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

Entropy

Organic Chemistry

6. Thermodynamics and Kinetics

Entropy

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6:18 minutes

Problem 39

Textbook Question

Predict which side of the equilibrium is favored by ∆H, ∆G, and ∆S.

Verified step by step guidance

Step 1: Analyze the reaction provided. The reaction involves the addition of water (H₂O) to a cyclohexene molecule, resulting in the formation of cyclohexanol. This is a hydration reaction.

Step 2: Consider the enthalpy change (∆H). Hydration reactions typically release energy because bonds are formed in the product (cyclohexanol) that are stronger than the bonds broken in the reactants. Therefore, ∆H is likely negative, favoring the product side.

Step 3: Evaluate the entropy change (∆S). The reaction involves combining two molecules (H₂O and cyclohexene) into one molecule (cyclohexanol). This results in a decrease in the number of particles, leading to a decrease in entropy (∆S is negative). A negative ∆S favors the reactant side.

Step 4: Assess the Gibbs free energy change (∆G). The relationship between ∆G, ∆H, and ∆S is given by the equation:

Δ G = Δ H - T Δ S

. At lower temperatures, the negative ∆H may dominate, favoring the product side. At higher temperatures, the negative ∆S may dominate, favoring the reactant side.

Step 5: Predict the equilibrium position. If ∆G is negative, the equilibrium will favor the product side (cyclohexanol). If ∆G is positive, the equilibrium will favor the reactant side (cyclohexene and H₂O). The temperature plays a crucial role in determining which side is favored.

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Key Concepts

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

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In the context of the given reaction, adding or removing reactants or products will influence which side of the equilibrium is favored, helping to predict the direction of the reaction.

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. A negative ∆G indicates that a reaction is spontaneous and favors the products, while a positive ∆G suggests that the reactants are favored. Understanding ∆G is crucial for predicting the favorability of the equilibrium position.

Enthalpy (∆H) and Entropy (∆S)

Enthalpy (∆H) refers to the heat content of a system, while Entropy (∆S) measures the disorder or randomness of a system. The relationship between these two concepts, along with temperature, is described by the Gibbs Free Energy equation (∆G = ∆H - T∆S). Analyzing ∆H and ∆S helps determine the thermodynamic favorability of a reaction and the direction in which the equilibrium will shift.

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Related Practice

Textbook Question

For each of the following processes, indicate whether you expect ∆S° to be greater than, less than, or equal to 0. Explain your answer.

(c)

Textbook Question

For each of the following processes, indicate whether you expect ∆S° to be greater than, less than, or equal to 0. Explain your answer.

(b) 2 C₆H₁₄(l) + 19 O₂(g) → 12 CO₂(g) + 14 H₂O(g)

Textbook Question

Using the bond-dissociation energies in Table 5.6 (see Section 5.3.1), estimate the equilibrium constant of the following reaction at 298 K.

Textbook Question

For the following reactions we have not seen yet, which side, if either, would be favored by increasing the temperature?

(b)

Textbook Question

For each of the following processes, indicate whether you expect ∆S° to be greater than, less than, or equal to 0. Explain your answer.

(a) Boiling water

Textbook Question

In Chapter 13, we discuss the ring-opening reactions of epoxides, such as the one shown here.

(b) Predict the sign of ∆S°.

Textbook Question

Would you expect ∆S to be greater than, less than, or equal to zero in the following reactions?

Textbook Question

For a reaction carried out at 25 °C with an equilibrium constant of 1 × 10^-3, to increase the equilibrium constant by a factor of 10:

a. how much must ∆G° change?

b. how much must ∆H° change if ∆S° = 0 kcal mol^-1K^-1?

c. how much must ∆S° change if ∆H° = 0 kcal mol^-1?

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