Question #66a05
1 Answer
The partial pressure of Ar will be
So, you know that you start with a certain mass of argon in the flask. The first thing you need to do is figure out exactly how many moles of argon you have
Now you add an unknown number of moles of ethane vapor to the flask. Since you know volume, total pressure, and temperature, you can use the ideal gas law equation to figure out how many moles of both argon and ethane can be found in the flask
So, your mixture contains a total of 0.0511 moles of gas, argon and ethane. Now, you can express the partial pressure of argon by using its mole fraction and the total pressure in the flask
Since you know how many moles of argon you have, its partial pressure will be