How Do You Calculate Percent Yield of C2H5Cl in a Complex Reaction?

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To calculate the percent yield of C2H5Cl from the reaction of ethane and chlorine, the theoretical yield is determined based on the balanced equation, which simplifies the process by focusing on the main product. The presence of minor products like C2H4Cl2 and C2H3Cl3 does not affect the calculation of percent yield, as the theoretical yield assumes only one primary product. The calculated percent yield of C2H5Cl is 82.9%, despite the formation of other products. Theoretical yield calculations are valid as long as the main product is clearly defined, and the amounts of byproducts do not require additional reactants. Thus, the balancing of the reaction can accommodate multiple products without altering the yield of the primary product.
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Homework Statement




"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)

Homework Equations



Balancing and math principles.

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

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