Ch.3 - Chemical Reactions and Reaction Stoichiometry

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook

Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 74c

Chapter 3, Problem 74c

(c) Can a reaction ever have 110% actual yield?

Verified step by step guidance

insert step 1> Understand the concept of actual yield and theoretical yield. Actual yield is the amount of product obtained from a chemical reaction, while theoretical yield is the maximum amount of product that could be formed from the given reactants, assuming perfect conditions.

insert step 2> Recognize that the percent yield is calculated using the formula: \( \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \).

insert step 3> Consider the implications of a percent yield greater than 100%. A percent yield over 100% would imply that more product was obtained than theoretically possible, which suggests an error in the experiment or measurement.

insert step 4> Identify potential reasons for a percent yield over 100%, such as measurement errors, impurities in the product, or side reactions that produce additional product.

insert step 5> Conclude that while a reaction can be reported to have a percent yield over 100%, it typically indicates an error or anomaly, as it is not physically possible to obtain more product than the theoretical maximum.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Actual Yield

Actual yield refers to the amount of product that is actually obtained from a chemical reaction, measured in grams or moles. It is determined through experimental procedures and can vary due to factors such as incomplete reactions, side reactions, or losses during product recovery. Understanding actual yield is crucial for evaluating the efficiency of a reaction.

Theoretical Yield

Theoretical yield is the maximum amount of product that could be formed from a given amount of reactants, assuming complete conversion and no losses. It is calculated based on stoichiometric ratios derived from balanced chemical equations. Theoretical yield serves as a benchmark against which actual yield is compared to assess the efficiency of a reaction.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by dividing the actual yield by the theoretical yield and multiplying by 100. It provides insight into how well a reaction proceeds and is expressed as a percentage. A percent yield greater than 100% indicates an error in measurement or calculation, as it is impossible to produce more product than theoretically possible.

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Related Practice

Textbook Question

(a) Define the terms limiting reactant and excess reactant.

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Textbook Question

The combustion of one mole of liquid octane, CH3(CH2)6CH3, produces 5470 kJ of heat. Calculate how much heat is produced if 1.000 gallon of octane is combusted.

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Textbook Question

Consider the mixture of propane, C3H8, and O2 shown here. (a) Write a balanced equation for the combustion reaction that occurs between propane and oxygen.

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Textbook Question

Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. (c) How many molecules of CO2, H2O, C2H5OH, and O2 will be present if the reaction goes to completion?

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Textbook Question

Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. (b) Which reactant is the limiting reactant?

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Textbook Question

(c) Why should you base your choice of which compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

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