Percent Yield Lesson

Drag and Drop

The ​

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is the ratio between the

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, which is measured directly from the lab, and the

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, which is calculated from the reactants. It is represented as a percentage.

Drag these tiles and drop them in the correct blank above

percent yield

actual yield

theoretical yield

molar mass

mole ratio

Multiple Choice

Four students were tasked with running an experiment in which they needed to produce hydrogen gas from the following reaction. Which student had the worst efficiency?

$$Zn\left(s\right)\ +\ 2\ HCl\left(aq\right)\ \rightarrow\ ZnCl_2\left(aq\right)\ +\ H_2\left(g\right)$$

• Student 1 had an 84.2% yield.

• Student 2 had an 89.1% yield.

• Student 3 had an 89.7% yield.

• Student 4 had an 86.5% yield.

Math Response

The theoretical yield of ammonia produced when hydrogen and nitrogen react is 46.4 g. During a lab, only 39.1 g was produced. What is the percent yield of the ammonia?

Percent Yield: _____%

Type answer here

Correct Answer: 84.3

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First things first, you need to write a balanced chemical equation.

​

Balanced Chemical Equation

1. ​Write a word equation.

2. Write the chemical formulas for the reactants and the products.

3. Balance.

Fill in the Blanks

What are the coefficients for the balanced chemical equation for the given problem?

A mass of 26.5 g of ammonia was produced when 7.00 g of hydrogen was reacted with excess nitrogen. What is the percent yield of ammonia produced?

Fill in the Blanks

3 H₂(g) + N₂(g) → 2 NH₃(g)

A mass of 26.5 g of ammonia was produced when 7.00 g of hydrogen was reacted with excess nitrogen. What is the theoretical yield?

Math Response

3 H₂(g) + N₂(g) → 2 NH₃(g)

A mass of 26.5 g of ammonia was produced when 7.00 g of hydrogen was reacted with excess nitrogen. What is the percent yield?

Percent Yield: ____ %

Type answer here

Correct Answer: 67.3

Deg^°

Rad