Percentage Yield - Topic 5
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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 in the time Practical losses - some reactants or products were left behind in containers or on apparatus when transferred between them Unwanted reactions - impurities in reactants or changes to reaction conditions