Atom Economy Calculator - Chemical Reaction Efficiency
An atom economy calculator finds what percentage of reactant mass ends up in a reaction's product, using the molecular weights of the reactants and product.
Atom Economy Calculator
For balanced reactions, you can include coefficients in your formulas:
- For N₂ + 3H₂ → 2NH₃, enter N2 and 3H2 as reactants and 2NH3 as the product
- For 2H₂ + O₂ → 2H₂O, enter 2H2 and O2 as reactants and 2H2O as the product
Results
Enter valid chemical formulas to see visualization
Documentation
What is an atom economy calculator?
An atom economy calculator works out how much of the mass of a chemical reaction's starting materials ends up in the desired product, rather than in waste byproducts. It does this by comparing the molecular weight of the product with the total molecular weight of the reactants, using the balanced chemical equation. The result is a percentage: atom economy.
Atom economy formula
Atom economy is calculated as:
The formula uses the coefficients from the balanced equation. Each reactant's molecular weight is multiplied by its coefficient before the weights are added together, and the product's molecular weight is multiplied by its own coefficient.
Atom economy was introduced by the chemist Barry M. Trost in 1991, as a way to judge how efficient a reaction's design is, separate from how well it performs in practice.
How to calculate atom economy
- Write out the balanced chemical equation for the reaction.
- Find the molecular weight of the desired product, using its coefficient from the equation.
- Add up the molecular weights of all the reactants, each multiplied by its coefficient.
- Divide the product weight by the total reactant weight, then multiply by 100.
Catalysts and solvents are left out of this calculation. A catalyst helps the reaction happen but is not used up, so it is not counted as a reactant. Solvents usually do not become part of the product either.
Worked example: hydrogen and oxygen
Consider the balanced equation for making water:
2H₂ + O₂ → 2H₂O
Using atomic weights H = 1.008 and O = 15.999:
- 2 H₂ = 2 × 2.016 = 4.032
- O₂ = 31.998
- total reactant weight = 4.032 + 31.998 = 36.030
- 2 H₂O = 2 × 18.015 = 36.030
Atom economy = (36.030 ÷ 36.030) × 100 = 100%
Every atom in the reactants ends up in the product, so the atom economy is 100%. This is expected for a properly balanced equation with only one product: mass cannot be created, so the product's mass can never exceed the combined mass of the reactants that made it. If a value above 100% comes out of a calculation, the equation entered is not correctly balanced.
Writing the same reaction without balancing it, as H₂ + O₂ → H₂O, does not describe a real reaction and gives a different, meaningless number: 18.015 ÷ (2.016 + 31.998) × 100 = 52.96%. This is why the equation must be balanced first.
Worked example: aspirin synthesis
Aspirin is made from salicylic acid and acetic anhydride:
C₇H₆O₃ + C₄H₆O₃ → C₉H₈O₄ + C₂H₄O₂
- salicylic acid (C₇H₆O₃): 138.12
- acetic anhydride (C₄H₆O₃): 102.09
- total reactant weight: 240.21
- aspirin (C₉H₈O₄, the desired product): 180.16
Atom economy = (180.16 ÷ 240.21) × 100 ≈ 75.0%
The remaining 25% of the mass leaves the reaction as acetic acid, a byproduct. In industrial production this acetic acid is commonly recovered and reused, which helps offset the loss.
Reading the result
- 90–100%: most reactant atoms end up in the product. Typical of addition reactions, where nothing is left over.
- 70–90%: good efficiency, common in many catalytic reactions.
- 50–70%: moderate. Substitution reactions, which release a leaving group as waste, often fall in this range.
- Below 50%: most of the reactant mass becomes waste rather than product.
These ranges are only a rough guide. A complex pharmaceutical intermediate with no cleaner route available might be considered acceptable at 65%, while a simple bulk chemical with cheaper alternatives would not be.
What atom economy does not measure
Atom economy only accounts for the reactants and product written in the balanced equation. It leaves out solvents, catalysts, and the energy needed to run the reaction. A reaction can have a high atom economy and still use a large amount of solvent, or need extreme temperature or pressure. For a fuller picture, chemists combine atom economy with other measures, such as the E-factor (mass of waste divided by mass of product) and process mass intensity (total mass used divided by mass of product).
History of atom economy
Barry M. Trost, a chemist then at the University of Wisconsin and later at Stanford University, introduced the concept of atom economy in a 1991 paper in the journal Science, "The Atom Economy—A Search for Synthetic Efficiency." Before this, chemists mostly judged a reaction by its yield: how close the amount of product obtained came to the theoretical maximum. Trost's idea added a different question. Even at high yield, how much of the reactant mass ends up as byproducts instead of product?
In 1998, atom economy became the second of the Twelve Principles of Green Chemistry, set out by Paul Anastas and John Warner in their book Green Chemistry: Theory and Practice. Since then, it has become a standard measure taught in chemistry courses and reported in many research papers on new synthetic methods.
Frequently asked questions
What is atom economy?
Atom economy is the percentage of the reactant mass in a chemical reaction that ends up in the desired product. It is found by dividing the product's molecular weight by the total molecular weight of the reactants, then multiplying by 100.
How is atom economy different from yield?
Yield measures how much product a reaction actually produces compared with the theoretical maximum, given the amount of starting material used. Atom economy measures something different: how much of the reactant mass could ever end up in the product, based on the reaction's chemistry alone. A reaction can have a high yield and a low atom economy at the same time, if it produces a lot of byproduct mass alongside the product.
Can atom economy be 100%?
Yes. Addition reactions, where reactant molecules combine without releasing any byproduct, reach 100% atom economy. Rearrangement reactions, which reorganize atoms within a molecule, can also reach 100%. A reaction with 100% atom economy can still be a poor choice overall if its yield is low or its reactants are hazardous.
Does atom economy include solvents and catalysts?
No. Catalysts are not consumed during the reaction, so they are not counted as reactants. Solvents are usually not counted either, unless part of the solvent becomes incorporated into the product. This means a reaction can show a high atom economy while still using large volumes of solvent.
What is a good atom economy?
Above 90% is considered excellent, 70–90% is good, and below 50% suggests most of the reactant mass is wasted. What counts as acceptable depends on the reaction: a complex product with no better route available can justify a lower atom economy than a simple, high-volume chemical.
How are the coefficients in a balanced equation used in the calculation?
Every reactant and the product must use their coefficients from the balanced equation. For 2H₂ + O₂ → 2H₂O, the reactant weight uses 2 × (weight of H₂) plus 1 × (weight of O₂), and the product weight uses 2 × (weight of H₂O). Skipping the coefficients, or using an unbalanced equation, gives a number that does not describe the real reaction.
References
- Trost, B. M. (1991). The atom economy—a search for synthetic efficiency. Science, 254(5037), 1471–1477.
- Anastas, P. T., & Warner, J. C. (1998). Green Chemistry: Theory and Practice. Oxford University Press.
- Sheldon, R. A. (2017). The E factor 25 years on: the rise of green chemistry and sustainability. Green Chemistry, 19(1), 18–43.