A bubble of air is underwater at a temperature15°C and the pressure 1.5 bar. If the bubble rises to the surface where the temperature is 25°C and the pressure is 1.0 bar, what will happen to the volume of the bubble?

1. Volume will become greater by a factor of 2.5
2. Volume will become greater by a factor of 1.6
3. Volume will become greater by a factor of 1.1
4. Volume will become smaller by a factor of 0.70

The pressure exerted by 6.0 g of methane gas in a 0.03 m³ vessel at 129 ºC is:
(Atomic masses : C = 12.01, H = 1.01 and R = 8.314 JK^–1mol^–1)

1. 13409 Pa

2. 41648 Pa

3. 31684 Pa

4. 215216 Pa

For real gases van der Waals equation is written as

$(P+\frac{a{n}^2}{V^2})$ $(V-nb)$ $=$ $nRT$

where 'a' and 'b' are van der Waals constants.

Two sets of gases are:
(I) $O_2,$ $C{O}_2$ $,$ $H_2$ $and$ $He$        (II)$C{H}_4,$ $O_2$ $$ $and$ $H_2$ 
The gases given in set-I are in increasing order of 'b' and gases given in set-II are in decreasing order of 'a'. Select the correct order from the following:

1. $($ $I)O_2<He<H_2<C{O}_2(II)$ $H_2>O_2>C{H}_4$

2. $($ $I)H_2<He<O_2<C{O}_2(II)$ $C{H}_4>O_2>H_2$

3. $($ $I)H_2<O_2<He<C{O}_2(II)$ $O_2>C{H}_4>H_2$

4. $($ $I)He<H_2<C{O}_2<$ $$ $O_2\left(II\right)$ $C{H}_4>H_2>O_2$

A certain gas takes three times as long to effuse out as helium. Its molecular mass will be:

1.  36 u
2.  64 u
3.  9 u
4.  27 u

Average molar kinetic energy of CO and N₂ at same temperature is:

1. KE₁ = KE₂

2. KE₁ > KE₂

3. KE₁ < KE₂

4. Can't say anything. Both volumes are not given.

In a gaseous mixture which of $N{O}_2,C{O}_2,\mathrm{an}\mathrm{d }{N}_{2}O$ gases have the same rate of diffusion:

1. $N{O}_2$ $,$ $C{O}_2$

2. $C{O}_2$ $,$ $N_{2}O$

3. $N{O}_2$ $,$ $N_{2}O$

4. All of the above.

If 400 ml gas at 500 torrs and 666.6 ml gas at 600 torrs is taken in a container of 3 liters, then the total pressure of the mixture is:

1.  200 torr

2.  400 torr

3.  600 torr

4.  50 torr

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 

The minimum pressure required to compress 600 dm³ of a gas at 1 bar to 150 dm³ at 40°C is

1. 4.0 bar

2. 0.2 bar

3. 1.0 bar

4. 2.5 bar

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