Actual Yield Calculator

Calculate actual product yield from theoretical yield and percent yield for chemistry experiments.

Calculate actual yield

Enter theoretical yield in grams and the measured or expected percentage yield.

Theoretical yield (g)

Percent yield (%)

About actual yield

Actual yield is the quantity of product recovered from a chemical reaction or manufacturing process. It is measured after the reaction, separation, purification, and drying steps are complete. Theoretical yield is different: it is the greatest product amount predicted by stoichiometry when the limiting reactant reacts completely and no material is lost. Percent yield compares these two amounts and provides a compact measure of how closely an experiment approached its theoretical maximum. This calculator rearranges the standard percent-yield relationship. Actual yield equals theoretical yield multiplied by percent yield and divided by 100. For example, a theoretical yield of 50 grams with an 80 percent yield corresponds to 40 grams actually recovered. Both yields must use the same mass unit for the percentage relationship to remain meaningful. This page labels the result in grams, so convert milligrams, kilograms, or moles before entry if your work uses a different basis. Several factors can make actual yield lower than theoretical yield. A reaction may not proceed to completion, competing reactions may consume reactants, equilibrium may favor reactants, and product can remain in glassware or be lost during filtration and transfer. Impurities, measurement uncertainty, and incomplete drying can also affect the observed mass. An apparent yield above 100 percent often signals residual solvent, contamination, an incorrect limiting-reactant calculation, or a mismatch in units rather than unusually successful chemistry. Before using the calculator, determine theoretical yield from the balanced equation and limiting reactant. Then use an experimentally measured percent yield or a realistic expected percentage for planning. The output can help estimate how much isolated product a synthesis may deliver, size downstream operations, or check a laboratory report. It does not calculate stoichiometry or identify the limiting reactant itself. Report the result with suitable significant figures, and retain enough unrounded precision during intermediate work to avoid introducing avoidable error.

Actual yield examples

Theoretical and actual yield use the same mass basis in each example.

Theoretical and percent yield	Actual yield	Context
50 g theoretical at 80%	40 g	A common teaching-lab example.
12.5 g theoretical at 72%	9 g	A moderate isolated yield.
250 g theoretical at 92.5%	231.25 g	A high-yield process estimate.

How to calculate actual yield

Calculate the theoretical yield from the limiting reactant and balanced equation.
Enter the theoretical product mass in grams.
Enter the percent yield measured or expected for the reaction.
Select Calculate Actual Yield and round the result to suitable significant figures.

Actual yield FAQ

How is actual yield different from theoretical yield?

Theoretical yield is the maximum amount predicted by stoichiometry. Actual yield is the amount of product physically recovered from the experiment.

Can percent yield exceed 100 percent?

A reported value above 100 percent is mathematically possible but normally indicates wet product, impurities, measurement error, or incorrect stoichiometry. Investigate the procedure before treating it as a valid reaction yield.

Must both yields use grams?

The percent-yield ratio works with any matching units. This calculator reports grams, so convert both the theoretical basis and desired result consistently before using it.

How do I find theoretical yield?

Balance the reaction, identify the limiting reactant, and convert its available moles to product moles using the stoichiometric ratio. Then multiply by the product's molar mass to obtain a theoretical mass.

Why is actual yield usually lower?

Reactions can be incomplete or produce side products, and product can be lost during handling and purification. These practical effects reduce the isolated amount relative to the ideal prediction.