Last updated: July 3, 2026
Actual Yield Calculator
Creators
Dharmendra SinghReviewers
Creators
Dharmendra SinghReviewers
Quick Answer
Actual yield is the product amount recovered from a reaction. To calculate it, multiply theoretical yield by percent yield divided by 100. For example, a 50 g theoretical yield at 90% gives 45 g actual yield. The equation can also be rearranged to find percent yield or theoretical yield when the other two quantities are known.
Actual yield equals percent yield divided by one hundred times theoretical yield. For a theoretical yield of 50 grams at 90 percent yield, the actual yield is 45 grams.
Key Takeaways
- Actual yield = (percent yield / 100) × theoretical yield.
- Use matching units for actual and theoretical yield, such as grams with grams or moles with moles.
- Percent yield = (actual yield / theoretical yield) × 100 when both amounts are known.
- A true pure-product yield above 100% usually indicates wet product, impurities, or a calculation error.
- Theoretical yield comes from limiting-reagent stoichiometry; actual yield comes from recovered product.
Creators
Dharmendra SinghReviewers
Creators
Dharmendra SinghReviewers
Formula
actual yield = (percent yield / 100) × theoretical yield; percent yield = (actual yield / theoretical yield) × 100
Where:
- Yactual=Actual yield obtained in the experiment(g or mol)
- Ytheoretical=Maximum yield predicted by stoichiometry(g or mol)
- %Y=Percent yield of the reaction(%)
Worked Examples
Find actual yield from a 90% reaction
A synthesis can produce at most 50 g by stoichiometry, and the isolated percent yield is 90%.
- 1Start with actual yield = (percent yield / 100) × theoretical yield.
- 2Substitute the values: actual yield = (90 / 100) × 50 g.
- 3Compute 0.90 × 50 g = 45 g.
- 4A 90% yield is commonly interpreted as a good isolated yield.
Actual yield at 80% recovery
Only 80% of a 25 g theoretical product amount is obtained after workup.
- 1Use actual yield = (% yield / 100) × theoretical yield.
- 2Substitute: actual yield = (80 / 100) × 25 g.
- 3Multiply: 0.80 × 25 g = 20 g.
- 4The obtained product mass is therefore 20 g.
Check percent yield from actual product
A reaction gives 18 g of product when stoichiometry predicts 20 g.
- 1Use percent yield = (actual yield / theoretical yield) × 100.
- 2Substitute: percent yield = (18 g / 20 g) × 100.
- 3Calculate 0.90 × 100 = 90%.
- 4The result confirms a good 90% yield.
Complete conversion to the theoretical amount
A reaction with 100 g theoretical yield and 100% yield should return the full theoretical mass.
- 1Use actual yield = (100 / 100) × 100 g.
- 2The factor is 1.00.
- 3Actual yield = 100 g.
- 4This represents quantitative recovery under the assumptions of the problem.
Recover the theoretical yield from actual mass
An experiment isolated 45 g, and the known percent yield was 90%.
- 1Rearrange the equation: theoretical yield = actual yield / (percent yield / 100).
- 2Substitute: theoretical yield = 45 g / (90 / 100).
- 3Calculate 45 g / 0.90 = 50 g.
- 4The stoichiometric maximum was 50 g.
Introduction
The actual yield is the amount of product you really collect from a chemical reaction after separation, washing, drying, and weighing. Stoichiometry predicts a maximum called the theoretical yield, but real reactions lose material through incomplete conversion, side reactions, transfer losses, impurities, and workup. This actual yield calculator centers on the practical question, how much product should I expect to obtain? Enter the theoretical yield from your balanced equation and the percent yield to compute the actual mass or amount. You can also rearrange the same relation to check percent yield or recover the theoretical yield.
Actual yield formula
The core equation is percent yield = (actual yield / theoretical yield) × 100. Solving for the product amount gives actual yield = (percent yield / 100) × theoretical yield. If a balanced-equation calculation predicts 50 g of product and the reaction runs at 90% yield, the actual yield is 0.90 × 50 g = 45 g. Use the molar mass calculator first when your stoichiometry begins with a chemical formula and gram-to-mole conversion.
Actual yield is measured or predicted product recovered, not the maximum possible amount.
Percent yield is a ratio, so convert it to a decimal by dividing by 100 before multiplying.
Theoretical and actual yield must use the same unit: both grams, both moles, or another consistent amount unit.
Round the final answer to match the meaningful precision of your measured masses.
How to calculate actual yield step by step
First, determine the theoretical yield from stoichiometry. That typically means balancing the equation, converting reactant masses to moles, applying the mole ratio, identifying the limiting reagent, and converting product moles back to grams. Then multiply that theoretical yield by the expected percent yield as a decimal. For example, 80% of 25 g is (80/100) × 25 g = 20 g. If you need solution concentration after weighing product, the molarity calculator connects product amount with final solution volume.
Keep extra digits during stoichiometry and round only after the actual yield calculation.
Rearranging for percent or theoretical yield
Although this tool focuses on actual yield, the same equation can be rearranged for common lab checks. If you know actual and theoretical yield, percent yield = (actual/theoretical) × 100. If you know actual yield and percent yield, theoretical yield = actual/(percent/100). These rearrangements are useful for auditing notebook data and comparing runs. The formal definition of yield is consistent with standard stoichiometric usage described in IUPAC terminology and educational references such as LibreTexts stoichiometry/04%3A_Stoichiometry_of_Chemical_Reactions).
Use grams or moles consistently
The yield equation is unit-agnostic because it uses a ratio. You may enter grams for mass yield or moles for amount yield, provided actual yield and theoretical yield use the same unit. Do not mix 45 g actual yield with 0.50 mol theoretical yield unless you first convert one quantity using molar mass. Atomic-weight data from sources like NIST chemistry data help make those conversions traceable.
When reporting a synthetic yield, grams are common for isolated product mass, while moles are useful for comparing stoichiometric equivalents.
Interpreting low, moderate, and good yields
A high percent yield usually means the reaction, purification, and drying steps were efficient. This calculator labels yields of 80% or more as good, 50–79.999% as moderate, and below 50% as low. These thresholds are practical teaching categories rather than universal rules: a 35% yield can be acceptable for a difficult multistep synthesis, while 90% may be expected for a clean precipitation reaction. Learn more about limiting reagents and reaction stoichiometry from OpenStax Chemistry 2e.
- Good yield:
often ≥80% for straightforward reactions.
- Moderate yield:
roughly 50–80%, common during optimization.
- Low yield:
below 50%, often worth troubleshooting.
Over 100% usually signals wet product, impurities, weighing error, or an incorrect theoretical yield.
Why actual yield is less than theoretical yield
Theoretical yield assumes complete reaction and perfect recovery. Real experiments rarely meet both assumptions. Product can remain dissolved in mother liquor, decompose during heating, stick to glassware, be lost during filtration, or be contaminated with solvent. Side reactions and equilibrium limitations also reduce isolated product. Good notebook practice records the mass before and after drying, purity observations, and any transfer losses so percent yield has a clear experimental context.
| Cause | Effect on actual yield | Typical fix |
|---|---|---|
| Incomplete reaction | Less product forms | Longer time, catalyst, temperature optimization |
| Transfer loss | Product left on glassware/filter | Rinse quantitatively and use correct filter size |
| Wet product | Apparent yield too high | Dry to constant mass |
| Impurity | Mass is not pure product | Recrystallize or purify before reporting |
Quick Reference Card
Actual Yield — Quick Reference
Quick reference • Actual Yield Calculator
Actual yield = (% yield ÷ 100) × theoretical yieldValid range: Percent yield is usually 0–100%; values above 100% require checking product purity, dryness, and stoichiometry.
Common Values
⚠ Watch Out
- •Do not mix grams and moles in the same yield ratio without converting first.
- •Do not treat wet or impure product mass as pure actual yield.
- •A percent yield above 100% usually signals an experimental or calculation problem.
- •The theoretical yield must be based on the limiting reagent, not simply the reactant with the smallest mass.
Pro Tips
- →Convert percent yield to a decimal before multiplying by theoretical yield.
- →Record product mass after drying to constant mass for reliable actual yield.
- →Use molar mass to convert between grams and moles before comparing yields.
- →Keep extra significant figures through stoichiometry and round the final actual yield.
- →Compare repeated trials using percent yield so different batch sizes are normalized.
FAQs
What is actual yield?
Actual yield is the amount of product actually obtained from a reaction. It is usually measured in grams after the product has been isolated and dried, but the same idea can be expressed in moles if both actual and theoretical yields use moles.
How do I calculate actual yield from percent yield?
Divide the percent yield by 100 and multiply by the theoretical yield. For example, if theoretical yield is 50 g and percent yield is 90%, actual yield = 0.90 × 50 g = 45 g.
Can actual yield be greater than theoretical yield?
A true pure-product actual yield should not exceed theoretical yield. Values above 100% usually indicate wet product, impurities, incomplete drying, a weighing error, or an incorrect limiting-reagent/theoretical-yield calculation.
Should I enter grams or moles?
Either is fine because the yield equation is unit-agnostic. The important rule is consistency: actual yield and theoretical yield must both be grams, both be moles, or both use another matching amount unit.
What is the difference between actual yield and theoretical yield?
Theoretical yield is the maximum amount predicted by stoichiometry from the limiting reagent. Actual yield is the amount recovered in the experiment. Percent yield compares the two using actual/theoretical × 100.
What counts as a good actual yield?
For many teaching-lab syntheses, 80% or higher is considered good, 50–80% moderate, and below 50% low. The acceptable yield depends strongly on reaction type, purification demands, and product stability.