(a) Interpretation: The stability of 1-butene and 2-methylpropene is to be compared. Concept introduction: Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

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Answer 1

Question

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

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Answer 2

Question

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

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Answer 3

Question

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

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Answer 4

Question

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

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Answer 5

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

Answer 6

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Answer 7

Chapter 4, Problem 4.69AP

Interpretation Introduction

(a)

Interpretation:

The stability of 1-butene and 2-methylpropene is to be compared.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The hydration reaction between 1-butene and 2-methylpropene is to be compared.

Concept introduction:

In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.

Answer 10

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Answer 11

Interpretation Introduction

(c)

Interpretation:

The free-energy-diagrams representing the hydration reaction of alkenes, 2-methylpropene and 1-butene on same scale with the relative free energies of both starting materials and rate-determining transition states are to be drawn.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.

Answer 12

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

Answer 13

Interpretation Introduction

(d)

Interpretation:

The difference in the standard free energies of the transition states for the hydration reactions of 1-butene and 2-methylpropene using the mechanism is to be stated. The molecule which has lower transition state energy is to be stated. The reason fot the stable transition state is to be stated.

Concept introduction:

Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the rate of reaction. A reactant has to undergo transition state, transition state has highest energy than reactant and product. More stable the carbocation formed on hydration, lesser will be the transition state energy.

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 4 - Prob. 4.1P Ch. 4 - Prob. 4.2P Ch. 4 - Prob. 4.3P Ch. 4 - Prob. 4.4P Ch. 4 - Prob. 4.5P Ch. 4 - Prob. 4.6P Ch. 4 - Prob. 4.7P Ch. 4 - Prob. 4.8P Ch. 4 - Prob. 4.9P Ch. 4 - Prob. 4.10P

Solution Summary: The author explains the hydration reaction between 1-butene and

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