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

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

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

A silver coin weighing 11.34 g was dissolved in nitric acid. When sodium chloride was added to the solution all the silver (present as $AgN{O}_3$) was precipitated as silver chloride. The weight of the precipitated silver chloride was 14.35 g. Calculate the percentage of silver in the coin.

1. 4.8%

2. 95.2%

3. 90%

4. 80%

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

It is known that an atom contains protons, neutrons, and electrons. If the mass of the neutron is assumed to be half of its original value, and that of the proton is assumed to be twice its original value, then the atomic mass of ${}_6{}^{14}\mathrm{C}$ will:

Nitric acid can be produced ${\mathrm{NH}}_3$ in three steps process:

(I) $4N{H}_3\left(g\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>5O_2\left(g\right)\to 4NO\left(g\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>6H_{2}O\left(g\right)$
(II) $2NO\left(g\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>O_2\left(g\right)\to 2N{O}_2\left(g\right)$
(III) $3N{O}_2\left(g\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>H_{2}O\left(l\right)<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>2HN{O}_3\left(aq\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>NO\left(g\right)$

percent yield Ist, IInd and IIIrd are respectively 50%, 60% and 80% respectively then what volume of $N{H}_3\left(g\right)$ at 1 atm and 0$°$C required to produces 1575 g of $HN{O}_3$

1. 156.25

2. 350 L

3. 3500 L

4. None of these

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?