Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases. Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Question

Want to see the full answer?

Answer 1

Question

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

For a particular reaction, AH° = −16.1 kJ/mol and AS° = −21.8 J/(mol·K). Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction? OT= Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than K

Which of the following statements are true for BOTH the "transition state" and an "intermediate" of reaction? (This is a multi-select question, select all that apply.). Both are only observed in enzyme-catalyzed reactions. Both can be converted to product(s) or might decompose back to the reactant(s). Neither are part of the "net equation" for the reaction. Both contain covalent bonds are in the process of breaking and/or forming. Both are part of every chemical reaction. (i.e. the mechanisms of all chemical reactions, whether enzyme catalyzed or not, will have involve both a transition state and an intermediate).

Consider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD what are the reactants and what are the products is this reaction spontaneous? How do you know? Is energy released or consumed by this reaction? If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneous

Answer 2

Question

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Answer 6

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Answer 7

Chapter 7.3, Problem 1C

Summary Introduction

To determine: Whether ∆G is zero, or have a positive value or a negative value in a reaction in which enthalpy decreases and entropy increases.

Introduction: Under conditions of a biochemical reaction, free energy (G) is defined as the amount of energy available to perform work. Entropy is defined as degree of randomness in a system and enthalpy is defined as the total potential energy of a system.

Answer 8

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Answer 9

Summary Introduction

To determine: Whether the given reaction in which enthalpy decreases and entropy increases is endergonic or exergonic.

Introduction: The chemical reactions are of two types, namely exergonic reaction and endergonic reaction. The type of reaction in which energy is released to the surrounding is known as exergonic reaction. This type of reactions is a spontaneous reaction and the Gibbs free energy (∆G) value for this reaction is negative. The type of reaction in which energy is absorbed from the surrounding is known as endergonic reaction. This type of reaction is a non-spontaneous reaction and the ∆G value for this reaction is positive.

Answer 10

Expert Solution & Answer

Answer 11

Expert Solution & Answer

Answer 12

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 13

Ch. 7.1 - Define energy, emphasizing how it is related to...Ch. 7.1 - Use examples to contrast potential energy and...Ch. 7.1 - Prob. 1C Ch. 7.2 - Prob. 3LO Ch. 7.2 - Prob. 1C Ch. 7.2 - Life is sometimes described as a constant struggle...Ch. 7.3 - Prob. 4LO Ch. 7.3 - Prob. 5LO Ch. 7.3 - Prob. 6LO Ch. 7.3 - Prob. 1C

Solution Summary: The author explains that free energy is defined as the amount of energy available to perform work in a biochemical reaction.

Concept explainers

Videos

Want to see the full answer?

Chapter 7 Solutions