I got Partial pressure of O2= 12.96 atm
And He= 3.425 atm ....Is it right?
This is the question..
Any help would be appreciated, I m just really unsure
Mixtures of helium and oxygen are used in scuba diving tanks to help prevent the
bends, which is a condition caused by nitrogen bubbles forming in the bloodstream. If
95 L of oxygen and 25 L of helium at STP are pumped into a scuba tank with a volume
of 8.0 L, what is the partial pressure of each gas in the tank and what is the total
pressure in the tank at 25 deg C?
And He= 3.425 atm ....Is it right?
This is the question..
Any help would be appreciated, I m just really unsure
Mixtures of helium and oxygen are used in scuba diving tanks to help prevent the
bends, which is a condition caused by nitrogen bubbles forming in the bloodstream. If
95 L of oxygen and 25 L of helium at STP are pumped into a scuba tank with a volume
of 8.0 L, what is the partial pressure of each gas in the tank and what is the total
pressure in the tank at 25 deg C?
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I got 12.96 atm O2 and 3.41 atm He, it must just be a rounding error. Really only two significant figures anyway. Sounds like you know how to do the problem, but one approach is to use the combined gas law P1V1/T1 = P2V2/T2
(1 atm)(120 L)/273.15 K = P2 (8.0 L)/ 298.15 K
Solving for P2 you get 16.37 atm
The mole fraction of O2 is 95/120 and multiplying the total pressure of 16.37 atm by this fraction gives you 12.96 atm.
The mole fraction of He is 25/120 and multiplying 16.37 by this fraction gives 3.41 atm. (Or you could subtract the 12.96 atm.)
(1 atm)(120 L)/273.15 K = P2 (8.0 L)/ 298.15 K
Solving for P2 you get 16.37 atm
The mole fraction of O2 is 95/120 and multiplying the total pressure of 16.37 atm by this fraction gives you 12.96 atm.
The mole fraction of He is 25/120 and multiplying 16.37 by this fraction gives 3.41 atm. (Or you could subtract the 12.96 atm.)