The fraction of molecular volume to the actual volume occupied by oxygen gas at STP is: (Take the diameter of an oxygen molecule to be 3 Å).
1. 4 × 10⁻⁴
2. 5 × 10⁻⁴
3. 3 × 10⁻⁴
4. 1 × 10⁻⁴

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure is:
(STP: \(1\) atmospheric pressure, \(0~^\circ \text{C}\))
1. \(0\) 
2. \(22.4\) litres
3. \(11.2\) litres
4. \(1\) litres

The figure shows a plot of \(\frac{PV}{T}\) versus \(P\) for \(1.00\times10^{-3} \) kg of oxygen gas at two different temperatures.

Then relation between \(T_1\) and \(T_2\) is: 
1. \(T_1=T_2\)
2. \(T_1<T_2\)
3. \(T_1>T_2\)
4. \(T_1 \geq T_2\)$\mathrm{}$

The figure shows a plot of PV/T versus P for $1.00\times {10}^{-3} kg$ of oxygen gas at two different temperatures.

The value of PV/T where the curves meet on the y-axis is:

$1. 0.06 J K^{-1}$
$2. 0.36 J K^{-1}$
$3. 0.16 J K^{-1}$
$4. 0.26 J K^{-1}$

An oxygen cylinder of volume 30 litres has an initial gauge pressure of 15 atm and a temperature of 27 °C. After some oxygen is withdrawn from the cylinder, the gauge pressure drops to 11 atm, and its temperature drops to 17 °C. The mass of oxygen taken out of the cylinder is: $\left(\mathrm{R}=8.31 {\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}, \mathrm{molecular} \mathrm{mass} \mathrm{of} {\mathrm{O}}_2=32 \mathrm{u}\right)$

1. 0.14 kg
2. 0.16 kg
3. 0.18 kg
4. 0.21 kg

An air bubble of volume 1.0 $c{m}^3$ rises from the bottom of a lake 40 m deep at a temperature of 12 °C. To what volume does it grow when it reaches the surface, which is at a temperature of 35 °C?
1. 5.3 cm³
2. 4.0 cm³
3. 3.7 cm³
4. 4.9 cm³

What is the total number of air molecules (inclusive of oxygen, nitrogen, water vapor, and other constituents) in a room of capacity \(25.0\) m³ at a temperature of \(27^\circ \mathrm C\) and \(1\) atm pressure?