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:
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.
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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
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.
What is the difficulty of this problem?
Our tutors rated the difficulty ofA mixture of He and O 2 is placed in a 4.00 L flask at 32°C....as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Sabrina took 5 minutes and 20 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Hernandez's class at UCF.