Theoretical Yield Calculator
ChemistryCalculate the theoretical yield of a chemical reaction from moles of limiting reagent and stoichiometric ratio. Find the maximum mass of product that can be formed.
0.1 mol
mol
1
180.16 g/mol
g/mol
Theoretical Yield (g)
18.016
Theoretical Yield (mol)
0.1
Theoretical Yield (mg)
18,016
What is a Theoretical Yield?
The Theoretical Yield Calculator computes the maximum mass of product that a chemical reaction can produce from a given quantity of the limiting reagent. Theoretical yield is the stoichiometric ceiling — the gram quantity you would recover if the reaction went to perfect completion with no losses, no side reactions, and no isolation waste.
The calculation bridges moles and grams through three inputs: how many moles of the limiting reagent you start with, the molar ratio (product-to-reagent coefficient from the balanced equation), and the molar mass of the product. The result — the theoretical yield in grams — is then compared against the actual yield you recover in the lab to compute the percent yield, which measures reaction efficiency.
Identifying the correct limiting reagent is the most critical step before using this calculator. When two reagents are present in unequal molar amounts relative to their stoichiometric coefficients, only the limiting reagent determines how much product can form. The Mole Calculator helps convert starting masses to moles, and the Molar Ratio Calculator handles the stoichiometric ratio step if you need to compare multiple reactants.
Once the theoretical yield is known, the Percent Yield Calculator shows how your actual recovered product compares to this maximum, and the Actual Yield Calculator estimates how much product to expect in a planned synthesis given a known typical yield efficiency.
How to use this Theoretical Yield calculator
- Balance your chemical equation and identify the limiting reagent (the reactant present in the fewest moles relative to its stoichiometric coefficient).
- Convert the mass of the limiting reagent to moles using the Mole Calculator if needed (moles = mass ÷ molar mass). Enter the result in the Moles of Limiting Reagent field.
- From the balanced equation, divide the stoichiometric coefficient of the product by the stoichiometric coefficient of the limiting reagent. Enter this ratio in the Molar Ratio (product : reagent) field. For a 1:1 reaction, enter 1.
- Enter the molar mass of the product in g/mol in the Molar Mass of Product field. Use the Molecular Weight Calculator if you need to compute this from the molecular formula.
- Read the Theoretical Yield (g) — this is the maximum mass of product stoichiometry permits. Note the milligrams value if working at small scale.
- Use this theoretical yield as input to the Percent Yield Calculator after you complete the reaction and weigh the recovered product.
Formula & Methodology
Core formula:Theoretical Yield (mol) = Moles of Limiting Reagent × Stoichiometric Ratio Theoretical Yield (g) = Theoretical Yield (mol) × Molar Mass of Product (g/mol) Theoretical Yield (mg) = Theoretical Yield (g) × 1000Stoichiometric ratio:Stoichiometric Ratio = Coefficient of Product ÷ Coefficient of Limiting ReagentWorked example — synthesis of iron(III) oxide: Balanced equation: 4 Fe + 3 O₂ → 2 Fe₂O₃ Starting material: 10.0 g of iron (Fe), molar mass = 55.845 g/mol Product: Fe₂O₃, molar mass = 159.69 g/molStep 1 — Moles of Fe: mol(Fe) = 10.0 / 55.845 = 0.17907 mol Step 2 — Stoichiometric ratio (Fe₂O₃ : Fe): Ratio = 2 / 4 = 0.5 Step 3 — Theoretical yield: mol(Fe₂O₃) = 0.17907 × 0.5 = 0.08953 mol mass(Fe₂O₃) = 0.08953 × 159.69 = 14.30 gIf the experiment recovers 11.2 g of Fe₂O₃, the percent yield is (11.2 / 14.30) × 100 = 78.3%.
Frequently Asked Questions
Theoretical yield is the maximum amount of product that can be formed from a given amount of limiting reagent in a chemical reaction, assuming the reaction goes to 100% completion with no side reactions or losses. It is calculated entirely from stoichiometry — the balanced chemical equation and the moles of the limiting reagent. Theoretical yield sets the upper ceiling against which the actual yield is compared to calculate percent yield.
Theoretical Yield (g) = Moles of Limiting Reagent × Stoichiometric Ratio × Molar Mass of Product. The stoichiometric ratio is the coefficient of the product divided by the coefficient of the limiting reagent in the balanced equation. For example, if 2 mol of reactant A produces 3 mol of product B, the stoichiometric ratio is 3 ÷ 2 = 1.5.
The limiting reagent is the reactant that runs out first and thus limits the amount of product formed. To identify it: (1) convert all reactant quantities to moles; (2) divide each by its stoichiometric coefficient from the balanced equation; (3) the reactant with the smallest result is the limiting reagent. Only the limiting reagent enters the theoretical yield formula — excess reagents are irrelevant.
Theoretical yield is the calculated maximum from stoichiometry; actual yield is the mass of product you physically recover after the reaction and purification. Actual yield is always less than theoretical yield due to incomplete reaction, side reactions, and product losses during isolation. The ratio of actual to theoretical, expressed as a percentage, is the percent yield — calculated with the [Percent Yield Calculator](/percent-yield-calculator/).
Theoretical yield is a stoichiometric ideal — a benchmark computed from conservation of mass and the balanced equation. Real reactions may not go to completion (especially reversible equilibrium reactions), reactants may be diverted into side reactions, and product isolation always involves some loss. These deviations are captured by percent yield. Theoretical yield must assume 100% completion to serve as a fixed, unambiguous reference point.
No. By definition, theoretical yield is the maximum; exceeding it would violate conservation of mass. A measured actual yield above the theoretical yield always indicates a calculation error or contamination — the product was not fully purified (solvent or impurities adding mass), the theoretical yield was computed incorrectly, or weighing errors occurred. Check your moles, stoichiometric ratio, and molar mass when a calculated percent yield exceeds 100%.
Molar mass (g/mol) is the conversion factor between moles of product and grams of product — the only step where units change from moles to grams. A product with a high molar mass produces more grams per mole than a light product. For example, 0.1 mol of glucose (M = 180.16 g/mol) gives a theoretical yield of 18.016 g, while 0.1 mol of water (M = 18.015 g/mol) gives only 1.8015 g. Use the [Molecular Weight Calculator](/molecular-weight-calculator/) if you need to compute molar mass from the molecular formula.
Enter the moles of the limiting reagent in the 'Moles of Limiting Reagent' field. Enter the stoichiometric ratio (product coefficient ÷ reagent coefficient from the balanced equation) in the 'Molar Ratio' field — enter 1 if both coefficients are equal. Enter the molar mass of the product in g/mol. The calculator returns the theoretical yield in grams, moles, and milligrams.
Theoretical yield is the starting point for every yield calculation in industrial process chemistry, pharmaceutical API manufacturing, and batch chemical production. It determines raw material requirements — if a batch requires 100 kg of product at 80% expected yield, you must plan for a theoretical yield of 125 kg and source enough limiting reagent to produce it. Under WHO-GMP and Schedule M, theoretical yield per batch is documented in the Master Manufacturing Record.
The Theoretical Yield Calculator returns the result in grams, moles, and milligrams simultaneously. To convert manually: multiply the gram result by 1,000 (1 g = 1,000 mg). This is useful for small-scale research syntheses where product masses are in the tens to hundreds of milligrams range, such as catalyst testing or medicinal chemistry hit-compound preparation.
Enter 1 as the stoichiometric ratio. A 1:1 ratio means one mole of limiting reagent produces exactly one mole of product — common for simple displacement and precipitation reactions. The moles of product equal the moles of reagent, and the theoretical yield in grams is simply moles × molar mass. If both coefficients are the same but not 1 (e.g., 2A → 2B), the ratio is still 2 ÷ 2 = 1.