Percentage Yield Flashcards
Define yield
The amount of product you get from a reaction
State the formula for percentage yield
actual yield/theoretical yield x 100
Define theoretical yield
Mass of product you’d make if all the reactants were converted to products
What has happened if a reaction has a low percentage yield?
A lot of reactants have been wasted
Why is it important to use reactions with the highest yield possible?
Reduce waste
Keep costs down
Explain 3 reasons you won’t get a 100% yield
Incomplete reactions
- not all reactants were converted to product
Practical losses
- you’ll lose some when transferring chemicals between containers
Unwanted reactions
- if unexpected reactions happen, the yield of the intended product goes down. This can be because of impurities in reactions or changes to reaction conditions
