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Theoretical yield is the maximum amount of product that can be formed in a chemical reaction, based on the stoichiometry of the balanced chemical equation. It is usually calculated using the limiting reactant, as it determines the maximum amount of product that can be formed. Theoretical yield does not take into account any losses or inefficiencies that may occur during the actual experiment.

Actual yield is the amount of product that is actually obtained from a chemical reaction, which is often less than the theoretical yield due to factors such as side reactions, impurities, incomplete reactions, and losses during the experimental process. Actual yield is determined through experimental measurements, such as weighing the product or using other analytical techniques.

Percent yield is a measure of the efficiency of a chemical reaction, expressed as a percentage of the actual yield to the theoretical yield. It is calculated using the formula: \[ \% Yield = \frac{Actual Yield}{Theoretical Yield} \times 100\] A high percent yield indicates that the reaction was efficient and produced close to the maximum amount of product possible, while a low percent yield suggests inefficiencies or losses during the reaction.

Theoretical yield, actual yield, and percent yield are related concepts used to describe the outcomes of chemical reactions. The key differences between these terms are: 1. Theoretical yield is based on stoichiometry and the limiting reactant, while actual yield is determined experimentally. 2. Theoretical yield represents the maximum possible amount of product that can be formed, while actual yield represents the amount of product actually obtained from the reaction. 3. Percent yield is a measure of the efficiency of the reaction, comparing the actual yield to the theoretical yield. By understanding these differences, students can better analyze and evaluate the results of chemical reactions and improve their experimental techniques to achieve higher percent yields.