Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: jennielynn_1980 on May 14, 2006, 03:16:55 PM
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How many moles of oxygen gas are present if the volume of the gas is 274mL at a pressure of 120 kPa and a temperature of 75 oC.
V= 274 mL = 0.274L
n = ?
R = 8.31 kPa x L/mol x K
T = 75 = 348 K
PV = nRT
therefore n = PV/RT
n = 120 kPa x 0.274 L
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8.31 kPa x L x mol -1 x K -1 x 348 K
(insert missing steps which is what I cannot figure out)
n = 0.0114 mol
I have never taken chemistry before so I really have no idea about conversions and I have very limited knowledge about the ideal gas law.
Thanks!
Jennie
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???
Everything is ok: what's the matter?
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n = 120 kPa x 0.274 L
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8.31 kPa x L x mol -1 x K -1 x 348 K
When I go to work out this part of the equation to get to the final answer, I am not sure if I am subing the correct numbers because I dont' come out with the correct answer
So kPa = 101.3
L= 22.4
mol -1 = 1 ?
K -1 1/273 ?
Are these the correct substitutions?
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These are units, you don't substitute any values for these as they define units of your answer. You have to do two things:
1. Multiply and divide all numbers present in the formula - it will give 0.0114 (watch significant digits number).
2. Cancel out units to check what is unit of your answer.
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Thank you! I understand now :)
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8.31 kPa x L x mol -1 x K -1 x 348 K
Why is the unit of R kPa.L/mol.K? R ought to be 8.314 J/mol.K or 8.314 kJ/kmol.K
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PV=nRT
R=PV/nT
Approximately
R = ( 101.325 kPa * 22.414 L ) / ( 1 mol * 273.15 K )
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Why is the unit of R kPa.L/mol.K?
Why not?
R ought to be 8.314 J/mol.K or 8.314 kJ/kmol.K
0.08205783 L*atm/(K*mol)
8.314510 kPa*dm3/(K*mol)
8,314472 L*kPa/(K*mol)
8.314472 J/(mol*K)
62,3637 L*mmHg/(K*mol)
83,14472 L*mbar/(K*mol)
1.987216 cal/(K*mol)
Use whichever fits units given in the question ;)
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Oh well.. I thought 8.314 is only applicable to J/mol.K or kJ/kmol.K
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83,14472 L*mbar/(K*mol)
what is this one? like what is mbar?
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1 bar = 100 000 pascals (Pa)
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1 bar = 100 000 pascals (Pa)
oh ok thanks :)
i had no idea about so many unit derevations for R, i was only aware of the ones for 8.314 and .0821 :P
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So if I have learned anything ;) this would be right:
P1V1 = P2V2
T1 T2
P = 0.75 atm
V = ?
T = -30?C = 243K
P = 1.25 atm
V = 255 L
T = 40.0 ?C = 313K
0.75 atm ? = 1.25atm x 255 L
243K 313K
? = 243K x 1.25 atm x 255 L
0.75 atm x 313K
? = 77456.25
234.75
? = 330 L
The volume of gas at -30? C and 0.75 atm would be 330L if the same gas had a volume of 255 L at 40.0?C and 1.25 atm.
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Looks correct.
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0.08205783 L*atm/(K*mol)
8.314510 kPa*dm3/(K*mol)
8,314472 L*kPa/(K*mol)
8.314472 J/(mol*K)
62,3637 L*mmHg/(K*mol)
83,14472 L*mbar/(K*mol)
1.987216 cal/(K*mol)
Oh man, that's nothing...
http://www.katmarsoftware.com/gconvals.htm