Percent Yield Chemistry Example 4

Follow the full solution, then compare it with the other examples linked below.

Example 4

easy

A reaction has a theoretical yield of

18.5

g and a percent yield of

92.0\%

. What actual mass of product was collected?

Solution

1
Use $\text{percent yield} = \frac{\text{actual}}{\text{theoretical}} \times 100\%$ .
2
So actual yield $= 0.920 \times 18.5 = 17.0\,\text{g}$ .

Answer

17.0\,\text{g}

Percent yield compares what was actually collected with the ideal theoretical amount. Multiply the theoretical yield by the decimal percent to find the actual yield.

About Percent Yield

The ratio of the actual yield obtained in an experiment to the theoretical yield predicted by stoichiometry, expressed as a percentage.

Learn more about Percent Yield →

More Percent Yield Examples

Example 1 easy

A reaction has a theoretical yield of [formula] g but only [formula] g of product is obtained. Calcu

Example 2 hard

In the reaction [formula], [formula] g of Al reacts with excess [formula] to produce [formula] g of

Example 3 easy

If the theoretical yield is [formula] g and the percent yield is [formula], what is the actual yield

← All Percent Yield Examples Percent Yield Concept

Related Concepts

Theoretical Yield