The actual yield of a reaction is usually less than the theoretical yield for all of the following reasons EXCEPT
Correct answer: C. the balanced equation was written incorrectly
- A. some product is lost during filtration and transfer
- B. side reactions produce unwanted products
- C. the balanced equation was written incorrectly
- D. the reaction is reversible and does not go to completion
Explanation
Physical losses, competing side reactions and reversibility are all genuine reasons why a real yield falls short. A wrongly balanced equation is not a reason for a low yield at all; it simply makes the calculated theoretical yield wrong, so the comparison itself becomes meaningless. Recognising which factors are chemical and which are arithmetic is the point of the question.
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About Theoretical and Percentage Yield
Theoretical yield is the maximum product predicted from a balanced equation and the amount of limiting reactant. Work includes identifying the limiting reagent, comparing theoretical and actual yield, and calculating percentage yield using stoichiometric mole relationships.
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