Actual yield is always less than theoretical yield due to:
Correct answer: D. All of these
- A. Operational losses
- B. Reaction reversibility
- C. Side reaction
- D. All of these
Explanation
Option D is correct since all three of these reasons are responsible for the actual yield being less than the theoretical yield. Option A is incorrect since operational losses alone are not responsible for the loss in actual yield.Option B is incorrect since reaction being reversible alone is not responsible for the loss in actual yield.Option C is incorrect since side reactions alone are not responsible for the loss in actual yield.
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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