Problem: A mixture of He and O 2 is placed in a 4.00 L flask at 32°C. The partial pressure of the He is 2.7 atm and the partial pressure of the O2 is 1.4atm. What is the mole fraction of O 2?a. 0.224b. 0.341c. 0.481d. 0.518e. 0.659

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FREE Expert Solution

We’re being asked to calculate the mole fraction of O2 in a 4.00 L flask at 32°C which contains a mixture of He and O2.


Mole fraction can be calculated using the equation shown below:

χGas 1=moles Gas 1Total Moles



We’re going to calculate the mole fraction of O2 in the flask using the following steps:

Step 1. Calculate the number of moles of O2 present in the container using the ideal gas equation.
Step 2. Calculate the total number of moles of gas present in the container using the ideal gas equation.

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Problem Details

A mixture of He and O 2 is placed in a 4.00 L flask at 32°C. The partial pressure of the He is 2.7 atm and the partial pressure of the O2 is 1.4atm. What is the mole fraction of O 2?

a. 0.224
b. 0.341
c. 0.481
d. 0.518
e. 0.659

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Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

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