The correct relation between density () and pressure of gas (P) is-
1.
2.
3.
4. None of the above
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
As per Charles's law ,–273° C is the lowest possible temperature because:
1. | All gases get liquefied before reaching a temperature of – 273° C. |
2. | All gases get liquefied after reaching a temperature of – 273° C. |
3. | All gases have a critical temperature of –273° C. |
4. | None of the Above. |
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 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
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 -
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 -
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.
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
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