The variation of pressure with the volume of the gas at different temperatures can be
graphically represented as per the following graph:

  

If the temperature increases from 200K to 400K (at constant pressure), the volume of a
gas would-  

1. Increase

2. Decrease

3. Remain constant

4. 1st decreases then increases

Consider the following graph:

The curve that represents CO₂ gas is - 

1. X

2. Y

3. Both X and Y 

4. Cannot predict from the graph

Pressure versus volume graph for a real gas and an ideal gas is shown below: 

The correct statement among the following is -

1. Real gases show a large deviation from ideal behaviour at low pressure.

2. Real gases show a very small deviation from ideal behaviour at low pressure.

3. Real gases do not behave ideally under any conditions at low pressure.

4. None of the above statements is correct

The plots of different values of pressure versus temperature are shown in the given figure. The correct order of volume for the following plot is-

1. V₄ < V₃ < V₂ < V₁

2. V₄ > V₃ < V₂ > V₁

3. V₄ > V₃ > V₂ > V₁

4. V₄ > V₃ > V₂ < V₁

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 

 Among water, ether, and acetone, water has the maximum boiling point and ether has the minimum boiling point. The correct order of vapour pressure of water, acetone and ether at $30°\mathrm{C}$ is-

1. Water<ether<acetone

2. Water<acetone<ether

3. Ether<acetone<water

4. Acetone<ether<water

The state of a gas can be described by quoting the relationship between:

1.  Pressure, volume, temperature

2.  Temperature, amount, pressure

3.  Amount, volume, temperature

4.  Pressure, volume, temperature, amount

With increase in temperature the surface tension of a liquid will:

1. Remains same

2. Decreases

3. Increases

4. No regular pattern is followed

The SI unit of viscosity coefficient $\left(\mathrm{\eta }\right)$ is-

1. Pascal

2. Nsm^-2

3. km^-2s

4. Nm^-2

Gases possess characteristic critical temperature which depends upon the magnitude of intermolecular forces between the particles. Following are the critical temperatures of some gases.

From the above data, the order of liquefaction of the given gases is-
(write the order from the gas liquefying first)
1. ${\mathrm{H}}_2,$ $\mathrm{He},$ ${\mathrm{O}}_2,$ ${\mathrm{N}}_2$
2. $\mathrm{He},$ ${\mathrm{O}}_2,$ ${\mathrm{H}}_2,$ ${\mathrm{N}}_2$
3. ${\mathrm{N}}_2,$ ${\mathrm{O}}_2,$ $\mathrm{He,}$ ${\mathrm{H}}_2$
4. ${\mathrm{O}}_2,$ ${\mathrm{N}}_2,$ ${\mathrm{H}}_2,$ $\mathrm{He}$