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
Van der Waals parameter 'a' signifies -
1.The magnitude of intermolecular attractive forces.
2. The magnitude of intermolecular repulsive forces.
3. The volume of a gas molecule.
4. All of the above.
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
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
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
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
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 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 -
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
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