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?

FREE Expert 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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Problem Details

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?

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