Ideal Gas Law (Simple )

  • Thread starter Rockstar47
  • Start date
  • #1
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Homework Statement



I need to find the volume for 1 kg of diatomic oxygen for a pressure of 150,000 Pa and a temperature of 100K. This is really part of a larger project, and I need to make sure I'm not tripping up on little details. It's that 1 kg of diatomic oxygen that I am a bit unsure about, or just plain having a brain freeze about.

R* = 8.314 J/K*mol
T = 100 K
P = 150,000 Pa
n = ??

Homework Equations



PV = nRT

The Attempt at a Solution



Solving the equation for V; V = nRT/P. No big deal. My problem is making sure I have the correct n in the equation. The mass of diatomic oxygen is 32.0 grams, which is what I was using in my solutions. However, I realize that I have 1 kg of O2, not 1 g of it. Should I really be using 32,000 for my n? Or something else?
 

Answers and Replies

  • #2
1,753
1
you're using the wrong R constant. i'm working on it right now.
 
Last edited:
  • #3
hage567
Homework Helper
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You haven't properly converted mass to moles. Check that your units make sense in your calculation.
 
  • #5
10
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Thanks, everyone.

If I am looking at this all correctly, since I have 1 kg of diatomic oxygen, my number of moles should be: 1000 g / 32.00 g, which gives me my number of moles (n) equal to 31.25. Am I on the right track now?
 
  • #6
1,753
1
yeppp
 
  • #7
10
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Thanks for the help, everyone!! It was a total brain freeze on my part...
 
  • #8
1,753
1
Thanks for the help, everyone!! It was a total brain freeze on my part...
what was your final answer?
 

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