If density of vapours of a substance of molar mass 18 g/mole at 1 atm pressure and 500 K is
0.36 kg m–3 , then the value of Z for the vapours is-
(R = 0.082 L atm mole K–1)
1.
2.
3. 1.1
4. 0.9
Flask A of volume 10 litre containing 20 gram of H2 and flask B of volume 10 litre containing 88 gram CO2 are connected by a connector having negligible volume. When the valve of the connector is opened, the composition of H2 gas in flask B after opening the valve is-
1. 10%
2. 13%
3. 15%
4. 20%
At a certain temperature for which RT = 25 lit. atm. mol–1, the density of a gas, in gm lit–1, is d = 2.00P + 0.020 P2, where P is the pressure in atmosphere. The molecular weight of the gas in gm mol–1 is-
1. 25
2. 50
3. 75
4. 100
A mixture of carbon monoxide and carbon dioxide is found to have a density of 1.7 g/L at S.T.P. The mole fraction of carbon monoxide is-
1. 0.37
2. 0.40
3. 0.30
4. 0.50
The volume of a gas is 100 ml at 100°C. If the pressure remains constant then the temperature at which the volume becomes 200 ml is-
1. 200°C
2. 473°C
3. 746°C
4. 50°C
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 |
A flask containing air (open to atmosphere) is heated from 300 K to 500 K. The percentage of air escaped to the atmosphere is nearly-
1. 16.6
2. 40
3. 66
4. 20
A sealed tube which can withstand a pressure of 3 atmosphere is filled with air at and 760 mm pressure. The tube will burst at -
1. 900°C
2. 627°C
3. 726°C
4. 1173°C
The number of moles of H2 in 0.224 litre of hydrogen gas at STP (273 K, 1 atm.) is-
1. 1
2. 0.1
3. 0.01
4. 0.001