Question

Reasons why the actual yield can be smaller than the theoretical yield

Answer 1

The actual yield can be smaller than the theoretical yield in a chemical reaction due to various reasons such as mechanical losses, inefficient separation procedures, competing reactions, and incomplete reactions.

Step-by-step explanation:

In a chemical reaction, the actual yield refers to the amount of product that is actually obtained. It is often smaller than the theoretical yield, which is the amount of product that would be produced according to calculations based on the stoichiometry of the balanced chemical equation. The actual yield can be smaller than the theoretical yield due to various reasons:

1. Mechanical losses, such as spilling or product getting stuck to the container or equipment, can contribute to a smaller actual yield.
2. Separation procedures may not be 100% efficient, resulting in the loss of some product.
3. Competing reactions can occur, forming undesired products and reducing the amount of the desired product.
4. Reactions may not run to completion, resulting in a mixture of products and reactants.

These factors, among others, can lead to a smaller actual yield compared to the theoretical yield.