What will be the minimum pressure required to compress 500 dm³ of air at 1 bar to 200 dm³ at 30^°C?

1. 5.0 bar

2. 2.5 bar

3. 2.7 bar

4. 3.0 bar

A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35 °C. What would be its pressure?

1. 0.8 bar

2. 1.8 bar

3. 2.6 bar

4. 3.5 bar

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                                                                                                                

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