A real gas obeying van der Waal's equation will resemble ideal gas if the constants — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

An ideal gas is defined theoretically by the absence of intermolecular forces and having point-mass molecules with zero volume. In the van der Waals equation, parameter '$a$' corrects for attractive forces and '$b$' for molecular volume. Thus, the gas behaves ideally when both $a$ and $b$ are negligibly small. Therefore, correct answer is A.