Chemistry · Stoichiometry

Limiting Reagent and Percent Yield Explorer

Choose a reaction and set the mass of each reactant. The page converts masses to moles, finds which reactant runs out first, and shows the particle picture before and after the reaction.

Then set the percent yield of your procedure to see actual yield against theoretical yield. The graph shows why adding more of the excess reactant does not make more product. Record points to build your own table.

Model notes

Molar masses (g/mol) are from standard atomic weights: H 1.008, C 12.011, N 14.007, O 15.999, Na 22.990, Cl 35.45. Calculations carry full precision and display three or four significant figures.
Each icon stands for the amount shown in the key. Icon counts are rounded, so the particle picture matches the mole ratio only approximately. The numbers in the tiles and the readout are exact.
Percent yield is applied to the main product only, as is usual in classroom problems. The first product listed is the main product.
Treat the reactions as ideal and complete: the limiting reactant is fully used up. Real reactions such as ammonia synthesis reach equilibrium and never use up a reactant entirely.

Sources

View the code