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Ideal gas law

  1. May 15, 2015 #1
    1. The problem statement, all variables and given/known data
    upload_2015-5-15_0-53-46.png

    2. Relevant equations
    PV = nRT


    3. The attempt at a solution
    n = 5.3 moles
    R = 8.31 J/(mol K)
    T = 273 K
    now, with P, do we use 1 atm or 1.013 x 105

    i'll go with the latter, and the answer comes out to be 0.119 liters , does this sound correct?
     
  2. jcsd
  3. May 15, 2015 #2
    What is R in terms of liter-atm/mol K ?
     
  4. May 15, 2015 #3
    hmm, it is 0.082

    also, do we normally express P in Pascals or atm?
     
  5. May 15, 2015 #4
    In SI units it is Pa but normally it is a very small unit.
    In our day to day life we use atm.
    Remember if you are solving you should keep a track on units.
    Your attempt is also good.
    You will get answer in m3 and then 1m3 = 1000 liter.
     
  6. May 15, 2015 #5
    hmmm, is 1.19 L correct?
     
  7. May 15, 2015 #6
    No, can you show what have you done?
     
  8. May 15, 2015 #7
    P V = n R T
    (1.013x105) V = (5.3 moles )( 0.082 liter-atm/mol K) (273K)

    V = 0.00119 , i'm pretty sure this is in liters
     
  9. May 15, 2015 #8
    But P should be in atm then.
    I said keep track of units.
    So take P = 1atm.
     
  10. May 15, 2015 #9
    so V = (5.3 moles )( 0.082 liter-atm/mol K) (273K) = 118.64 Liters?

    thats huge for a bottle
     
  11. May 15, 2015 #10
    Yeah, that was what I was getting.

    Yeah, that is huge for a bottle but holding 5.3 moles of an ideal gas is a big thing.
     
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