Textbook Question
Under certain conditions, the bromination of cyclohexene follows an unusual rate law:
c. What is the overall kinetic order?
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Ch.4 - The Study of Chemical Reactions
Wade9th EditionOrganic ChemistryISBN: 9780135213728
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Table of contents
- Ch.1 - Structure and Bonding107
- Ch. 2 - Acids and Bases; Functional Groups115
- Ch.3 - Structure and Stereochemistry of Alkanes100
- Ch.4 - The Study of Chemical Reactions99
- Ch.5 - Stereochemistry93
- Ch.6 - Alkyl Halides; Nucleophilic Substitution118
- Ch. 7 - Structure and Synthesis of Alkenes; Elimination158
- Ch.8 - Reactions of Alkenes171
- Ch.9 - Alkynes91
- Ch.10 - Structure and Synthesis of Alcohols143
- Ch.11 - Reactions of Alcohols104
- Ch. 12 - Infrared Spectroscopy and Mass Spectrometry22
- Ch. 13 - Nuclear Magnetic Resonance Spectroscopy45
- Ch. 14 - Ethers, Epoxides, and Thioethers72
- Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy89
- Ch. 16 - Aromatic Compounds74
- Ch. 17 - Reactions of Aromatic Compounds126
- Ch. 18 - Ketones and Aldehydes193
- Ch. 19 - Amines129
- Ch. 20 - Carboxylic Acids77
- Ch. 21 - Carboxylic Acid Derivatives141
- Ch. 22 - Condensations and Alpha Substitutions of Carbonyl Compounds175
- Ch. 23 - Carbohydrates and Nucleic Acids93
- Ch. 24 - Amino Acids, Peptides, and Proteins54
Chapter 4, Problem 14a
Draw the reaction-energy diagram for the following reverse reaction:
•CH3 + HCl → CH4 + Cl•
Verified step by step guidance1
Step 1: Understand the reverse reaction. The reverse reaction involves the formation of a methyl radical (•CH3) and hydrogen chloride (HCl) from methane (CH4) and a chlorine radical (Cl•). This is the reverse of a typical radical halogenation reaction.
Step 2: Identify the energy components of the reaction. The reaction-energy diagram will include the reactants (CH4 and Cl•), the transition state, and the products (•CH3 and HCl). The energy of the transition state will be higher than both the reactants and products.
Step 3: Determine the relative energy levels. Methane (CH4) is a stable molecule, so it will have a lower energy compared to the methyl radical (•CH3). The chlorine radical (Cl•) is also relatively reactive, so its energy will be higher than CH4 but lower than the transition state.
Step 4: Sketch the reaction-energy diagram. On the y-axis, plot the energy levels, and on the x-axis, plot the reaction progress. Start with CH4 and Cl• as the reactants, show a peak for the transition state, and end with •CH3 and HCl as the products. Label each part of the diagram clearly.
Step 5: Indicate the activation energy and overall energy change. The activation energy is the difference between the energy of the reactants and the transition state. The overall energy change (ΔE) is the difference between the energy of the reactants and the products. Ensure these are marked on the diagram.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reaction Energy Diagram
A reaction energy diagram visually represents the energy changes during a chemical reaction. It typically includes the energy of reactants and products, as well as the activation energy required for the reaction to proceed. The diagram helps illustrate the transition state and the overall energy change, indicating whether the reaction is exothermic or endothermic.
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06:07
Introduction to free energy diagrams.
Activation Energy
Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to form products. In a reaction energy diagram, this is depicted as the peak of the curve, where the transition state exists before the system can proceed to the products.
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06:07Introduction to free energy diagrams.
Bond Dissociation Energy
Bond dissociation energy is the energy required to break a specific bond in a molecule. In the context of the given reaction, understanding the bond dissociation energies of H-Cl and C-H bonds is crucial for predicting the energy changes during the reaction. This concept helps explain the stability of reactants and products and their relative energies in the reaction energy diagram.
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04:09How to calculate enthalpy using bond dissociation energies.
Related Practice
Textbook Question
When a small piece of platinum is added to a mixture of ethene and hydrogen, the following reaction occurs: Ethene
Doubling the concentration of hydrogen has no effect on the reaction rate. Doubling the concentration of ethene also has no effect.
a. What is the kinetic order of this reaction with respect to ethene? With respect to hydrogen? What is the overall order?
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Textbook Question
When a small piece of platinum is added to a mixture of ethene and hydrogen, the following reaction occurs:
Doubling the concentration of hydrogen has no effect on the reaction rate. Doubling the concentration of ethene also has no effect.
b. Write the unusual rate equation for this reaction.
c. Explain this strange rate equation, and suggest what one might do to accelerate the reaction.
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Textbook Question
•CH3 + HCl → CH4 + Cl•
b. What is the activation energy for this reverse reaction?
c. What is the heat of reaction (ΔH°) for this reverse reaction?
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Textbook Question
Draw a reaction-energy diagram for the following reaction:
•CH3 + Cl2 → CH3Cl + Cl•
The activation energy is 4 kJ/mol (1 kcal/mol), and the overall ΔH° for the reaction is –110 kJ/mol (–27 kcal/mol).
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Textbook Question
•CH3 + Cl2 → CH3Cl + Cl•
The activation energy is 4 kJ/mol (1 kcal/mol), and the overall ΔH° for the reaction is –110 kJ/mol (–27 kcal/mol).
b. Give the equation for the reverse reaction.
c. What is the activation energy for the reverse reaction?
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