For a real gas (van der Waal's gas), behaving ideally, the pressure may be — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

Van der Waals gas behaves ideally when intermolecular forces are negligible. (A) At very low pressure: molecules far apart, forces $\to0$, $Z\to1$. \checkmark (C) At Boyle temperature and moderate pressure: attractive and repulsive corrections cancel. \checkmark (B) Very high pressure: repulsive forces dominate, $Z>1$. \texttimes Correct options: $\boxed{A,\ C}$