A candle is burnt in a beaker until it extinguishes itself. A sample of gaseous mixture in the beaker contains $6.08\times {10}^{20}$ molecules of ${\mathrm{N}}_2$, $0.76\times {10}^{20}$ molecules of ${\mathrm{O}}_2$, and $0.50\times {10}^{20}$ molecules of ${\mathrm{CO}}_2$. The total pressure is $734 \mathrm{mm} \mathrm{of} \mathrm{Hg}$. The partial pressure of ${\mathrm{O}}_2$ would be:

'$\mathrm{x}$' $\mathrm{g}$ 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?