Textbook Question
(a) Define the terms limiting reactant and excess reactant.
Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 3, Problem 73c
(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?
Verified step by step guidance1
Understand the concept of a limiting reactant: The limiting reactant in a chemical reaction is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this reactant since the reaction cannot continue without it.
Recognize the difference between moles and mass: Moles measure the number of particles in a substance, which directly correlates to the number of reactant particles available to react. Mass, on the other hand, measures the weight of these particles, which varies depending on the molecular weight of each substance.
Convert mass to moles for comparison: To accurately determine which reactant will limit the reaction, convert the mass of each reactant into moles using their respective molar masses. This step is crucial because it aligns the units of measure, allowing for a direct comparison of the reactants' availability for the reaction.
Compare the stoichiometric ratios: Use the balanced chemical equation to compare the mole ratios of the reactants. This comparison will help you determine which reactant is in insufficient quantity relative to the others, according to the stoichiometric requirements of the reaction.
Identify the limiting reactant: The reactant that has the smallest ratio of available moles to required moles (as per the balanced equation) is the limiting reactant. This is because it will be consumed first, stopping the reaction, regardless of the amounts of other reactants present.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Limiting Reactant
The limiting reactant is the substance that is completely consumed in a chemical reaction, thus determining the maximum amount of product that can be formed. It is essential to identify this reactant to predict the yield of the reaction accurately. The reactant that runs out first limits the reaction's progress, making it crucial for stoichiometric calculations.
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Limiting Reagent Concept
Mole Concept
The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole corresponds to Avogadro's number (approximately 6.022 x 10²³) of particles, such as atoms or molecules. Using moles allows chemists to relate mass to the number of particles, facilitating comparisons between reactants in a reaction based on their stoichiometric ratios.
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on balanced equations. It involves using the mole ratios derived from the coefficients in a balanced equation to determine how much of each reactant is needed or how much product can be formed. This concept is vital for understanding how initial moles, rather than mass, dictate the limiting reactant in a reaction.
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Related Practice
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.
Textbook Question
(c) Can a reaction ever have 110% actual yield?
Textbook Question
(b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant?
Textbook Question
(b) Why is the actual yield in a reaction almost always less than the theoretical yield?
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Textbook Question
(a) Define the terms theoretical yield, actual yield, and percent yield.
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