The minimum pressure required to compress 500 dm³ of air at 1 bar to 200 dm³ at 30°C is :

1. 3.6 bar

2. 3.2 kbar

3. 2.5 bar

4. 2.8 kbar

The correct relation between density ($\mathrm{\rho }$) and pressure of gas (P) is-

1. $\mathrm{P}$ $\mathrm{\alpha }$ ${\mathrm{d}}^2$

2. $\mathrm{P}$ $\mathrm{\alpha }$ $\frac{1}{\mathrm{d}}$

3. $\mathrm{P}$ $\mathrm{\alpha }$ $\mathrm{d}$

4. None of the above

At 0^°C, the density of a certain oxide of a gas at 2 bar is the same as that of dinitrogen at 5 bar.

The molecular mass of the oxide would be -

1. 35 g/mol

2. 45 g/mol

3. 70 g/mol

4. 60 g/mol

The pressure of 1 gm of an ideal gas A at 27 °C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at the same temperature, the pressure becomes 3 bar.

The correct relationship between their molecular masses is -

1. M_A=M_B

2. 4M_A=M_B

3. M_A= 2M_B

4. 2M_A=M_B

The volume of H₂ that would be released when 0.15 g of aluminium reacts at 20 °C and 1 bar pressure with caustic soda is-

1. 225 L

2. 301 mL

3. 156 L

4. 203 mL

The pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm³ flask at 27 °C would be -

$1.$ $8.31$ $\times$ ${10}^4$ $\mathrm{Pa}$
$2.$ $7.43$ $\times$ ${10}^{-4}$ $\mathrm{Pa}$
$3.$ $6.87$ $\times$ ${10}^3$ $\mathrm{Pa}$
$4.$ $8.31$ $\times$ ${10}^6$ $\mathrm{Pa}$

0.5 L of H₂ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C.

The pressure inside the vessel would be -

1. 3.6 bar

2. 1.8 bar

3. 4.1 bar

4. 0.7 bar

The density of a gas is found to be 5.46 g/dm³ at 27^°C at 2 bar pressure. The density of gas at STP would be -

$1.<mspace\; width="1em"></mspace>2.0<mspace\; width="1em"></mspace>\mathrm{g}<mspace\; width="1em"></mspace>{\mathrm{dm}}^{-3}$
$2.<mspace\; width="1em"></mspace>3.0<mspace\; width="1em"></mspace>\mathrm{g}<mspace\; width="1em"></mspace>{\mathrm{dm}}^{-3}$
$3.<mspace\; width="1em"></mspace>4.5<mspace\; width="1em"></mspace>\mathrm{g}<mspace\; width="1em"></mspace>{\mathrm{dm}}^{-3}$
$4.<mspace\; width="1em"></mspace>1.5<mspace\; width="1em"></mspace>\mathrm{g}<mspace\; width="1em"></mspace>{\mathrm{dm}}^{-3}$

34.05 mL of phosphorus vapour weighs 0.0625 g at 546 °C and 0.1 bar pressure. The molar mass of phosphorus would be -

$1.$ $1247.5$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$2.$ $2234.7$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$3.$ $3126.9$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$4.$ $1134.6$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$

A student forgot to add the reaction mixture to the round-bottomed flask at 27 °C but instead, he placed the flask on the flame. After a lapse of time, he realized his mistake and using a pyrometer he found the temperature of the flask was 477 °C. The fraction of air that would  expel out would be :

1. 1/3

2. 4/5

3. 3/5

4. 2/3