Practice Theoretical Yield, Actual Yield, And Percent Yield (1.3.2) - Unit 1: Stoichiometric Relationships

Practice: Theoretical Yield, Actual Yield, and Percent Yield

Lesson 1.3.2Unit 1: Stoichiometric Relationships

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6 sample questions

Question 1.
Define theoretical yield in your own words.
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Think about how yield connects to reactants.
Question 2.
What typically causes the actual yield to be less than theoretical yield?
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Consider laboratory practices.
3Question 3.
What is the theoretical yield?
- The amount actually produced
- The maximum possible amount
- The yield in a given reaction
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Think about the ideal chemical reactions.
4Question 4.
If actual yield is 25 g and theoretical yield is 40 g, what is the percent yield?
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Remember the percent yield formula.
Question 5.
In an experiment to synthesize magnesium oxide, it was determined that 20 g of magnesium reacts with oxygen to produce 30 g of magnesium oxide. What is the theoretical yield if 10 g of magnesium were used?
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Use stoichiometry based on the balanced equation for magnesium and oxygen.
Question 6.
If the theoretical yield of a reaction is 100 g and the actual yield is 50 g, what factors could explain why the actual yield is 50%?
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Think about practical lab scenarios.

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