Percent Yield Examples in Chemistry
Start with the recap, study the fully worked examples, then use the practice problems to check your understanding of Percent Yield.
This page combines explanation, solved examples, and follow-up practice so you can move from recognition to confident problem-solving in Chemistry.
Concept Recap
The ratio of the actual yield obtained in an experiment to the theoretical yield predicted by stoichiometry, expressed as a percentage. It measures how efficient a chemical reaction was in practice.
How much of the possible product you actually got — 100% is perfect, real reactions are always less.
Read the full concept explanation →How to Use These Examples
- Read the first worked example with the solution open so the structure is clear.
- Try the practice problems before revealing each solution.
- Use the related concepts and background knowledge badges if you feel stuck.
What to Focus On
Core idea: Percent yield measures how efficient a reaction was compared to the ideal stoichiometric outcome.
Common stuck point: Percent yield over 100% usually means impurities or measurement error.
Sense of Study hint: When calculating percent yield, you need both actual and theoretical yields. First calculate the theoretical yield using stoichiometry from the limiting reactant. Then obtain the actual yield from the experiment. Finally, divide actual by theoretical and multiply by 100%.
Worked Examples
Example 1
easySolution
- 1 Start with the percent-yield formula: \%\text{yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100\%.
- 2 Substitute the given masses: \%\text{yield} = \frac{42.0}{50.0} \times 100\%.
- 3 Compute the ratio and convert to a percent: \%\text{yield} = 84.0\%.
Answer
Example 2
hardPractice Problems
Try these problems on your own first, then open the solution to compare your method.
Example 1
easyExample 2
easyRelated Concepts
Background Knowledge
These ideas may be useful before you work through the harder examples.