Solution Found!
Answer: Ethylene (C2H4), an important industrial organic
Chapter 3, Problem 92P(choose chapter or problem)
Ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\), an important industrial organic chemical, can be prepared by heating hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)\) at \(800^{\circ} \mathrm{C}\):
\(\mathrm{C}_{6} \mathrm{H}_{14} \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}+\) other products
If the yield of ethylene production is 42.5 percent, what mass of hexane must be reacted to produce 481 g of ethylene?
Questions & Answers
QUESTION:
Ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\), an important industrial organic chemical, can be prepared by heating hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)\) at \(800^{\circ} \mathrm{C}\):
\(\mathrm{C}_{6} \mathrm{H}_{14} \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}+\) other products
If the yield of ethylene production is 42.5 percent, what mass of hexane must be reacted to produce 481 g of ethylene?
ANSWER:Step 1 of 2
Here we have to calculate mass of hexane required to produce 481 g of ethylene.
The given chemical reaction is,
+ other product
Yield of ethylene = 42.5 %
Mass of ethylene = 481 g
It is known that, the % yield can be calculated as,
% yield = 
100 %
We can write this equation as,
42.5 % yield = 
100 %
Theoretical yield = 481
