How do real gases differ from…

Real gases differ from ideal gases because, in a real gas, C. The particles occupy space A. Inter-molecular forces are present between particles Explanation: The particles in an ideal gas are considered to have no volume and do not exert attractions on each other. In contrast, real gas molecules possess a small but significant volume. For instance, at standard temperature and pressure (0 °C and 1 bar), the molar volume of an ideal gas is 22.711 L, while the molar volume of a real gas will typically exceed 22.711 L due to the volume taken up by the molecules. Furthermore, real gas molecules experience intermolecular forces, which means they tend to be slightly more compact, resulting in a molar volume that may be less than 22.711 L. Nevertheless, real gases still exhibit characteristics akin to ideal gases, as their molecules are constantly in motion, their average kinetic energy is solely a function of temperature, and they undergo elastic collisions, meaning there is no energy loss during interactions with one another or with the container walls.