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 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 -

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

The total pressure of a mixture that contains 8 g of O₂ and 4 g of H₂ confined in a vessel of 1 dm³ at 27^°C would be -

(R = 0.083 bar dm³ K^-1mol^-1)

1. 45.67 bar

2. 56.02 bar

3. 34.67 bar

4. 67.13 bar  

Find the mass of payload of a balloon of radius 10 m, if a mass of 100 kg is filled with helium at 1.66 bar and 27°C temperature.

(Density of air = 1.2 kg m^–3 and R = 0.083 bar dm³ K^–1 mol^–1).

1. 2905 Kg

2. 3811 Kg 

3. 2721 Kg

4. 4201 Kg                                                                                                                

2.9 g of a gas at 95^°C occupies the same volume as 0.184 g of dihydrogen at 17^°C, at the same pressure. The molar mass of the gas is -

1. 20 g mol^-1

2. 40 g mol^-1

3. 34 g mol^-1

4. 14 g mol^-1

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. The partial pressure of dihydrogen is -

1. 0.2 bar

2. 0.7 bar

3. 0.8 bar

4. 0.6 bar

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 -

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

The temperature of 4.0 mole of a gas occupying 5 dm³ at 3.32 bar is -
(R = 0.083 bar dm³ K^–1 mol^–1).

1. 40 K 

2. 30 K 

3. 20 K

4. 50 K 

The volume occupied by 8.8 g of CO₂ at 31.1°C and 1 bar pressure is:

(R = 0.083 bar L K^–1 mol^–1)

1. 4.05 L 

2. 3.05 L 

3. 6.05 L 

4. 5.05 L 

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