What conditions define an ideal gas?

An ideal gas is defined under conditions of high temperature and low pressure. At high temperatures, the kinetic energy of gas particles increases, allowing them to move rapidly and overcome intermolecular forces that can cause deviations from ideal behavior. Additionally, low pressure means that gas particles are further apart and the volume occupied by individual particles becomes negligible compared to the volume of the container. This scenario minimizes interactions between gas particles, which is a key assumption of the ideal gas model.

Under these conditions, gases behave in accordance with the ideal gas law, as there are minimal forces acting between particles and they occupy a volume that can be approximated as entirely empty space. In essence, high temperature ensures high kinetic energy, while low pressure reduces the influence of particle size and intermolecular forces, both of which contribute to a gas behaving ideally.