Stoichiometry
Enter the reaction and what you weighed or measured out. The equation is balanced for you, and the table shows the limiting reagent, what is left over and the theoretical and percent yield.
Reaction
Reaction table
match a compound to fill in its density| Reactants | M (g/mol) | Amount | Density | n | Mass | Equiv | Status |
|---|---|---|---|---|---|---|---|
| C7H6O3 | 138.12 | g/mL | 14.48 mmol | 2.000 g | 1.00 | Limiting reagent | |
| C4H6O3 | 102.09 | g/mL | 52.90 mmol | 5.400 g | 3.65 | 38.42 mmol left over3.922 g | |
| Products | M (g/mol) | Actual yield | n, theoretical | Theoretical yield | Yield | ||
| C9H8O4 | 180.16 | 14.48 mmol | 2.609 g | 80.5 % yield | |||
| C2H4O2 | 60.05 | 14.48 mmol | 869.6 mg |
How the table is worked out
The reaction is balanced first, with the same exact method as the equation balancer. Every amount you enter is turned into moles: a mass through the molar mass, a volume through the density and then the molar mass. Dividing each reactant's moles by its coefficient gives how often the reaction could run on that reactant alone; the smallest of these is the extent of reaction, and the reactant that sets it is the limiting reagent.
Equivalents are moles relative to the limiting reagent, as in a lab notebook. Each product forms its coefficient times the extent: that is the theoretical yield, and the percent yield is the actual yield over it. A reactant without an amount is taken to be in excess, and the table shows how much of it the limiting reagent needs.
Where the numbers come from
Molar masses use the IUPAC 2021 standard atomic weights (Pure Appl. Chem. 94, 573, 2022). Densities come from the compound's entry in the Chempirical catalogue when you match a compound, and you can overwrite them; they are room-temperature values for the pure substance, so for solutions enter the amount in moles instead.