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ChemBench
The best-case output of a reaction.
Theoretical yield converts the limiting reactant's moles into moles of product (using the balanced equation's coefficient ratio), then multiplies by the product's molar mass to get an answer in grams.
No real reaction exceeds its theoretical yield — it's the benchmark used to calculate percent yield and judge how efficient an actual lab or industrial run was.
Molar mass of any chemical formula (e.g. H2O, C6H12O6, Ca(OH)2).
OpenPercent composition of an element within a chemical formula.
OpenSimplest whole-number ratio formula from elemental masses or percentages.
OpenPercent yield from actual and theoretical reaction yields.
OpenTheoretical yield
36 g
What you entered
Moles of product = (limiting moles ÷ reactant coeff) × product coeff
(2 ÷ 1) × 1= 2Theoretical yield = moles × molar mass
2 × 18= 36 gResult
Theoretical yield: 36 g
The maximum possible yield from this reaction is 36g of product.