At $300 \ K$,the compressibility factor of $1 \ mole$ of a gas is $1.1$. Its pressure is $2.706 \ atm$. What is its volume in $L$? (Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$).

For a real gas at $25^{\circ} C$ temperature and high pressure $(99 \ bar)$,the value of the compressibility factor is $2$. The value of the Van der Waals constant '$b$' is $\times 10^{-2} \ L \ mol^{-1}$. (Nearest integer) (Given $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

Maximum deviation from ideal gas behavior is expected from which of the following gases?

$A$ gas at $350 \; K$ and $15 \; bar$ has a molar volume $20$ percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor $(Z)$ is

The compressibility factor $(z)$ is lower for $NH_3$ and $CO_2$ gases than that of $N_2$ gas, because

The correction factor '$a$' in the van der Waals equation for real gases corresponds to: