Textbook Question
(c) Which step is the fastest?
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Ch.14 - Chemical Kinetics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 14, Problem 70b
Consider the following energy profile.
(b) How many intermediates are formed in the reaction?
Verified step by step guidance1
Identify the peaks and valleys in the energy profile diagram. Each valley between peaks represents a stable intermediate formed during the reaction process.
Count the number of valleys in the energy profile, as each valley corresponds to one intermediate.
Ensure that you are only counting the valleys that occur between the reactants and the products, excluding the starting reactant state and the final product state.
Verify if any intermediates are revisited or if any intermediate appears more than once in the reaction pathway, as each unique intermediate should be counted only once.
Sum up the total number of unique intermediates formed throughout the reaction pathway as indicated by the energy profile.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reaction Mechanism
A reaction mechanism is a step-by-step description of the pathway taken during a chemical reaction. It outlines the sequence of elementary steps, including the formation and consumption of intermediates. Understanding the mechanism helps in identifying how reactants transform into products and the role of intermediates in this process.
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03:06
Reaction Mechanism Overview
Intermediates
Intermediates are species that are formed during the course of a chemical reaction but are not present in the final products. They exist only transiently and are crucial for understanding the reaction pathway. Identifying intermediates can provide insights into the stability and reactivity of different species involved in the reaction.
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02:14Reaction Mechanism Example
Energy Profile Diagram
An energy profile diagram visually represents the energy changes that occur during a chemical reaction. It typically shows the energy of reactants, intermediates, and products, along with activation energy barriers. Analyzing this diagram helps in determining the number of intermediates and the overall energy changes associated with the reaction.
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01:57Energy Diagrams
Related Practice
Textbook Question
The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:
H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)
IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)
(a) Write the chemical equation for the overall process.
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Textbook Question
The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:
H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)
IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)
(c) Assuming that the first step of the mechanism is rate determining, predict the rate law for the overall process.
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Textbook Question
Consider the following energy profile.
(c) Which step is rate limiting?
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Textbook Question
(a) Based on the following reaction profile, how many intermediates are formed in the reaction A→D?
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Textbook Question
Consider the following energy profile.
(a) How many elementary reactions are in the reaction mechanism?
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