List several reasons why the actual yield from a chemical reaction is not usually equal to the theoretical yield.
Added by Penny S.
Step 1
Step 1: Recognize that the theoretical yield is calculated from the balanced equation based on the assumption that all of the limiting reactant is converted completely and exclusively into the desired product. Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 81 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Give two reasons why the actual yield from a chemical reaction is usually less than the theoretical yield.
Why is the actual yield of a reaction often less than the theoretical yield?
Define the terms theoretical yield, actual yield, and percent yield. (b) Why is the actual yield in a reaction almost always less than the theoretical yield?(c) Can a reaction ever have 110$\%$ actual yield?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD