A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn. Concept introduction: Thermodynamic stability can be represented as Δ G 0 . Depend upon the value of Δ G 0 it is possible to find stability of the product compared with the reactant. If Δ G 0 is negative, then the product is thermodynamically stable compared with the reactant. If Δ G 0 is positive, then the product is thermodynamically unstable compared with the reactant In an exergonic reaction the products have a lower free energy than it consumes. In an endergonic reaction the product have a higher free energy than it consumes. Kinetic stability can be represented as Δ G ∓ . Depend upon the value of Δ G ∓ it is possible to find stability of the product compared with the reactant. If Δ G ∓ is large, then the reactant is kinetically stable because it reacts slowly. If Δ G ∓ is small, then the reactant is kinetically unstable because it reacts rapidly. If Δ G ∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable. Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

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Answer 1

Question

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

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Answer 2

Question

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Expert Solution & Answer

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Answer 3

Question

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

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Answer 4

Question

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Expert Solution & Answer

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Answer 5

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Answer 6

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Answer 7

Chapter 5.7, Problem 16P

(a)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Answer 8

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Answer 9

(b)

Interpretation Introduction

Interpretation:

A reaction coordinate diagram for the reaction in which the product is thermodynamically unstable and kinetically stable should be drawn.

Concept introduction:

Thermodynamic stability can be represented as ΔG0. Depend upon the value of ΔG0 it is possible to find stability of the product compared with the reactant.

If ΔG0 is negative, then the product is thermodynamically stable compared with the reactant.

If ΔG0 is positive, then the product is thermodynamically unstable compared with the reactant.

In an exergonic reaction the products have a lower free energy than it consumes.

In an endergonic reaction the product have a higher free energy than it consumes.

Kinetic stability can be represented as ΔG∓. Depend upon the value of ΔG∓ it is possible to find stability of the product compared with the reactant.

If ΔG∓ is large, then the reactant is kinetically stable because it reacts slowly.

If ΔG∓ is small, then the reactant is kinetically unstable because it reacts rapidly.

If ΔG∓ for the reverse reaction is large then he product is kinetically stable, similarly if it is small then the product is kinetically unstable.

Reaction coordinate diagram shows how the energy of the system changes during a chemical reaction.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 5.1 - Prob. 1P Ch. 5.1 - Draw the structure for each of the following: a....Ch. 5.1 - What is each compounds systematic name?Ch. 5.3 - Prob. 4P Ch. 5.3 - Prob. 5P Ch. 5.3 - Prob. 7P Ch. 5.4 - a. For which reaction in each set below will S be...Ch. 5.6 - Prob. 9P Ch. 5.6 - How many different alkenes can be hydrogenated to...Ch. 5.6 - The same alkane is obtained from the catalytic...

Solution Summary: The author explains that a reaction coordinate diagram for the reaction in which the product is thermodynamically stable and kinetically unstable should be drawn.

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