Chemistry › Section D · Stoichiometry of reactions › Topic D.4
Limiting reactants and yields
Real reactions rarely start with reactants in exact proportion, and they rarely deliver every gram the equation promises. The limiting reactant sets the most product you can make, and percent yield measures how close you came.
In this topic
- Something always runs out first
- Limiting and excess reactants
- Worked example: the smaller mass is not always limiting
- Worked example: comparing with the required amount
- Theoretical, actual and percent yield
- Why actual yields fall short
- Worked example: percent yield of aspirin
- Atom economy and green chemistry
- Yields across several steps
- Common mistakes to avoid
- Key takeaways
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