How do ideal gases differ from real gases?

Real gases can deviate from ideal behavior under certain conditions due to various intermolecular forces and the finite volume of gas molecules. In contrast to ideal gases, which are based on theoretical assumptions that imply no intermolecular forces and that the volume of the gas particles themselves is negligible, real gases experience attractions and repulsions between their molecules. This is particularly evident under high pressure and low temperature conditions, where the molecules are closer together, and these forces become significant.

Additional factors contributing to the deviation from ideal behavior include the presence of polar molecules, the complexity of the gas, and the interactions between molecules. For instance, at high pressures, the volume occupied by the gas particles becomes non-negligible, thus affecting the overall behavior of the gas. This understanding of how real gases deviate from ideal conditions is crucial for accurate predictions and calculations in chemistry and physics when dealing with gases in practical situations.