  14.4 gm
2.  96 gm
3.  640 gm
4.  64 gm