Actual yield
Definition
Actual yield is the quantity of product actually obtained from a chemical reaction. It is often measured in grams or moles and is usually less than the theoretical yield due to various practical limitations.
5 Must Know Facts For Your Next Test
- Actual yield can be affected by factors such as incomplete reactions, side reactions, and loss of product during recovery.
- It is essential for calculating percent yield, which compares actual yield to theoretical yield.
- Unlike theoretical yield, actual yield must be determined experimentally.
- The difference between actual and theoretical yields helps identify inefficiencies in a reaction process.
- In laboratory settings, achieving an actual yield close to the theoretical yield indicates a well-conducted experiment.
Review Questions
- What factors can cause the actual yield to be less than the theoretical yield?
- How is actual yield determined in a laboratory setting?
- Why is it important to compare actual yield with theoretical yield using percent yield?
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Related terms
Theoretical Yield: The maximum amount of product that could be formed from given reactants, assuming complete conversion without any losses.
Percent Yield: A measure of the efficiency of a reaction, calculated as $(\text{actual \;yield} / \text{theoretical \;yield}) \times 100\%$.
Limiting Reactant: The substance that is completely consumed first in a chemical reaction, thus limiting the amount of product formed.
