A mixture of $\mathrm{C}{\mathrm{H}}_4$ and ${\mathrm{C}}_2{\mathrm{H}}_2$ occupied a certain volume at a total pressure equal to 63 torr. The same gas mixture was burnt to $\mathrm{C}{\mathrm{O}}_2$ and ${\mathrm{H}}_2\mathrm{O}\mathrm{ }\left(\mathrm{\lambda }\right)$ $\mathrm{C}{\mathrm{O}}_2\mathrm{ }\left(\mathrm{g}\right)$ alone was collected in the same volume and at the same temperature, the pressure was found to be 69 torr.

What was the mole fraction of $\mathrm{C}{\mathrm{H}}_4$ in the original gas mixture?

'$\mathrm{x}$' $\mathrm{g}$ of molecular oxygen $\left({\mathrm{O}}_2\right)$ is mixed with $200 \mathrm{g}$ of neon $\left(\mathrm{Ne}\right)$. The total pressure of the nonreactive mixture of ${\mathrm{O}}_2$ and $\mathrm{Ne}$ in the cylinder is $25$ bar. The partial pressure of $\mathrm{Ne}$ is $20$ bar at the same temperature and volume. The value of '$\mathrm{x}$' is

[Given: Molar mass of ${\mathrm{O}}_2=32 \mathrm{g} {\mathrm{mol}}^{-1}$. Molar mass of $\mathrm{Ne}=20 \mathrm{g} {\mathrm{mol}}^{-1}$]

$2{\mathrm{SO}}_2( \mathrm{g})+{\mathrm{O}}_2( \mathrm{g})\to 2{\mathrm{SO}}_3( \mathrm{g})$ 

The above reaction is carried out in a vessel starting with partial pressure ${\mathrm{P}}_{{\mathrm{SO}}_2}=250 \mathrm{m} \mathrm{bar}$, ${\mathrm{P}}_{{\mathrm{O}}_2}=750 \mathrm{m} \mathrm{bar}$ and ${\mathrm{P}}_{{\mathrm{SO}}_3}=0 \mathrm{bar}$. When the reaction is complete, the total pressure in the reaction vessel is _____ $\mathrm{m} \mathrm{bar}$. 

(Round off of the nearest integer).

The volume of gas $\mathrm{A}$ is twice than that of gas $\mathrm{B}$. The compressibility factor of gas $\mathrm{A}$ is thrice than that of gas $\mathrm{B}$ at same temperature. What are the pressures of the gases for equal number of moles?

Which one of the following graphs is not correct for ideal gas?

$\mathrm{d}=$ Density, $\mathrm{P}=$ Pressure, $\mathrm{T}=$Temperature