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

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

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.

The surface tension of which of the following liquid is maximum:

1. C₆H₆

2. H₂O

3. C₂H₅OH

4. CH₃OH

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

Van der Waal's real gas acts as an ideal gas at which condition?

1. High temperature, Low pressure

2. Low temperature, High pressure

3. High temperature, High pressure

4. Low temperature, Low pressure

Choose the correct option for graphical representation of Boyle's law, which shows a graph of pressure vs. volume of a gas at different temperatures:

1.
2.
3.
4.

The correct option for the total pressure (in atm) in a mixture of 4 g O₂ and 2 g H₂ confined in a total volume of one liter at 0$°$C is :
[Given R=0.082 L atm mol^-1 K^-1, T=273 K]

1. 25.18

2. 26.02

3. 2.518

3. 2.602