A gas mixture containing He, Ne, and Ar exerts a pressure of 3.00 atm . What is the partial pres

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A gas mixture containing He, Ne, and Ar exerts a pressure of...

A gas mixture containing $\mathrm{He}, \mathrm{Ne}$, and Ar exerts a pressure of 3.00 atm . What is the partial pressure of each gas present in the mixture under the following conditions? a. There is an equal number of moles of each gas present. b. There is an equal number of atoms of each gas present. c. The partial pressures of $\mathrm{He}, \mathrm{Ne}$, and Ar are in a $3: 2: 1$ ratio. d. The partial pressure of He is one-half that of Ne and one-third that of Ar.

Key Concepts

Dalton’s Law of Partial Pressures

This law states that in a mixture of non-reacting gases, the total pressure is equal to the sum of the partial pressures of each individual gas. It provides a fundamental basis for understanding how the pressure contributed by each gas in a mixture is related to its mole fraction, independent of the identity of the gases present.

Mole Fraction

The mole fraction is the ratio of the number of moles of a particular component to the total number of moles in the mixture. In the context of gas mixtures, the partial pressure of a gas is directly proportional to its mole fraction. This concept is central when determining the individual contributions to the total pressure, regardless of whether gases are counted in equal numbers of moles or atoms.

Ideal Gas Behavior

Ideal gas behavior, as described by the Ideal Gas Law, underpins the analysis of gas mixtures. This concept assumes that gases behave independently and that their collisions are perfectly elastic. It allows one to apply simple proportional relationships between pressure, volume, temperature, and number of moles for each gas within the mixture.

Pressure Ratio Analysis

When partial pressures are given by specific ratios, it means that the individual pressures of the gases are distributed according to these ratios while still summing to the total pressure. Analyzing these ratios involves understanding that the individual pressures can be represented as fractions of the total pressure, based on the specified proportional relationships.

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