Calculating Oxygen Mass in a Portable Cylinder | Physics Homework Help

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SUMMARY

The discussion focuses on calculating the mass of oxygen in a portable cylinder with a volume of 0.0029 m3 and an absolute pressure of 1 x 107 Pa at a temperature of 290 K. The ideal gas law equation, pv = nRT, was utilized to determine the number of moles (n), resulting in 12.03 moles. The mass was incorrectly calculated using the molar mass of a single oxygen atom (16 g/mol) instead of the correct molar mass for O2 (32 g/mol), leading to an erroneous final mass of 0.1925 kg.

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Homework Statement


In a portable oxygen system, the oxygen (O2) is contained in a cylinder whose volume is 0.0029 m3. A full cylinder has an absolute pressure of 1 107 Pa when the temperature is 290 K. Find the mass of oxygen in the cylinder.



Homework Equations


pv=nRt


The Attempt at a Solution


I used pv=nRt to get-----> (1E7)(.0029)=n(8.31)(290) and I solved for "n" and got n=12.03. Then i multiplied 12.03 by 16 (the mass of oxygen from the periodic table) to get mass from moles. This gave me 192.54 grams. But my answer had to be in kg, so i got .1925. But, my online homework keeps marking that wrong? Can you tell me if I made a mistake anywhere along the way? I am very confused about this.
 
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Your molar mass of oxygen is wrong. 16 is molar mass of just O.
 
oh i see now. thanks for your assistance
 

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