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. $\frac{41}{50}$

2. $\frac{50}{41}$

3. 1.1

4. 0.9

The graph that represents an isobar $\left(\frac{\mathrm{nR}}{\mathrm{p}}\mathrm{\hspace{0.17em}}>\mathrm{\hspace{0.17em}1}\right)$ is-

1.  

2. 

3. 

4.  

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:

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 ${27}^{o}C$ 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