All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium.What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.6 atm ?

Problem

A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium.

What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.6 atm ?

Solution

We’re being asked to calculate the partial pressure of oxygen (O) in a mixture of oxygen (O) and helium (He)


Recall that the partial pressure of a gas (PGas) in a mixture is given by:


Pgas = χgasPtotal


where χGas = mole fraction of the gas and Ptotal = total pressure of the gas mixture


The mole fraction of the gas is then given by: 


χgas = moles gastotal moles


We will do the following steps to solve the problem: 

Step 1: Calculate the moles of O and He

Step 2: Calculate the mole fraction of O

Step 3: Calculate the partial pressure of O


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