$A$ gas deviates from ideal behaviour at a high pressure because its molecules

At Boyle's temperature,the compressibility factor $Z$ for a real gas is:

For a gas,deviation from ideal behaviour is maximum at

$1 \ mol$ of a real gas is kept at a high pressure of $100 \ bar$ at $300 \ K$. If the van der Waals constant $b$ is $0.005 \ L \ mol^{-1}$, what are the values of the compressibility factor $Z$ of the gas and the $\%$ deviation of volume from ideality?

$Z$	$\%$ Deviation

For a gas,the deviation from ideal behavior is maximum at:

Consider the equation $Z = \frac{PV}{RT}.$ Which of the following statements is correct?