At relatively high pressure,the van der Waals equation reduces to

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 $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$).

The deviation from the ideal gas equation $PV = nRT$ is maximum under which of the following conditions?

The correct equation for one mole of a real gas is ($a, b$ are constants)

Calculate the compressibility factor for $SO_2$,if $1 \ mol$ of it occupies $0.35 \ L$ at $300 \ K$ and $50 \ atm$ pressure.

Under which conditions do intermolecular forces become effective?