Question

A heliox deep-sea diving mixture contains $4.0 \%$ oxygen and 96.0\% helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm?

   A heliox deep-sea diving mixture contains $4.0 \%$ oxygen and 96.0\% helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm?

Introductory Chemistry

Introductory Chemistry

Nivaldo J. Tro 5th Edition

Chapter 11, Problem 81

Instant Answer

Solved by Expert Madeline Currie

09/01/2020

Step 1

Mathematically, it can be represented as: \[P_{total} = P_{O2} + P_{He}\] where \(P_{total}\) is the total pressure, \(P_{O2}\) is the partial pressure of oxygen, and \(P_{He}\) is the partial pressure of helium. Show more…

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A heliox deep-sea diving mixture contains $4.0 \%$ oxygen and 96.0\% helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm?

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Key Concepts

Mole Fraction

The mole fraction is the ratio of the number of moles of a particular gas to the total number of moles in the gas mixture. It is used to determine the proportion of each gas in a mixture, and when multiplied by the total pressure, it yields the partial pressure of that gas.

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 the individual gases. It is a fundamental concept in gas behavior, particularly when calculating the contributions of specific gases in mixtures.

Partial Pressure

Partial pressure refers to the pressure that an individual gas in a mixture would exert if it occupied the entire volume alone. It is calculated by multiplying the total pressure by the mole fraction of that specific gas, making it a key concept in understanding gas mixtures.

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