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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?