Under which conditions does Dalton's law closely describe real gases?

Dalton’s law, formulated by the British scientist John Dalton in 1801, states that the total pressure of a gas mixture is the sum of the partial pressures of its individual components.123

While the law is derived from the kinetic theory of gases under the assumption of an ideal gas, it is only an approximation for real gases. Dalton’s law describes the behavior of real gases quite closely under the following conditions:1

• Low pressures: When the gas is at sufficiently low pressure, the molecules are far enough apart that their interactions are minimized.14
• High temperatures: At high temperatures, the high speeds of the gas molecules allow them to overcome potential interactions, causing them to behave more like an ideal gas.14

Conversely, the law becomes less accurate when gases are near their condensation point, as the assumptions of negligible molecular volume and lack of intermolecular forces no longer hold.42