Dang, I was hoping to come to a solid conclusion on this one today since it's due, but you know, I do appreciate your help and will certainly repost for curiosity's sake. You'll hear from me again, thanks again!
From my original post:
In my last post when I said I didn't understand how I could treat water vapor as an ideal gas, I was referring to the total pressure (given) of 830 mm Hg. Perhaps to be more clear: I am confused as to whether or not this rule is referring to the TOTAL pressure of a...
Crap, you're right! Sorry, my brain gets jumbled from the numbers flying around in my head all day with these engineering classes... and I didn't do so great in psychrometrics or thermodynamics. But I'm in biothermodynamics now, so I need to understand this or it's fail for me.
I'm sorry, I didn't mean saturation pressure. I meant vapor pressure. So, should I recalculate mole fractions of the two ideal gases excluding water vapor and use that to calculate their partial pressures?
A gas mixture of 0.13 mol NH3, 1.27 mol N2, and 0.025 mol H2O vapor is contained at a total pressure of 830 mm Hg and 323 K. Calculate the following:
(a) Mole fraction of each component.
(b) Partial pressure of each component in mm Hg.
(c) Total volume of mixture in m3...