Two flasks of equal volume are connected by a narrow tube (of negligible volume) at 27ºC and contain 0.70 mole of at 0.5 atm. One of the flasks is then immersed in a hot bath, kept at 127 ºC, while the other remains at 27 ºC. The final pressure is -
1. 5.714 atm
2. 0.5714 atm
3. 2.5214 atm
4. 5.5114 atm
Flask X is filled with 20 g of gas at 100 °C and another identical flask Y with 40 g gas at the same temperature. The correct statement among the following is –
1. The pressure of the gases in the two flasks is identical
2. The pressure of in flask X is higher than that of in flask Y
3. The pressure of in flask X is lower than that of in flask Y
4. The pressure of in flask X is half that of in flask Y
Maximum deviation from ideal gas is shown by-
1. H2(g)
2. N2(g)
3. CH4(g)
4. NH3(g)
A gaseous mixture contains 56 g of N2, 44 g of CO2 and 16 g of CH4. The total pressure of the mixture is 720 mm Hg. The partial pressure of CH4 is-
1. 180 mm
2. 360 mm
3. 540 mm
4. 720 mm
In a flask of volume V litres, 0.2 mol of oxygen, 0.4 mol of nitrogen, 0.1 mol of ammonia and 0.3 mol of helium are enclosed at . If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is-
1. 1 atm
2. 0.1 atm
3. 0.2 atm
4. 0.4 atm
The density of methane at 2.0 atmosphere pressure and 27°C is-
1. 0.13 gL–1
2. 0.26 gL–1
3. 1.30 gL–1
4. 2.60 gL–1
3.2 g of oxygen and 0.2 g of hydrogen are placed in a 1.12 litre flask at 0°C.
The total pressure of the gas mixture will be-
1. 1 atm
2. 4 atm
3. 3 atm
4. 2 atm
120 g of an ideal gas of molecular weight 40 g mole–1 are confined to a volume of 20 L at 400 K. The pressure of the gas is-
( )
1. 3.90 atm
2. 4.92 atm
3. 6.02 atm
4. 2.96 atm
If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, its final volume will be:
1. | 135 ml | 2. | 540 ml |
3. | 350 ml | 4. | 280 ml |
The kinetic energy for 14 grams of nitrogen gas at 127°C is nearly -
(mol. mass of nitrogen = 28 and gas constant = 8.31JK–1mol–1)
1. 1.0 J
2. 4.15 J
3. 2493 J
4. 3.3 J