The temperature at which the second virial coefficient of a real gas is zero is called:

$A$ certain quantity of real gas occupies a volume of $0.15 \ dm^3$ at $100 \ atm$ and $500 \ K$ when its compressibility factor is $1.07$. Its volume at $300 \ atm$ and $300 \ K$ (when its compressibility factor is $1.4$) is $........ \times 10^{-4} \ dm^3$ (Nearest integer).

The $Z$ vs $P$ graph for four gases is given below at the same temperature.
Which of the gases will have the highest value of critical temperature $(T_c)$?

For a real gas (molar mass $= 60 \, g/mol$),if the density at the critical point is $0.80 \, g/cm^3$ and its critical temperature $T_c = \frac{4 \times 10^5}{821} \, K$,then the van der Waals constant $a$ (in $atm \, L^2 \, mol^{-2}$) is:

What are the values of $Z$ for $CO_2, CH_4$,and $O_2$ at $200 \ bar$ and $900 \ bar$ pressure?

What are the ideal pressure and volume of a real gas?