Problem, Where did I go wrong?

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In summary, in a portable oxygen system, the oxygen is stored in a cylinder with a volume of 0.00260 m3 and an absolute pressure of 1.00e7 Pa at 299 K. Using the ideal gas law, the number of moles of oxygen was calculated to be 935499.4. Multiplying this by Avogadro's number and the atomic mass of oxygen (32), the mass of oxygen in the cylinder was found to be incorrect.
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physics4u
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Homework Statement



In a portable oxygen system, the oxygen (O2) is contained in a cylinder whose volume is 0.00260 m3. A full cylinder has an absolute pressure of 1.00e7 Pa when the temperature is 299 K. Find the mass of oxygen in the cylinder.

Homework Equations


PV=nRT


The Attempt at a Solution


So first I solved for n in the PV=nRT eqn, (1.00e7)(.00260)/(8.31)(299K)= 935499.4 moles. After I obtained the Moles I multiplied by avadro's number (6.022e23) to get molecules, and than I multiplied by 1.6605e-27kg/atomic units to get mass. Aparently my answer is incorrect, where did I go wrong for solving this problem?


 
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  • #2
What did you multiply by 1.6605e-27kg/atomic units to get mass? Also remember the molecular weight of O2 is 32.
 
  • #3


It seems like you have correctly used the ideal gas law to solve for the number of moles of oxygen in the cylinder. However, the issue may be with your conversion from moles to mass. In your calculation, you multiplied by Avogadro's number and then by the conversion factor from atomic units to kilograms. This would give you the mass of the entire cylinder, not just the oxygen. To find the mass of oxygen, you need to multiply the number of moles by the molar mass of oxygen (32 g/mol). This will give you the mass of oxygen in grams. You can then convert to kilograms if needed. I hope this helps!
 

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