Final answer:
The mass of each gas in a 1.05 L mixture at 25.0 °C cannot be determined without additional information about the gases' identities and partial pressures or mole fractions. Ideal gas behavior and the Ideal Gas Law could be used if such details were available.
Step-by-step explanation:
To determine the mass of each gas present in a 1.05 L sample of a gas mixture at 25.0 °C, we would need to know the molar amount (moles) of each individual gas and their respective molar masses. Due to the limited information provided in the question, we cannot calculate the exact masses without additional data such as the identity of the gases and their partial pressures or mole fractions.
However, if we assume ideal gas behavior, we could use the Ideal Gas Law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. The mass (m) can then be calculated using n (the number of moles) and the molar mass (M) of the gas, such that m = n * M. Again, without specific details regarding the gases present, this calculation cannot be performed.