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Chemical Equilibrium with Multiple Kc

  1. Dec 7, 2012 #1
    1. The problem statement, all variables and given/known data
    Compound A can react to form B and C according to the following

    A<->2B Kc=1
    A<->C Kc=1

    If 1 mole of A is solved into 1 litre of water, what will the concentration of A be after equilibrium has been reached?


    2. Relevant equations
    ICE-tables(?)
    A<->2B+C
    Kc=(^2[C])/[A]




    3. The attempt at a solution
    Doing this homework the usual way, doing the ICE tables, I ended up with the solution c(A)=0.39, which is not correct according to the answer.
    This made me think that perhaps this can't be solved assuming that
    A<->2B+C , Kc=1, C(A) at start=1, but instead there is some other method?

    I would be grateful to have some tips on how I should approach this problem.
     
  2. jcsd
  3. Dec 7, 2012 #2

    Borek

    User Avatar

    Staff: Mentor

    This system can be described by three equations - two Kc and one mass balance. Write them all, solve.
     
  4. Dec 8, 2012 #3
    Hi
    I forgot to mention this task is something "off course" so I don't have any books to get information from. Also I don't know the english term for this reaction so it's hard to find answers on the internet.

    That being said, thank you for your advice. I would ask a bit more about what you meant with two Kc and Mass Balance.
    I suppose Mass Balance refers to conservation of mass? Would that mean that since [A] at start is 1 mole, then [A]+[2B]+[C] at end =1?
    I also made an attempt to solve this doing
    A<->C K=1 and solving for c(C)
    and
    A-<->2B K=1 and solving for c(B)
    but neither gave results that would be possible.
    I think the trouble is that once A reacts to form B it reacts again to form C, lowering c(A)
    and then A reacts again to form B in smaller amounts and so on in an endless loop.

    If there is a particular term used for this "multiple Kc" reaction, could you tell it? I'm sure if I knew where to look I'd be able to finish this.
     
  5. Dec 8, 2012 #4

    Borek

    User Avatar

    Staff: Mentor

    Yes.

    That's the approach I tried and it yielded something that looks quite reasonable.

    Doesn't matter. System is described by the equations that were listed and they are enough to take care of the problem. General approach to every equilibrium problem is to write all equations describing the equilibrium and all mass balances, and then to solve this system for all unknowns.
     
  6. Dec 10, 2012 #5
    Hi

    Thank you for your help.

    I redid my calculations and it seems that by iterating between the result of
    A<->C
    and
    A<->2B
    I got results with [A] starting off at 0,5 0,375 0.335 0,355... nearing the correct answer 0,35.

    Still it amazes me what this makes this reaction different from plain A<->2B+C

    Thank you, now I am able to perform this calculation from now on.
     
  7. Dec 10, 2012 #6

    Borek

    User Avatar

    Staff: Mentor

    Have you tried to correctly balance this reaction?
     
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