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.
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 O2 and He
Do a mass to mole calculation using the molar mass
2. Find the mole fraction of O2 using the equation:
3. Solve for partial pressure of O2 given a total pressure of 8.2 atm.
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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