Quantitative Chemistry: Percentage Yield
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What is the theoretical yield?
The volume of products you would get in theory if you were to calculate it.
What is actual yield?
The volume of products you actually get
How do you calculate percentage yield?
Actual yield _____________ x 100 Theoretical yield
What are the 3 main reasons for a lower actual yield?
• Reactants may not all react If the reaction is slow then it may not have finished or if it‘s reversible then it ma have reached equilibrium. • Side reactions may have taken place Reactants could’ve produced a different product to the expected one each they could’ve reacted to oxygen in the air • Some of the product may have been lost in the process eg. gaseous products may escape and float away
For the balanced equation shown below, if the reaction of 40.8 grams of C6H6O3 produces a 39.0% yield, how many grams of H2O would be produced ? C6H6O3 +6O2 → 6CO2 + 3H2O
actual yield = 6.83 grams
What is the percentage yield of NH3 if 40.5g of NH3 is produced from 20.0mol H2 and excess N2
• Write the balanced equation • Calculate the theoretical amount of NH3 • Calculate the percentage yield of NH3 40.5/227 x 100 = 17.8%