A gas mixture contains each of the following gases at the...

A gas mixture contains each of the following gases at the indicated partial pressures: $\mathrm{N}_{2}, 215$ torr; $\mathrm{O}_{2}, 102$ torr; and He, 117 torr. What is the total pressure of the mixture? What mass of each gas is present in a 1.35 -L sample of this mixture at $25.0^{\circ} \mathrm{C}$ ?

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Key Concepts

Molar Mass and Mole Concept

This concept relates the mass of a substance to the number of moles through its molar mass. Once the number of moles of a gas is calculated using the Ideal Gas Law, the mass of the gas can be determined by multiplying these moles by the respective molar mass of the gas.

Ideal Gas Law

The Ideal Gas Law, expressed as PV = nRT, relates the pressure, volume, temperature, and number of moles of a gas. It is essential for determining the number of moles of each gas when given the conditions of a container, and subsequently for further calculations such as mass determination.

Dalton's Law of Partial Pressures

This principle states that in a mixture of non-reactive gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. It allows us to calculate the overall pressure of the gas mixture by adding the individual contributions from each gas present.

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