As per Charles's law ,–273° C is the lowest possible temperature because:

1.	All gases get liquefied before reaching a temperature of – 273° C.
2.	All gases get liquefied after reaching a temperature of – 273° C.
3.	All gases have a critical temperature of –273° C.
4.	None of the Above.

The correct relation between density ($\mathrm{\rho }$) and pressure of gas (P) is-

1. $\mathrm{P}$ $\mathrm{\alpha }$ ${\mathrm{d}}^2$

2. $\mathrm{P}$ $\mathrm{\alpha }$ $\frac{1}{\mathrm{d}}$

3. $\mathrm{P}$ $\mathrm{\alpha }$ $\mathrm{d}$

4. None of the above

A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35 °C. The pressure would be-

1. 0.6 bar

2. 1.2 bar

3. 0.8 bar

4. 0.4 bar

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

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

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

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

A plot of pressure versus $\frac{1}{\mathrm{V}}$ for a gas at constant temperature is given below:

The relation between ${\mathrm{T}}_1, {\mathrm{T}}_2, \mathrm{and} {\mathrm{T}}_3$ is- 

 $1. {\mathrm{T}}_1>{\mathrm{T}}_2>{\mathrm{T}}_3$
$2. {\mathrm{T}}_1<{\mathrm{T}}_2<{\mathrm{T}}_3$
$3. {\mathrm{T}}_1>{\mathrm{T}}_2<{\mathrm{T}}_3$
$4. \mathrm{None} \mathrm{of} \mathrm{the} \mathrm{above}$

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