Why is the experimental actual yield is typically less than the maximum calculated theoretical yield? Due to side reactions incomplete reactions, and losses during purification Because all reactions go to completion without any losses Because the theoretical yield is always incorrect Because more product is always formed than predicted

The experimental actual yield is typically less than the maximum calculated theoretical yield due to side reactions, incomplete reactions, and losses during purification. In a chemical reaction, the theoretical yield is the maximum amount of product that can be formed based on the stoichiometry of the reaction. However, in reality, there are various factors that can cause the actual yield to be lower than the theoretical yield. Some of these factors include:<br /><br />1. Side reactions: Side reactions can occur during the reaction process, which can lead to the formation of by-products instead of the desired product. This reduces the overall yield of the desired product.<br /><br />2. Incomplete reactions: In some cases, the reaction may not go to completion, meaning that not all of the reactants are converted into the product. This can result in a lower yield than the theoretical yield.<br /><br />3. Losses during purification: After the reaction is complete, the product may need to be purified to remove any impurities. During this purification process, some of the product may be lost, which can also reduce the overall yield.<br /><br />Therefore, the correct answer is: Due to side reactions, incomplete reactions, and losses during purification.