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Chapter 3: Problem 88

Why is the actual yield of a reaction almost always smaller than the theoretical yield?

Short Answer

Expert verified
The actual yield of a chemical reaction is often less than the theoretical yield due to several factors, including reversible reactions, side reactions, loss during product recovery, and measurement errors.

Step by step solution

01

Theoretical vs Actual Yield Explanation

The theoretical yield of a chemical reaction is the quantity of products that can be formed from the limiting reactants according to stoichiometry and the balanced chemical equation. It is what we would expect under 'perfect' conditions. On the other hand, the actual yield is the amount of product that is actually formed in a chemical reaction and is almost always less than the theoretical yield.
02

Reasons for Less Actual Yield

There are several reasons for this departure between the two yields. 1) The reaction may not go to completion because it is reversible, meaning the reactants and products remain in balance with each other. 2) There may be side reactions that consume reactants or create additional products aside from the one desired. 3) Some product may be lost when it is separated from the reaction mixture or purified. 4) There might be experimental errors during measurement phases which contribute to a decrease in the actual yield.
03

Practical Yield Considerations

In summary, while the theoretical yield provides an important benchmark, many practical considerations mean that the actual yield is typically less. It's important to note that comparing the actual yield to the theoretical yield (as a percentage, known as the percent yield) is a key measurement in evaluating the efficiency of a laboratory or industrial reaction.

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Most popular questions from this chapter

Describe the operation of a mass spectrometer.

When heated, lithium reacts with nitrogen to form lithium nitride: $$ 6 \mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Li}_{3} \mathrm{~N}(s) $$ What is the theoretical yield of \(\mathrm{Li}_{3} \mathrm{~N}\) in grams when \(12.3 \mathrm{~g}\) of \(\mathrm{Li}\) are heated with \(33.6 \mathrm{~g}\) of \(\mathrm{N}_{2} ?\) If the actual yield of \(\mathrm{Li}_{3} \mathrm{~N}\) is \(5.89 \mathrm{~g}\), what is the percent yield of the reaction?

Cinnamic alcohol is used mainly in perfumery, particularly in soaps and cosmetics. Its molecular formula is \(\mathrm{C}_{9} \mathrm{H}_{10} \mathrm{O}\) (a) Calculate the percent composition by mass of \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{O}\) in cinnamic alcohol. (b) How many molecules of cinnamic alcohol are contained in a sample of mass \(0.469 \mathrm{~g} ?\)

A sample of a compound of \(\mathrm{Cl}\) and \(\mathrm{O}\) reacts with an excess of \(\mathrm{H}_{2}\) to give \(0.233 \mathrm{~g}\) of \(\mathrm{HCl}\) and \(0.403 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\). Determine the empirical formula of the compound.

Tin(II) fluoride \(\left(\mathrm{SnF}_{2}\right)\) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of \(\mathrm{F}\) in grams in \(24.6 \mathrm{~g}\) of the compound?
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