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.

A mixture of ${\mathrm{N}}_2$ and Ar gases in a cylinder contains 7 g of ${\mathrm{N}}_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of ${\mathrm{N}}_2$ is:

[Use atomic masses (in g ${\mathrm{mol}}^{-1}$): N=14, Ar=40]

1. 12 bar

2. 15 bar

3. 18 bar

4. 9 bar

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

Equal masses of H₂, O₂ and CH₄ have been taken in a container of volume V at temperature 27 ºC in identical conditions. The ratio of the volumes of gases H₂:O₂ : CH₄ would be:

1. 8:16:1
2. 16:8:1
3. 16:1:2
4. 8:1:2

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

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