According to Dalton's Law of Partial Pressure, what is the relationship between the total pressure of a gas mixture and the individual gases within it?

The correct answer reflects that Dalton's Law of Partial Pressure states that the total pressure exerted by a mixed gas is precisely equal to the sum of the partial pressures of the individual gases present in the mixture. Each gas in the mixture contributes to the overall pressure in proportion to its amount, or mole fraction, in the mixture. This law is derived from the assumption that gases behave ideally and do not interact with each other; thus, each gas can be considered separately without affecting the others.

In practical terms, if you have a mixture of gases, you can find the total pressure by simply adding together the pressures that each gas would exert if it occupied the entire volume alone at the same temperature. This concept is fundamental for understanding gas behaviors and is widely applicable in various scientific and engineering contexts.