Real gas behavior approaches ideal gas equation when

Correct option is D

​$$\textbf{Ideal Gas Law:} \quad PV = nRT\text{Assumes:} \\\text{- Zero molecular volume.} \\\text{- No intermolecular forces.} \\\text{Real gases deviate due to:} \\\textbf{- Finite molecular size} \ (\text{excluded volume}) \\\textbf{- Intermolecular forces} \ (\text{e.g., van der Waals})\\[1em]\textbf{Mathematical Justification (van der Waals Equation):} \\\left( P + \frac{an^2}{V^2} \right)(V - nb) = nRT\\[1em]\text{As } P \to 0 \text{ and } T \to \infty: \\\quad \frac{an^2}{V^2} \to 0 \quad \text{(forces negligible)} \\\quad V - nb \approx V \quad \text{(volume correction negligible)} \\\quad \text{Reduces to } PV = nRT$$​​