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

(I) $4N{H}_3\left(g\right) + 5O_2\left(g\right)\to 4NO\left(g\right) + 6H_{2}O\left(g\right)$
(II) $2NO\left(g\right) + O_2\left(g\right)\to 2N{O}_2\left(g\right)$
(III) $3N{O}_2\left(g\right) + H_{2}O\left(l\right) \to 2HN{O}_3\left(aq\right) + NO\left(g\right)$

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

A gaseous mixture of ${\mathrm{H}}_2$ and ${\mathrm{CO}}_2$ gas contains 66 mass % of ${\mathrm{CO}}_2$. The vapour density of the mixture is:

1.  6.1

2.  5.4

3.  2.7

4.  10.8

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)?

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 %

A mixture of ${\mathrm{O}}_2$ and gas "Y" (mol. wt. 80) in the mole ratio a : b has a mean molecular weight of 40. What would be the mean molecular weight, if the gases are mixed in the ratio b : a under identical conditions? (assume that these gases do not react)

 If 2.74 g of the metal oxide contains 1.53 g of metal, then the empirical formula of vanadium oxide is:

(Atomic Mass of V = 52)

1. ${\mathrm{V}}_2{\mathrm{O}}_3$

2. $\mathrm{VO}$

3. ${\mathrm{V}}_2{\mathrm{O}}_5$

4. ${\mathrm{V}}_2{\mathrm{O}}_7$

A gaseous mixture of propane and butane of volume 3 litre on complete combustion produces 11.0 litre $C{O}_2$ under standard conditions of temperature and pressure. The ratio of volume of butane to propane is:

1. 1 : 2

2. 2 : 1

3. 3 : 2

4. 3 : 1

The percentage by volume of $C_3{H}_8$ in a gaseous mixture of $C_3{H}_8$, $C{H}_4$ and CO is 20. When 100 mL of the mixture is burnt in excess of $O_2$, the volume of $C{O}_2$ produced is:

1. 90 mL

2. 160 mL

3. 140 mL

4. None of the above

The percentage of oxygen present in the compound ${\mathrm{CaCO}}_3.3{\mathrm{Ca}}_3 {\left({\mathrm{PO}}_4\right)}_2$ is-

1.  23.3%

2.  45.36%

3.  41.94%

4.  17.08%

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.  ${\mathrm{C}}_4{\mathrm{H}}_{10}$