Percent Yield and Stoichiometry Concepts

In this AP Chemistry video, Jeremy Krug discusses percent yield, explaining how it is calculated by dividing the actual yield by the theoretical yield and multiplying by 100. He highlights the difference between actual and theoretical yields, noting that actual yield is often less due to side reactions. The video includes examples of calculating percent yield, both simple and advanced, and demonstrates using stoichiometry to determine theoretical yield. The video concludes with a call to action for viewers to engage with the content.

What is the percent yield if the actual yield is 10 grams and the theoretical yield is 12 grams?

• 12%

• 10%

• 120%

• 83.33%

Which of the following is NOT a reason for actual yield being less than theoretical yield?

• Loss of product during transfer

• Side reactions

• Measurement errors

• Complete reaction

In the example problem, what was the percent yield when 14.08 grams were collected, but 16.37 grams were expected?

• 86.01%

• 72.0%

• 14.08%

• 100%

If a process has a 72% yield and you want to produce 10 grams, what should be the theoretical yield?

• 72 grams

• 10 grams

• 7.2 grams

• 13.9 grams

What is the first step in solving a stoichiometry problem to find theoretical yield?

• Measure actual yield

• Convert grams to moles

• Balance the chemical equation

• Calculate percent yield

In the stoichiometry example, what was the theoretical yield of calcium hydroxide?

• 74.10 grams

• 7.76 grams

• 9.24 grams

• 5 grams

What is the percent yield if the actual yield is 7.76 grams and the theoretical yield is 9.24 grams?

• 72.0%

• 100%

• 84.0%

• 7.76%

Which of the following is a step in calculating percent yield?

• Divide actual yield by theoretical yield

• Add actual yield to theoretical yield

• Multiply theoretical yield by 100

• Subtract actual yield from theoretical yield

What is the purpose of balancing a chemical equation in stoichiometry?

• To ensure mass conservation

• To increase reaction speed

• To reduce side reactions

• To maximize percent yield

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