Calculating Oxygen Mass in a Portable Cylinder | Physics Homework Help

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To calculate the mass of oxygen in a portable cylinder with a volume of 0.0029 m3 and an absolute pressure of 1E7 Pa at 290 K, the ideal gas law equation pv=nRt is applied. The calculation yields 12.03 moles of oxygen, which is then multiplied by the molar mass of O2 (32 g/mol) instead of just O (16 g/mol). This results in a mass of 384.96 grams, or 0.38496 kg, which is the correct answer. The initial confusion stemmed from using the incorrect molar mass for oxygen. The final mass of oxygen in the cylinder is 0.38496 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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