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Chapter 3: Problem 74

Define the terms theoretical yield, actual yield, and percent yield. (b) Why is the actual yield in a reaction almost always less than the theoretical yield? (c) Can a reaction ever have \(110 \%\) actual yield?

Short Answer

Expert verified
Theoretical yield is the maximum amount of product that can be formed based on stoichiometry, while actual yield is the experimentally obtained product amount, and percent yield is the efficiency of a reaction calculated as \(\frac{Actual Yield}{Theoretical Yield} \times 100\%\). Actual yield is usually less than theoretical yield due to factors like incomplete reactions, side reactions, and impurities. A reaction cannot have a \(110\%\) actual yield, as it would contradict the principles of chemical reactions; any excess product would likely be due to experimental errors.

Step by step solution

01

1. Define Theoretical Yield

Theoretical yield refers to the maximum amount of product that can be formed from a given amount of limiting reactant, calculated based on stoichiometry and using balanced chemical equations.
02

2. Define Actual Yield

Actual yield is the actual amount of product that is obtained experimentally from a reaction, which is generally measured in the laboratory. It can be influenced by various factors, including impurities in reactants, side reactions, environmental conditions, and loss of material during the procedure.
03

3. Define Percent Yield

Percent yield represents the efficiency of a reaction, which is calculated by dividing the actual yield by the theoretical yield and then multiplying by 100. It is expressed as a percentage and illustrates the extent to which the reaction has produced the desired product. \(Percent Yield = \frac{Actual Yield}{Theoretical Yield} \times 100\%\)
04

4. Reason for Actual Yield being less than Theoretical Yield

The actual yield in a reaction is almost always less than the theoretical yield for a variety of reasons. Some of the factors contributing to lower actual yields include incomplete reactions, side reactions that consume reactants, unstable products that may decompose, impurities in the reactants, and loss of material during the separation and purification process.
05

5. Possibility of having 110% Actual Yield

It is not possible for a reaction to have a \(110\%\) actual yield because the maximum yield that can be achieved is \(100\%\). A percent yield greater than \(100\%\) would imply that more product has been formed than what is stoichiometrically possible, which contradicts the principles of chemical reactions. The presence of excess product in such cases can be attributed to experimental errors, such as inaccurate measurements or contamination of the product with other substances.

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Most popular questions from this chapter

At least \(25 \mu \mathrm{g}\) of tetrahydrocannabinol \((\mathrm{THC}),\) the active ingredient in marijuana, is required to produce intoxication. The molecular formula of \(\mathrm{THC}\) is $\mathrm{C}_{21} \mathrm{H}_{30} \mathrm{O}_{2} .\( How many moles of THC does this \)25 \mu \mathrm{g}$ represent? How many molecules?

(a) When a compound containing C, H, and O is completely combusted in air, what reactant besides the hydrocarbon is involved in the reaction? (b) What products form in this reaction? (c) What is the sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone, \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l),\) in air?

Determine the empirical and molecular formulas of each of the following substances: (a) Ibuprofen, a headache remedy, contains \(75.69 \% \mathrm{C}\), $8.80 \% \mathrm{H},\( and \)15.51 \% \mathrm{O}\( by mass and has a molar mass of \)206 \mathrm{~g} / \mathrm{mol}$. (b) Cadaverine, a foul-smelling substance produced by the action of bacteria on meat, contains \(58.55 \% \mathrm{C}\), \(13.81 \% \mathrm{H},\) and $27.40 \% \mathrm{~N}\( by mass; its molar mass is \)102.2 \mathrm{~g} / \mathrm{mol}$ (c) Epinephrine (adrenaline), a hormone secreted into the bloodstream in times of danger or stress, contains \(59.0 \%\) C, \(7.1 \%\) H, \(26.2 \%\) O, and $7.7 \% \mathrm{~N}\( by mass; its molar mass is about \)180 \mathrm{u}$.

Propenoic acid, \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{2},\) is a reactive organic liquid that is used in the manufacturing of plastics, coatings, and adhesives. An unlabeled container is thought to contain this liquid. A \(0.275-g\) sample of the liquid is combusted to produce \(0.102 \mathrm{~g}\) of water and \(0.374 \mathrm{~g}\) carbon dioxide. Is the unknown liquid propenoic acid? Support your reasoning with calculations.

The fat stored in a camel's hump is a source of both energy and water. Calculate the mass of \(\mathrm{H}_{2} \mathrm{O}\) produced by the metabolism of \(1.0 \mathrm{~kg}\) of fat, assuming the fat consists entirely of tristearin \(\left(\mathrm{C}_{57} \mathrm{H}_{110} \mathrm{O}_{6}\right)\), a typical animal fat, and assuming that during metabolism, tristearin reacts with \(\mathrm{O}_{2}\) to form only \(\mathrm{CO}_{2}\) and $\mathrm{H}_{2} \mathrm{O}$.
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