### Standard Gibbs Free Energy Changes for ReactionsThe table below presents the standard Gibbs free energy changes (ΔG°) for five different reactions, denoted as reactions A through E. The Gibbs free energy change is an important thermodynamic quantity that helps determine the spontaneity of a reaction. | **Reaction** | **ΔG° (kJ/mol)** ||--------------|------------------|| A | -31.5 || B | -16 || C | -35.6 || D | +6 || E | +26.3 |The ΔG° values provided indicate the amount of energy change for each reaction under standard conditions:- Negative ΔG° values (less than 0) suggest that the reactions (A, B, and C) are spontaneous under standard conditions.- Positive ΔG° values (greater than 0) suggest that the reactions (D and E) are non-spontaneous under standard conditions.The question posed is, "Of these reactions, which is the furthest from chemical equilibrium?"### Answer ExplanationChemical equilibrium is reached when the Gibbs free energy change, ΔG, is zero. This is a state where the forward and reverse reactions occur at the same rate. The reaction that is furthest from equilibrium will have the largest ΔG° value, either positive or negative.In this context, reaction **C** has the most negative ΔG° value (-35.6 kJ/mol), indicating it is the furthest from chemical equilibrium among the given reactions because it is the most spontaneous reaction under standard conditions.Therefore, the correct option is:- [x] **C**- [ ] A- [ ] B- [ ] D

A thermodynamic potential which is used to determine the maximum of reversible work that can be done…

Answered: Reaction AG° (kJ/mol) A -31.5 В -16 C…

Reaction AG° (kJ/mol) A -31.5 В -16 C -35.6 D +6 E +26.3 Of these reactions, which is the furthest from chemical equilibrium? A D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

### Standard Gibbs Free Energy Changes for Reactions

The table below presents the standard Gibbs free energy changes (ΔG°) for five different reactions, denoted as reactions A through E. The Gibbs free energy change is an important thermodynamic quantity that helps determine the spontaneity of a reaction.

| **Reaction** | **ΔG° (kJ/mol)** |
|--------------|------------------|
| A | -31.5 |
| B | -16 |
| C | -35.6 |
| D | +6 |
| E | +26.3 |

The ΔG° values provided indicate the amount of energy change for each reaction under standard conditions:

- Negative ΔG° values (less than 0) suggest that the reactions (A, B, and C) are spontaneous under standard conditions.
- Positive ΔG° values (greater than 0) suggest that the reactions (D and E) are non-spontaneous under standard conditions.

The question posed is, "Of these reactions, which is the furthest from chemical equilibrium?"

### Answer Explanation
Chemical equilibrium is reached when the Gibbs free energy change, ΔG, is zero. This is a state where the forward and reverse reactions occur at the same rate. The reaction that is furthest from equilibrium will have the largest ΔG° value, either positive or negative.

In this context, reaction **C** has the most negative ΔG° value (-35.6 kJ/mol), indicating it is the furthest from chemical equilibrium among the given reactions because it is the most spontaneous reaction under standard conditions.

Therefore, the correct option is:
- [x] **C**
- [ ] A
- [ ] B
- [ ] D

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