If a reaction is exergonic, then which of these statements is true? a. The products have lower Gibbs free energy than the reactants. b. Energy must be added for the reaction to proceed. c. The products have lower entropy (are more ordered) than the reactants. d. The reaction always occurs quickly.

Question

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Answer 1

Textbook Question

Chapter 8, Problem 1TYK

If a reaction is exergonic, then which of these statements is true?

a. The products have lower Gibbs free energy than the reactants.

b. Energy must be added for the reaction to proceed.

c. The products have lower entropy (are more ordered) than the reactants.

d. The reaction always occurs quickly.

Expert Solution & Answer

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.

Conclusion

In an exergonic reaction, the products have lower Gibbs free energy than the reactants.

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Students have asked these similar questions

Define the following terms: a. velocity b. kinetics c. half-life d. first-order reactions e. pseudo-first-order reaction

Which statements concerning free energy change are true?a. Free energy change is a measure of the rate of a reaction.b. Free energy change is a measure of the maximum amountof work available from a reaction.c. Free energy change is a constant for a reaction under anyconditions.d. Free energy change is related to the equilibrium constantfor a specific reaction.e. Free energy change is equal to zero at equilibrium.

Which of the following is true for all exergonic reactions? Group of answer choices A. The reactions are nonspontaneous B. A net input of energy from the surroundings is required for the reactions to proceed C. Some reactants will be converted to products D. The products have more total energy than the reactants E. The reaction proceeds with a net release of free energy

Answer 2

Textbook Question

Chapter 8, Problem 1TYK

If a reaction is exergonic, then which of these statements is true?

a. The products have lower Gibbs free energy than the reactants.

b. Energy must be added for the reaction to proceed.

c. The products have lower entropy (are more ordered) than the reactants.

d. The reaction always occurs quickly.

Expert Solution & Answer

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.

Conclusion

In an exergonic reaction, the products have lower Gibbs free energy than the reactants.

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Answer 3

Textbook Question

Chapter 8, Problem 1TYK

If a reaction is exergonic, then which of these statements is true?

a. The products have lower Gibbs free energy than the reactants.

b. Energy must be added for the reaction to proceed.

c. The products have lower entropy (are more ordered) than the reactants.

d. The reaction always occurs quickly.

Expert Solution & Answer

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.

Conclusion

In an exergonic reaction, the products have lower Gibbs free energy than the reactants.

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Answer 4

Textbook Question

Chapter 8, Problem 1TYK

If a reaction is exergonic, then which of these statements is true?

a. The products have lower Gibbs free energy than the reactants.

b. Energy must be added for the reaction to proceed.

c. The products have lower entropy (are more ordered) than the reactants.

d. The reaction always occurs quickly.

Expert Solution & Answer

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.

Conclusion

In an exergonic reaction, the products have lower Gibbs free energy than the reactants.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution & Answer

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.

Conclusion

In an exergonic reaction, the products have lower Gibbs free energy than the reactants.

Answer 8

Expert Solution & Answer

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.

Conclusion

In an exergonic reaction, the products have lower Gibbs free energy than the reactants.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Summary Introduction

Introduction:

The Gibbs free energy is a thermodynamic equation, where it is enthalpy (of a system or process) minus the product of the entropy and the absolute temperature. It is used to determine the spontaneity of the reaction.

Answer 12

Answer to Problem 1TYK

Correct answer:

The Gibbs free energy of the products is lower than that of the reactants.

Answer 13

Explanation of Solution

Explanation/Justification for the correct answer:

Option (a) is given as lower Gibbs free energy of products as compared to the reactants. In the case of exergonic reactions, the energy is always released. In this case, the reactants on interaction lose energy, so the energy of the products is lower than that of the reactants. The Gibbs free energy of the reaction is always negative in this case. Hence, option (a) is correct.

Explanation for incorrect answers:

Option (b) is given as need of energy for the reaction to proceed. There is no requirement for the energy to be added in the reaction, as these reactions do not require energy. So, it is a wrong answer.

Option (c) is given as that the products have lower entropy (are more ordered) than the reactants. The entropy of the products is increased in the case of exergonic reactions. The exergonic reactions are spontaneous and the spontaneity is favored toward the increase in entropy. Thus, the entropy of the products increases. So, it is a wrong answer.

Option (d) is given as that the reaction always occurs quickly. The rate of the reaction depends on many physical factors; hence, the reaction may be slow or quick depending on the external conditions. So, it is a wrong answer.