Final answer:
The partial pressure of each gas in a mixture is directly proportional to its mole fraction. The combined partial pressures of the gases yield the total pressure of the mixture, as described by Dalton's law. The ideal gas law also affirms this relationship between partial pressure and molar concentration.
Step-by-step explanation:
The partial pressure of each gas in a mixture is directly proportional to its mole fraction (X). This can be understood by considering that in a mixture of ideal gases, each gas exerts a pressure that is equal to the total pressure multiplied by the fraction that the gas comprises within the mixture.
Dalton's law of partial pressures states that in a mixture of gases, the total pressure is the sum of the partial pressures of the individual components, assuming no interaction between the gases.
The ideal gas law, which can be represented as pV = nRT, where 'p' is pressure, 'V' is volume, 'n' is moles of gas, 'R' is the ideal gas constant, and 'T' is temperature, also indicates that the partial pressure is proportional to the molar concentration of the gas within a given volume and temperature.
For example, if gas A and gas B are in a container and the total pressure is 2 atmospheres with gas A making up 1/4 of the mixture, then the partial pressure of gas A would be 0.5 atmospheres (1/4 of the total pressure).