When the volume of the balloon approaches 0.0 L How do you account for the discrepancy?

When the volume of a balloon approaches 0.0 L, the ideal gas law (PV=nRT) suggests that pressure (P) would approach infinity, which is not physically realistic. This discrepancy arises because the assumptions of ideal gas behavior break down at very low volumes, where intermolecular forces and the finite size of gas molecules become significant. Additionally, real gases deviate from ideal behavior under high pressures and low volumes, leading to non-ideal interactions that the ideal gas law does not account for. Consequently, more complex models, such as the Van der Waals equation, are needed to accurately describe gas behavior in such conditions.