Thermodynamically stable product compared with reactant in the given reaction has to be determined. 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.

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Answer 1

Question

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

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Draw an energy diagram for each reaction. Label the axes, the startingmaterial, product, transition state, ΔHo, and Ea.a.) a concerted reaction with ΔHo = −80 kJ/mol and Ea = 16 kJ/molb.) a two-step reaction, A → B → C, in which the relative energy of thecompounds is A < C < B, and the step A → B is rate-determining

At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 10? Is this a thermodynamically-favorable reaction? 2. At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 100? Is this a thermodynamically-favorable reaction? 3. At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 0.1? Is this a thermodynamically-favorable reaction? 4. At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 0.01? Is this a thermodynamically-favorable reaction? 5. What do you notice about the sign of ∆G ̊ and the magnitude of Keq? 6. What is the change in ∆G ̊ when Keq increases by a factor of 10? 100? Write 1-2 sentences to describe this relationship.

6. Draw a reaction energy diagram for an endergonic reaction that is fast.

Answer 2

Question

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Expert Solution & Answer

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Answer 3

Question

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Expert Solution & Answer

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See solution

Answer 5

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Answer 6

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

Answer 7

Chapter 5.7, Problem 26P

(a)

Interpretation Introduction

Interpretation:

Thermodynamically stable product compared with reactant in the given reaction has to be determined.

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.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Answer 9

(b)

Interpretation Introduction

Interpretation:

Most kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Answer 10

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Answer 11

(c)

Interpretation Introduction

Interpretation:

Least kinetically stable product compared with reactant in the given reaction has to be determined.

Concept introduction:

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.

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.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 5.1 - Determine the degree of unsaturation and then draw...Ch. 5.1 - Prob. 4P Ch. 5.2 - Prob. 5P Ch. 5.2 - Draw the structure for each of the following: a....Ch. 5.2 - What is each compounds systematic name?Ch. 5.4 - Assign relative priorities to each set of...Ch. 5.4 - Tamoxifen slows the growth of some breast tumors...Ch. 5.4 - Draw and label the E and Z isomers for each of the...Ch. 5.4 - Prob. 12P Ch. 5.4 - Name each of the following:

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