Concept:The mathematical relationship between actual, theoretical, and percent yield perfectly dictates this logic. If the real-world mass matches the paper-calculated mass, the reaction was flawless.
Formula:$$ \text{If Actual} = \text{Theoretical, then } \frac{\text{Actual}}{\text{Theoretical}} = 1 $$
Solution:- The formula is \( \% \text{ yield} = (\text{Actual} / \text{Theoretical}) \times 100 \).
- If the Actual yield exactly equals the Theoretical yield, the fraction (Actual/Theoretical) becomes exactly 1.
- \( 1 \times 100 = 100\% \).
- Therefore, a 100% percent yield implies zero mechanical losses, zero side reactions, and perfect 100% stoichiometric efficiency.
Why other options are incorrect:- 10%, 50%, 90%: All these numbers indicate that the actual yield fell significantly short of the ideal theoretical value.
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