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Physical Chemistry: Chemical Equlibrium

  1. Oct 26, 2014 #1
    1. The problem statement, all variables and given/known data
    For the reaction:
    2SO3(g) →2SO2(g)+O2(g)
    when 2.00 mol of SO3 is added to a flask at 10.0 L and 350 K at fixed volume, at equilibrium the ratio of SO2:SO3 is 0.663. What is the values of the equilibrium constant? What is ΔG° at this temperature?
    2. Relevant equations
    ΔrxnG°=-RTlnK

    3. The attempt at a solution
    I cannot figure out how to find K. I'm thinking I need to find the partial pressures of the various gases in order to get it but I cannot see how to do that.
     
  2. jcsd
  3. Oct 26, 2014 #2

    Borek

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    Staff: Mentor

    How many moles of SO2 and SO3 together? Knowing how many moles in total and the ratio, can you calculate number of moles of each?
     
  4. Oct 26, 2014 #3
    Well if we used 2.00 moles of SO2 to start then:
    1.326 moles of SO2
    0.674 moles of SO3
    at equilibrium
     
  5. Oct 26, 2014 #4

    Borek

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    Staff: Mentor

    Simple check:

    [tex]\frac {1.326}{0.674} \neq 0.663[/tex]
     
  6. Oct 26, 2014 #5
    I though I could but nothing I can come up with gives me a ratio of 0.663 :mad:
     
  7. Oct 26, 2014 #6
    What equation did you use to get the molar amounts?

    Chet
     
  8. Oct 27, 2014 #7

    Borek

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    Staff: Mentor

    I would ask "what equations" (and that's an important hint).
     
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