ANS:C - 1

As the pressure of a gas approaches zero, the compressibility factor of a real gas approaches 1. The compressibility factor (𝑍Z) of a gas is defined as the ratio of the actual volume of the gas to the volume predicted by the ideal gas law at the same temperature and pressure. At low pressures, real gases behave more like ideal gases, and their compressibility factors approach 1. This is because at low pressures, the molecules of a gas are far apart and experience minimal intermolecular forces, causing them to behave more like an ideal gas. As a result, the actual volume of the gas closely approximates the volume predicted by the ideal gas law. Therefore, as the pressure of the gas approaches zero, the compressibility factor approaches 1.