Daltons law of partial pressures
Dalton's partial pressure law (also known as Dalton's law) describes the properties of an ideal gas. This rule of thumb was observed by John Dalton in 1801. In a gas mixture in any container, if no chemical reaction occurs between the components, each gas is evenly distributed throughout the container, the pressure it generates and the pressure it generates when it occupies the entire container alone the same. That is, the pressure of a certain amount of gas in a certain volume of container is only related to temperature. For example, at zero degrees Celsius, the pressure of 1mol of oxygen in a volume of 22.4L is 101.3kPa. If 1 mol of nitrogen is added to the container and the volume of the container is maintained, the pressure of oxygen is still 101.3 kPa, but the total pressure in the container doubles. It can be seen that the pressure generated by 1 mol of nitrogen in this state is also 101.3 kPa. Dalton's partial pressure law is only applicable to ideal gas mixtures in principle, but it can also be approximately applied to real gas mixtures at low pressures.