Percent Yield in Chemical Reactions
A Grade 12 Chemistry worksheet on calculating and understanding percent yield in chemical reactions.
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Percent Yield in Chemical Reactions
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Read each question carefully and answer to the best of your ability. Show all calculations where necessary.
The percent yield is a measure of the efficiency of a chemical reaction. It is the ratio of the actual yield (the amount of product actually obtained) to the theoretical yield (the maximum amount of product that could be formed from the given amounts of reactants), expressed as a percentage.
1. Which of the following statements best defines theoretical yield?
The amount of product actually obtained from a reaction.
The maximum amount of product that can be formed from the given amounts of reactants.
The amount of reactant consumed in a reaction.
The percentage of product obtained compared to the reactant.
2. A percent yield of 100% indicates:
No product was formed.
The actual yield was greater than the theoretical yield.
The actual yield equals the theoretical yield.
The reaction was incomplete.
3. The formula for percent yield is ( ) / (Theoretical Yield) x 100%.
4. Impurities in reactants or side reactions can lead to a actual yield.
5. In a reaction, 10.0 g of a reactant produces 8.5 g of product. If the theoretical yield for this reaction is 9.2 g, calculate the percent yield.
6. A chemist performs a synthesis and obtains 15.0 g of product. If the calculated theoretical yield was 18.5 g, what is the percent yield of this reaction?
7. A percent yield greater than 100% is possible due to experimental error or impurities.
True
False
8. Discuss at least three factors that can cause the actual yield of a reaction to be less than the theoretical yield.
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