Practice Percent Yield in Chemistry
Use these practice problems to test your method after reviewing the concept explanation and worked examples.
Quick 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.
Example 1
easyA reaction has a theoretical yield of 50.0 g but only 42.0 g of product is obtained. Calculate the percent yield.
Example 2
hardIn the reaction 2\text{Al} + 3\text{Cl}_2 \rightarrow 2\text{AlCl}_3, 10.0 g of Al reacts with excess \text{Cl}_2 to produce 40.0 g of \text{AlCl}_3. Calculate the percent yield.
Example 3
easyIf the theoretical yield is 25.0 g and the percent yield is 90.0\%, what is the actual yield?
Example 4
easyA reaction has a theoretical yield of 18.5 g and a percent yield of 92.0\%. What actual mass of product was collected?