A suba divers tank contains. 29Kg of O2 (Oxygen) compressed into a volume of 2.3L. Calculate the oxygen gas pressure inside the tank at 9 degrees celcius. I got 96.35 atm. For my answer but i don't know if the answer is reasonable because the pressure is so high.
-
PV=nRT
29kg O2 - convert to moles for n
O2 is 32g/mol, therefore: 29000g O2 (1mol/32g) = 906.25 mol O2
R is Faraday's constant, T = 9+273 = 282K
P(2.3) = 906.25(.08206)(282)
2.3p = 20971.46
P = 9118.025 atm
Where you got 96.35 from I don't know.
And people wonder why scuba tanks can explode. :)
29kg O2 - convert to moles for n
O2 is 32g/mol, therefore: 29000g O2 (1mol/32g) = 906.25 mol O2
R is Faraday's constant, T = 9+273 = 282K
P(2.3) = 906.25(.08206)(282)
2.3p = 20971.46
P = 9118.025 atm
Where you got 96.35 from I don't know.
And people wonder why scuba tanks can explode. :)
-
R is most definitely NOT Faraday's constant...It is the universal gas constant. Please educate your self to the very important difference.
Report Abuse
-
PV = nRT
P is the pressure you are trying to find.
V is the volume.
n is the number of moles. You find it by dividing the mass of the oxygen by the molar mass of oxygen(32 g/mol).
R is the gas constant(0.08205746 L*atm/K*mol).
T is the temperature in Kelvin. You find it by adding the Celsius temperature to 273.15.
V = 2.3L
n = 29kg / 32g/mol = 906.25mol
R = 0.08205746L*atm/K*mol
T = 273.15 + 9 = 282.15K
P = nRT/V = 9122.59 atm
Your answer of 96.35 atm was much too low. However, the actual answer is ridiculously high. Real life scuba tanks can typically store gas at 200 to 300 atm. However, they usually only contain only 3kg of gas and have a volume of around 10L. The scuba tank in your problem not only contains an unrealistic amount of oxygen, it is also extremely small.
P is the pressure you are trying to find.
V is the volume.
n is the number of moles. You find it by dividing the mass of the oxygen by the molar mass of oxygen(32 g/mol).
R is the gas constant(0.08205746 L*atm/K*mol).
T is the temperature in Kelvin. You find it by adding the Celsius temperature to 273.15.
V = 2.3L
n = 29kg / 32g/mol = 906.25mol
R = 0.08205746L*atm/K*mol
T = 273.15 + 9 = 282.15K
P = nRT/V = 9122.59 atm
Your answer of 96.35 atm was much too low. However, the actual answer is ridiculously high. Real life scuba tanks can typically store gas at 200 to 300 atm. However, they usually only contain only 3kg of gas and have a volume of around 10L. The scuba tank in your problem not only contains an unrealistic amount of oxygen, it is also extremely small.