Percentage Yield Worksheet
A Grade 10 Chemistry worksheet covering percentage yield calculations, theoretical yield, actual yield, and factors affecting yield.
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Percentage Yield Worksheet
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Read each question carefully and answer to the best of your ability. Show all your work for calculation questions.
1. Which of the following best defines theoretical yield?
The amount of product obtained from a reaction.
The maximum amount of product that can be formed from given amounts of reactants.
The percentage of product obtained compared to the expected amount.
The amount of reactant consumed in a reaction.
2. Why is the actual yield almost always less than the theoretical yield?
Reactants are always impure.
Some product is lost during transfer or purification.
The reaction produces more than one product.
The limiting reactant is consumed too quickly.
3. The formula for calculating percentage yield is ( / ) x 100%.
4. A reaction that does not go to completion will result in a actual yield.
5. Side reactions occurring during a chemical process can the percentage yield.
6. In a chemical reaction, 25.0 g of product was theoretically expected, but only 20.0 g was actually collected. Calculate the percentage yield for this reaction.
7. Consider the reaction: 2Al (s) + 3Cl₂ (g) → 2AlCl₃ (s). If 5.0 g of aluminum reacts completely and produces 15.0 g of aluminum chloride, what is the percentage yield? (Molar mass of Al = 26.98 g/mol, AlCl₃ = 133.34 g/mol)
8. A percentage yield greater than 100% is impossible under any circumstances.
True
False
9. Impurities in the reactants can lead to a lower actual yield.
True
False
10. A student performed an experiment to synthesize aspirin. They calculated a theoretical yield of 10.0 g, but after purification, they obtained 11.5 g of aspirin. Explain two possible reasons why their percentage yield was greater than 100%.
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