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: $\mathrm{N}_{2}$, 325 torr; $\mathrm{O}_{2}, 124$ torr; and $\mathrm{He}_{3}, 209$ torr. What is the total pressure of the mixture? What mass of each gas is present in a $1.05-\mathrm{L}$ sample of this mixture at $25.0^{\circ} \mathrm{C} ?$

Key Concepts

Unit Conversions

Accurate application of these concepts requires careful unit conversions, for example, converting pressure from torr to atmospheres when using the Ideal Gas Law. Ensuring that all measurements are in consistent units is vital for correct calculation results.

Gas Mixture Composition

Analyzing a gas mixture involves understanding that each component contributes independently to the total pressure, and that its individual properties, such as molar mass, can be used along with the Ideal Gas Law to determine its specific amount and mass.

Molar Mass

Molar mass represents the mass of one mole of a substance and is used to convert the number of moles obtained from the Ideal Gas Law into mass. This concept is key to quantifying how much of each gas is present in a sample based on its chemical identity.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) connects pressure, volume, temperature, and the number of moles, allowing us to calculate the amount of substance present in a gas sample. This law is fundamental when converting measured pressures and volumes into molar quantities, which can then be related to mass.

Dalton's Law of Partial Pressures

Dalton's Law states that the total pressure of a gas mixture equals the sum of the individual partial pressures of each gas. This principle is crucial for determining the overall pressure in a mixture when the pressures of individual components are known.

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