Under which of the following conditions does a gas deviate from ideal behaviour?
$A$. Low pressure
$B$. High pressure
$C$. Low temperature
$D$. High temperature

Pressure exerted by $1 \, mole$ of methane in a $0.25 \, L$ container at $300 \, K$ using van der Waals equation is ............... $atm$ (given $a = 2.253 \, atm \, L^2 \, mol^{-2}, b = 0.0428 \, L \, mol^{-1}$):

Write the van der Waals equation.

What kind of deviation will $2 \, mol$ of $N_2$ gas show in a $50 \, L$ container at $STP$?

$A$ gas has a compressibility factor of $0.5$ and a molar volume of $0.4 \ dm^3 \ mol^{-1}$ at a temperature of $800 \ K$ and pressure $x \ atm$. If it shows ideal gas behaviour at the same temperature and pressure,the molar volume will be $y \ dm^3 \ mol^{-1}$. The value of $x / y$ is . . . . . .
[Use: Gas constant,$R = 8 \times 10^{-2} \ L \ atm \ K^{-1} \ mol^{-1}$ ]

In the van der Waals equation,which of the following will have the highest value of '$a$'?