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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

For many years chloroform \(\left(\mathrm{CHCl}_{3}\right)\) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that may cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of this compound.

Define the term "mole." What is the unit for mole in calculations? What does the mole have in common with the pair, the dozen, and the gross? What does Avogadro's number represent?

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen. $$ 3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) $$ In a particular reaction, 6.0 moles of \(\mathrm{NH}_{3}\) were produced. How many moles of \(\mathrm{H}_{2}\) and how many moles of \(\mathrm{N}_{2}\) were reacted to produce this amount of \(\mathrm{NH}_{3} ?\)

The aluminum sulfate hydrate \(\left[\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} \cdot x \mathrm{H}_{2} \mathrm{O}\right]\) contains 8.20 percent Al by mass. Calculate \(x\), that is, the number of water molecules associated with each \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) unit.

Monosodium glutamate (MSG), a food-flavor enhancer, has been blamed for "Chinese restaurant syndrome," the symptoms of which are headaches and chest pains. MSG has the following composition by mass: 35.51 percent \(\mathrm{C}, 4.77\) percent \(\mathrm{H}, 37.85\) percent \(\mathrm{O}, 8.29\) percent \(\mathrm{N},\) and 13.60 percent \(\mathrm{Na}\). What is its molecular formula if its molar mass is about \(169 \mathrm{~g} ?\)
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