At what condition do the ideal gas law and Dalton's law typically apply?

The ideal gas law and Dalton's law apply best under conditions of low pressure and high temperature. This is because, under low pressure, gas particles are far apart, meaning there is minimal interaction between them, allowing them to behave more ideally. The assumptions of the ideal gas law—that gas particles occupy no volume and do not exert forces on each other—hold true when the pressure is low.

High temperature complements this situation as it increases the average kinetic energy of the gas molecules, making them move faster and reducing the likelihood of intermolecular forces affecting their behavior. Under these conditions, gases behave more closely to the ideal predictions provided by the ideal gas law.

In contrast, at high pressures or low temperatures, gas particles are forced closer together, which increases intermolecular forces and leads to deviations from ideal behavior.