1. Limited time only! Sign up for a free 30min personal tutor trial with Chegg Tutors
    Dismiss Notice
Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Homework Help: Balancing Chemical equations

  1. Sep 14, 2013 #1
    1. The problem statement, all variables and given/known data

    "The reaction of ethane gas (C2H6) with chlorine gas produces C2H5Cl as its main product (along with HCl). In addition, the reaction invariably produces a variety of other minor products, including C2H4Cl2, C2H3Cl3, and others. Naturally, the pro- duction of these minor products reduces the yield of the main product. Calculate the percent yield of C2H5Cl if the reaction of 300. g of ethane with 650. g of chlorine produced 490. g of C2H5Cl." (Zumdahl, Chemistry, 2013)

    2. Relevant equations

    Balancing and math principles.

    3. The attempt at a solution

    Ok, I have the answer in the solution manual. It gives out 82.9%.
    But, the thing I do not understand about the way they do the problem is this:
    They use the formula C2H6+ Cl2-> C2H5Cl+ HCl
    However, that's not what is really happening. There are other products formed.
    I thought of this formula (which is missing ''the other'' products):
    C2H6+ Cl2-> C2H5Cl+ HCl +C2H4Cl2+C2H3Cl3 + others
    I found different ways of balancing this last formula if I ignore the others.

    Why does the first equation give the right answer? Won't the other molecules intervene in the calculations?
  2. jcsd
  3. Sep 14, 2013 #2


    User Avatar
    Science Advisor
    Homework Helper
    Gold Member

    No, they don't. You can't be certain the other products were produced anyway. The other "products" COULD be unreacted starting material!
  4. Sep 14, 2013 #3
    But, there still may be other products. I don't understand how those cannot have an impact on the reaction balancing.
  5. Sep 14, 2013 #4


    User Avatar

    Staff: Mentor

    Theoretical yield assumes only one product.

    Note that in this particular case you can't uniquely balance reaction with several products. Each of these:

    2C2H6 + 3Cl2 -> C2H5Cl + C2H4Cl2 + 3HCl

    50C2H6 + 67Cl2 -> 33C2H5Cl + 17C2H4Cl2 + 67HCl

    1028C2H6 + 1119Cl2 -> 937C2H5Cl + 91C2H4Cl2 + 1119HCl

    is balanced OK. Which one of these is the correct one?
  6. Sep 14, 2013 #5
    All of them could be correct i guess. Hmm, you are intriguing me here. Theoretical yield applies only when there is one product? What about the HCl?
  7. Sep 14, 2013 #6


    User Avatar

    Staff: Mentor

    Sorry, lousy wording, one main product. HCl doesn't matter, as its amount is related to the main product - you don't need more ethane to produce HCl.
Share this great discussion with others via Reddit, Google+, Twitter, or Facebook

Have something to add?
Draft saved Draft deleted