At extremely high pressures, which of the following thermodynamic statements accurately describe the — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

At very high pressures, molecules are forced very close together, making repulsive forces dominant ($Z>1$). Because $Z>1$, the gas is *harder* to compress than an ideal gas, making D incorrect. Because pressure is very large, the $a/V^2$ term becomes negligible compared to $P$, simplifying the van der Waals equation to $P(V_m - b) = RT$.