Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

6. Thermodynamics and Kinetics

Energy Diagram

Organic Chemistry

6. Thermodynamics and Kinetics

Energy Diagram

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4:39 minutes

Problem 32

Textbook Question

The rate constant for a reaction can be increased by the stability of the reactant or by the stability of the transition state.

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Identify the relationship between the rate constant and the activation energy using the Arrhenius equation: k = Ae^{-Ea/RT}, where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature.

Understand that the activation energy (Ea) is the energy barrier that must be overcome for a reaction to proceed. Lowering the activation energy increases the rate constant.

Recognize that increasing the stability of the reactant typically increases the activation energy, as the reactant is at a lower energy state, making it harder to reach the transition state.

Realize that increasing the stability of the transition state lowers the activation energy, as the energy difference between the reactant and the transition state is reduced.

Conclude that the rate constant for a reaction can be increased by decreasing the stability of the reactant or by increasing the stability of the transition state.

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Key Concepts

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

Rate Constant

The rate constant (k) is a proportionality factor in the rate equation of a chemical reaction, indicating how quickly a reaction proceeds. It is influenced by factors such as temperature, concentration, and the nature of the reactants. A higher rate constant signifies a faster reaction, while a lower rate constant indicates a slower reaction.

Stability of Reactants

The stability of reactants refers to their energy state and tendency to undergo a reaction. More stable reactants have lower energy and are less likely to react, while less stable reactants are more reactive. Enhancing the stability of reactants can lead to a decrease in the rate of reaction, as they are less inclined to transition into products.

Transition State

The transition state is a high-energy, unstable arrangement of atoms that occurs during the transformation from reactants to products. It represents the peak of the energy barrier that must be overcome for a reaction to proceed. Increasing the stability of the transition state lowers the activation energy, thereby increasing the rate constant and accelerating the reaction.

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Textbook Question

Parts (a)–(f) of this assessment refer to the rotation around the single bond of ethane.

(a) Given that the rate of the reaction is independent of concentration, fill in the missing rates in the following table.

Textbook Question

How will the rate of the reaction between bromomethane and hydroxide ion be affected if the following changes in concentration are made?

a. The concentration of the alkyl halide is not changed and the concentration of the nucleophile is tripled.

Textbook Question

For rotation around a bond, the rate constant is equal to the reaction rate. Why?

Textbook Question

The rate constant for the uncatalyzed reaction of two molecules of glycine ethyl ester to form glycylglycine ethyl ester is 0.6 M^-1 s^-1. In the presence of Co²⁺, the rate constant is 1.5 × 10⁶ M^-1 s^-1. What rate enhancement does the catalyst provide?

Textbook Question

From the Arrhenius equation, predict how

a. increasing the experimental activation energy affects the rate constant for a reaction.

Textbook Question

From the Arrhenius equation, predict how

b. increasing the temperature affects the rate constant for a reaction.

Textbook Question

Consider the following reaction-energy diagram.

a. Label the reactants and the products. Label the activation energy for the first step and the second step.

b. Is the overall reaction endothermic or exothermic? What is the sign of ΔH°?

c. Which points in the curve correspond to intermediates? Which correspond to transition states?

d. Label the transition state of the rate-limiting step. Does its structure resemble the reactants, the products, or an intermediate?

Textbook Question

The rate of the reaction of methyl chloride with hydroxide ion is linearly dependent on both the concentration of methyl chloride and the concentration hydroxide ion. At 30 °C, the constant (k) for the reaction is 1.0 × 10^-5 M^-1 s^-1

b. If the concentration of methyl chloride is decreased to 0.010 M, what will be the effect on

1. the rate of the reaction?

2. the rate constant for the reaction?

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