[mike_302]

I am checking my review answers before a test tomorrow... Thing is, the book doesn't give answers for it's unit review questions. So I have a couple of questions here for you guys... Let me know if my final answer is correct please, and thank you.

A mixture of gases in a cylinder contains 0.85 mol of methane, 0.55 mol of oxygen, 1.25 mol of nitrogen, and 0.27 mol of propane. The pressure on the cylinder guage is 2573 kPa. What pressure does each gas exert?

My answer would be to divide each molar amount by the total number of moles in the cylinder, then multiply by 100 to get the percent space taken up by each gas, then to find that percent of 2573 kPa. . Is that correct?


Thanks

[mike_302]

and then there's this one:

http://i160.photobucket.com/albums/t161/mike_302/HW001.jpg

[The_Student]

It all looks fine to me.

[mike_302]

so how bout the first question... with the pressure of the 4 gasses... I figured that my hand-written question was right... (wanted confirmation) but the first question I'm not sure of

[The_Student]

What did you get for your answer for the partial pressure of Oxygen?

[mike_302]

sorry about te slow response..

partial pressure of oxygen: I calculate 74.87kPa . 2.91% of the pressure...


If this IS right, then my hypothesis for this whole thing (for my own educational purposes...) would be the following (tell me if I am correct please):


The partial pressures inside a cylinder are proportional to the moles of gas inside the cylinder, assuming all gases are the same temp... Of course, this is with ideal gases and not real gases.