We’re being asked to calculate the theoretical yield of C2H5Cl when 121 g of C2H6 reacts with 226 g of Cl2 to form only C2H5Cl and HCl.
For this problem, we need to do the following steps:
Step 1: Write and balance a chemical equation for the given reaction.
Step 2: Determine the limiting reactant and calculate the theoretical yield of C2H5Cl formed.
Step 1: From the problem, the given chemical reaction is:
C2H6 + Cl2 → C2H5Cl + HCl
This equation is already balanced. The number of elements on both sides are equal.
Now that we have a balanced equation, we can determine the theoretical yield of C2H5Cl.
When ethane (C2H6) reacts with chlorine (Cl2), the main product is C2H5Cl; but other products containing Cl, such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl.
Calculate the theoretical yield of C2H5Cl when 121 g of C2H6 reacts with 226 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.