For a real gas, the $\mathrm{P}-\mathrm{V}$ curve was experimentally plotted, and it had the following appearance. With respect to liquefaction, choose the correct statement:

 

Consider the following statements:
The coefficient B in the Virial equation of state
(i) is independent of temperature
(ii) is equal to zero at Boyle temperature
(iii) has the dimension of molar volume, Which of the above statements are correct.

Which of the above statements are correct.
${\mathrm{PV}}_{\mathrm{m}}=\mathrm{RT}\left(1+\frac{\mathrm{B}}{{\mathrm{V}}_{\mathrm{m}}}+\frac{\mathrm{C}}{{\mathrm{V}}_{\mathrm{m}}^2}+\dots \dots \dots \right)$

The curve of pressure volume $\left(\mathrm{PV}\right)$ against pressure $\left(\mathrm{P}\right)$ of the gas at a particular temperature is as shown, according to the graph which of the following is incorrect (in the low pressure region):

$1$ mole of ${\mathrm{CCl}}_4$ vapours at $27 °\mathrm{C}$ occupies a volume of $35.0 \mathrm{L}$.If Van der Waal's constant are $\mathrm{a}=20.39 {\mathrm{L}}^2 \mathrm{atm} {\mathrm{mol}}^{-2}$ and $\mathrm{b}=0.1383 \mathrm{L}$ ${\mathrm{mol}}^{-1}$, calculate compressibility factor $\mathrm{Z}$ under,
$\left(\mathrm{x}\right)$ low pressure region    $\left(\mathrm{y}\right)$ high pressure region

Report your answer as nearest whole number of $(\mathrm{x}+\mathrm{y})\times 10$.

To an evacuated $504.2 \mathrm{ml}$ steel container, is added $25 \mathrm{g} {\mathrm{CaCO}}_3$ and the temperature is raised to $1500 \mathrm{K}$causing a complete decomposition of the salt. If the density of $\mathrm{CaO}$ formed is $3.3 \mathrm{g} {\mathrm{cc}}^{-1},$ find the accurate pressure developed in the container using the Van der Waals equation of state. The Van der Waals constants for ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ are $\mathrm{a}=4\frac{{\mathrm{L}}^2-\mathrm{atm}}{{\mathrm{mol}}^2}, \mathrm{b}=0.04\frac{\mathrm{L}}{\mathrm{mol}}·$

Given that atomic weight of $\mathrm{Ca}=40, \mathrm{C}=12, \mathrm{O}=16$.

Report your answer as nearest whole number.