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?