Assertion: The theoretical yield of a reaction is the amount of the product produced by
the balanced equation when whole of the limiting reagent has reacted.
Reason: In practice actual yield is always less than the theoretical yield.
a) Assertion and reason both are correct and reason is the correct explanation of
assertion.
b) Assertion and reason both are correct but reason is not the correct explanation
of assertion.
c) Assertion is correct statement but reason is wrong statement.
d) Assertion is wrong statement but reason is correct statement.
Answers
Explanation:
Theoretical and Actual Yields
Reactants not completely used up are called excess reagents, and the reactant that completely reacts is called the limiting reagent. This concept has been illustrated for the reaction:
2Na+Cl2→2NaCl(1)
Amounts of products calculated from the complete reaction of the limiting reagent are called theoretical yields, whereas the amount actually produced of a product is the actual yield. The ratio of actual yield to theoretical yield expressed in percentage is called the percentage yield.
percentyield=actualyieldtheoreticalyield×100
Chemical reaction equations give the ideal stoichiometric relationship among reactants and products. Thus, the theoretical yield can be calculated from reaction stoichiometry. For many chemical reactions, the actual yield is usually less than the theoretical yield, understandably due to loss in the process or inefficiency of the chemical reaction.