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

 A = $\frac{{\mathrm{pV}}^2{\mathrm{T}}^2}{\mathrm{n}}$ 

The SI unit for the quantity A is -

1. $\mathrm{N} {\mathrm{m}}^2 {\mathrm{K}}^2 {\mathrm{mol}}^{-1}$

2. $\mathrm{N} {\mathrm{m}}^4 \mathrm{K} {\mathrm{mol}}^{-1}$

3. $\mathrm{N} {\mathrm{m}}^2 {\mathrm{K}}^3 {\mathrm{mol}}^{-1}$ 

4. $\mathrm{N} {\mathrm{m}}^4 {\mathrm{K}}^2{\mathrm{mol}}^{-1}$

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 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

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

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