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Thread: Chemistry... I freakin hate it
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02-09-09, 10:13 AM #21
Re: Chemistry... I freakin hate it
Originally Posted by H?b
....
computerscience >physics >bio>chem
...
compsci + physics.... pricesless awsome...'ness
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02-09-09, 10:15 AM #24
Re: Chemistry... I freakin hate it
Originally Posted by H?b
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02-09-09, 10:34 AM #25
Re: Chemistry... I freakin hate it
Originally Posted by Bunni
If chem is < bio...and kraker sucks at chem, but is good at bio..that would mean that kraker=bio>chem...
But by that...you could say...god>compsci+phiscs=pricesless awesome+bio=kraker
Then....since i banged a compsci major once...and bunni gave me a reach around...you could say
Compsci+reacharound+B(compsci-major)priceless awesome=God
Kraker=God!
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02-09-09, 10:36 AM #26
Re: Chemistry... I freakin hate it
first of all the assumption you made is incorrect. 1 mL or N2 gas is not equal to 1 g of N2 gas. but you are on the right track.
I would go along these lines. Using P1/n1=P2/n2 we can conclude that this amount of gas would go from the .0012531 at 4atm to .0004177 at 1 atm. thus the amount of N2 gas released would be the difference of this... or 0.0012531 mol/L.
now you can use the ideal gas law to find the volume. PV=nRT
(1.0)(x)=(0.0012531)(0.082)(310)
x=0.03189L
or 31.89mL
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02-09-09, 11:21 AM #29
Re: Chemistry... I freakin hate it
Draco was asleep for this discourse, but took upon himself to have a stab at it over morning crap.
Slightly different approach than sacred's, let's see if it holds water (*rimshot*).
Answer is in units of volume, so solve PV = nRT for V, V = nRT/P.
We know:
0.0016708 mol/L @ 4 atm
and, doing a little multiplication: 0.0005355 mol/L @ 1 atm.
We're taking a gas under 4 atm of pressure and reducing it to 1 atm, so only a portion comes out of solution (the rest remaining to maintain saturation in the solution). Further, we can assume that we're working with 1L solution's worth of gas, therefore we subtract:
0.0016708 - 0.0005355 = 0.00113528 mol
And then we solve our ideal gas equation:
(0.00113528 mol)(0.0821 atmL/molK)(310 K)/(1 atm) = 0.02889393 L, or 28.89393 mL gas will come out of solution, per L of solution.
Draco
PS: The difference may be in rounding errors in the given numbers or whathave you. We're within 10%. Claim atmospheric variance and throw yourself on the mercy of the court, AFAIAC.
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02-09-09, 12:54 PM #30
Re: Chemistry... I freakin hate it
Thanks for the help draco and sacredsarcasm, I see I was supposed to be solving for V now, DUH.
Originally Posted by Imisnew2
V = nRT/P
n = x4atm - x1atm = 0.0012531 mol/L
V = (0.0012531mol)(0.0821 L atm/K mol)(310K)/(1.00atm)
=0.0318926481 L
=31.8926481 mL
"or 31.89mL"
Originally Posted by sacredsarcasm
Originally Posted by draco7891
THANKYOU EVERYONE WHO HELPED WITH THIS, YOU GUYS ARE GREAT! (not you bunni!)
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