The theoretical yield is, when % yield and actual yield are 55% and 24g respectively:

The correct answer is 43.6g.

To arrive at this result, we must apply the fundamental principles of stoichiometry and yield analysis. In a perfect chemical environment, every atom of reactant would convert into the desired product. However, the physical world is rarely perfect. The relationship between what we expect to get (theoretical) and what we actually get (actual) is expressed through the percentage yield.

The Concept of Yield in Chemical History

The mathematical foundation for these calculations traces back to the late 18th century, specifically to the work of Jeremias Benjamin Richter, who coined the term "stoichiometry." Before Richter’s work, chemistry was largely qualitative—scientists described what happened but struggled to predict exactly how much material would be produced. Richter’s realization that chemical elements combine in fixed ratios allowed chemists to begin predicting the "Theoretical Yield" of any given reaction.

In the context of this specific problem, we are looking at a scenario where the efficiency of the reaction is already known (55%) and the final mass of the product obtained in the lab is recorded (24g). To find the starting expectation, we must "reverse-engineer" the percent yield formula.

Why is Theoretical Yield Always Higher?

In laboratory and industrial settings, the actual yield is almost always lower than the theoretical yield. This discrepancy is a point of intense study for chemical engineers and researchers. Several factors contribute to this:

1. Incomplete Reactions: Some reactions reach a state of equilibrium where reactants and products exist simultaneously, preventing a 100% conversion.


2. Side Reactions: Reactants might combine in unexpected ways to form "by-products" instead of the target product.


3. Physical Loss: During the process of filtration, evaporation, or transferring material from a beaker to a flask, small amounts of the product are inevitably left behind or lost to the environment.


4. Impurity of Reactants: If the starting materials are not 100% pure, the amount of product formed will naturally be lower than the calculation suggests.

The Industrial Significance

Understanding this calculation is vital in pharmaceutical and industrial manufacturing. For example, in the production of life-saving medicine, a 55% yield might be considered unacceptably low, prompting chemists to change the temperature or pressure to move the actual yield closer to the theoretical maximum. By calculating the theoretical yield first, scientists can set a "gold standard" for what is possible, allowing them to measure exactly how much room for improvement exists in their chemical processes.