Why chemical reactions rarely produce the perfect amount of product
In short: In a perfect world, chemistry would follow math exactly. In reality, there is always a gap between what we calculate and what we actually create. This video explains the mechanics of chemical yield and how to calculate the discrepancy.
The video explores the distinction between theoretical yield—the maximum amount of product predicted by chemical equations—and actual yield, which is the amount physically obtained during an experiment. It highlights three primary reasons why actual yields typically fall short: incomplete reactions (due to slow speeds or reversibility), unwanted side reactions that divert reactants, and physical losses during lab procedures like filtering or transferring substances.
For students preparing for 2027/28 exams, the video provides the essential formula for quantifying these losses: (Actual Yield / Theoretical Yield) x 100. It includes worked examples to demonstrate how to apply these calculations across various exam boards, including AQA, Edexcel, and OCR.
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Sources
- Summary by Intellect · source: GCSE Chemistry - Percentage Yield - Theoretical & Actual Yield | Calculations (2027/28 exams)
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