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 8.2 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 8.2 atm?

Solution

For this problem, we need to determine the partial pressure of Oxygen, in a mixture of 2.0 g O2 for every 98.0 g He at a total pressure of 8.2 atm. 


Recall that based on Dalton’s Law, the partial pressure of each gas is the total pressure multiplied by the mole fraction of that gas.


 Pgas=Xgas·PTot 

Where:

PTot = total Pressure in atm

P° = partial pressure of a gas in atm 

X = mole fraction of gas


We will need to do these steps to solve the partial pressure of O2:

1.  Solve for # of moles of Oand He 

Do a mass to mole calculation using the molar mass 

2. Find the mole fraction of Ousing the equation:


XO2 =moles O2moles O2 + moles He

3. Solve for partial pressure of O2 given a total pressure of 8.2 atm. 


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