# 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.

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:

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