Textbook Question
Of the compounds you named in Problem 45:
b. Which is the least stable?
a.
b.
c.
d.
e.
f.
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Ch. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and Kinetics
Bruice8th EditionOrganic ChemistryISBN: 9780135213711
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Table of contents
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)31
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)65
- Ch. 2 - Acids and Bases: Central to Understanding Organic Chemistry84
- Ch. 3 - An Introduction to Organic Compounds:Nomenclature, Physical Properties, and Structure183
- Ch. 4 - Isomers: The Arrangement of Atoms in Space121
- Ch. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and Kinetics83
- Ch. 6 - The Reactions of Alkenes • The Stereochemistry of Addition Reactions175
- Ch. 7 - The Reactions of Alkynes • An Introduction to Multistep Synthesis119
- Ch. 8 - Delocalized Electrons: Their Effect on Stability, pKa, and the Products of a Reaction • Aromaticity and Electronic Effects: An Introduction to the Reactions of Benzene148
- Ch. 9 - Substitution and Elimination Reactions of Alkyl Halides212
- Ch. 10 - Reactions of Alcohols, Ethers, Epoxides, Amines, and Sulfur-Containing Compounds131
- Ch. 11 - Organometallic Compounds60
- Ch. 12 - Radicals90
- Ch. 13 - Mass Spectrometry; Infrared Spectroscopy; UV/Vis Spectroscopy62
- Ch. 14 - NMR Spectroscopy95
- Ch. 15 - Reactions of Carboxylic Acids and Carboxylic Acid Derivatives123
- Ch. 16 - Reactions of Aldehydes and Ketones • More Reactions of Carboxylic Acid Derivatives141
- Ch. 17 - Reactions at the Alpha-Carbon101
- Ch. 18 - Reactions of Benzene and Substituted Benzenes144
- Ch. 19 - More About Amines • Reactions of Heterocyclic Compounds49
- Ch. 20 - The Organic Chemistry of Carbohydrates80
- Ch. 21 - Amino Acids, Peptides, and Proteins57
- Ch. 22 - Catalysis in Organic Reactions and in Enzymatic Reactions35
- Ch. 23 - The Organic Chemistry of the Coenzymes—Compounds Derived from Vitamins1
- Ch. 28 - Pericyclic Reactions58
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Bruice 8th EditionCh. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and KineticsProblem 50a,b
Bruice 8th EditionCh. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and KineticsProblem 50a,bChapter 6, Problem 50a,b
In a reaction in which reactant A is in equilibrium with product B at 25 °C, what relative amounts of A and B are present at equilibrium if ∆G° at 25 °C is
a. 2.72 kcal/mol?
b. 0.65 kcal/mol?
Verified step by step guidance1
Understand the relationship between the Gibbs free energy change (∆G°) and the equilibrium constant (K) using the equation: , where R is the gas constant (1.987 cal/(mol·K)) and T is the temperature in Kelvin (25 °C = 298 K).
Rearrange the equation to solve for the equilibrium constant (K): . This will allow you to calculate the ratio of products (B) to reactants (A) at equilibrium.
Substitute the given values of ∆G° (2.72 kcal/mol and 0.65 kcal/mol) into the equation. Remember to convert ∆G° from kcal/mol to cal/mol by multiplying by 1000 (e.g., 2.72 kcal/mol = 2720 cal/mol).
For each case, calculate the value of K using the rearranged equation. This will give you the equilibrium constant, which represents the ratio of the concentration of B to A at equilibrium: .
Interpret the results: If K > 1, product B is favored at equilibrium. If K < 1, reactant A is favored. Use the calculated K values to determine the relative amounts of A and B for each case.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Gibbs Free Energy (∆G)
Gibbs Free Energy (∆G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It indicates the spontaneity of a reaction; a negative ∆G suggests that the reaction proceeds forward, while a positive ∆G indicates that the reaction is non-spontaneous. The standard Gibbs free energy change (∆G°) at a specific temperature helps predict the equilibrium position of a reaction.
Recommended video:
Guided course
05:02
Breaking down the different terms of the Gibbs Free Energy equation.
Equilibrium Constant (K)
The equilibrium constant (K) is a dimensionless value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is derived from the Gibbs free energy change, where a negative ∆G° corresponds to a K value greater than 1, favoring products, while a positive ∆G° corresponds to a K value less than 1, favoring reactants. Understanding K is essential for determining the relative amounts of A and B at equilibrium.
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02:19The relationship between equilibrium constant and pKa.
Relationship between ∆G° and K
The relationship between standard Gibbs free energy change (∆G°) and the equilibrium constant (K) is given by the equation ∆G° = -RT ln(K), where R is the universal gas constant and T is the temperature in Kelvin. This equation allows us to calculate K from ∆G° and vice versa. By knowing the value of ∆G° at 25 °C, we can determine the relative concentrations of reactants and products at equilibrium, which is crucial for answering the question.
Recommended video:
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01:40Same atoms, same connectivity, 1 chiral center.
Related Practice
Textbook Question
a. Which is the most stable: 3,4-dimethyl-2-hexene, 2,3-dimethyl-2-hexene, or 4,5-dimethyl-2-hexene?
b. Which compound has the largest heat of hydrogenation?
c. Which compound has the smallest heat of hydrogenation?
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Textbook Question
Which bond is stronger? Briefly explain why.
a.
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Textbook Question
Draw the skeletal structure of 3,3-dimethyl-7-(1-methylethyl)-6-(1-methylpropyl)decane.
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Textbook Question
Which bond is stronger? Briefly explain why.
b.
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Textbook Question
In a reaction in which reactant A is in equilibrium with product B at 25 °C, what relative amounts of A and B are present at equilibrium if ∆G° at 25 °C is
c. -2.72 kcal/mol?
d. -0.65 kcal/mol?
849
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