**3. Was there a metal which was oxidized by each of the others? (Anode in a cell producing + voltage with all other metals) Compare the voltages for the cell above and arrange the metals in order from most easily oxidized to least.** The image displays a table detailing the electrochemical cells, with columns labeled Cell, Anode, Cathode, and Volts. ### Table Breakdown:- **Cell:** Denotes the label for each electrochemical cell, ranging from A to H.- **Anode:** Indicates the metal used at the anode for each cell.- **Cathode:** Indicates the metal used at the cathode for each cell.- **Volts:** Displays the voltage output for each cell, which represents the potential difference between the anode and cathode.### Table Data:| Cell | Anode | Cathode | Volts ||------|-------|---------|-------|| A | Mg | Zn | 1.31 || B | Zn | Cu | -0.83 || C | Mg | Cu | +0.85 || D | Zn | Sn | -0.34 || E | Mg | Sn | +0.92 || F | Sn | Zn | +0.34 || G | Sn | Cu | -0.46 || H | Zn | Mg | -1.28 |### Explanation:- Positive voltages indicate a spontaneous reaction in the galvanic cell configuration with electrons flowing from the anode to the cathode.- Negative voltages could imply non-spontaneous reactions, requiring external potential to drive the reaction in the given direction under a galvanic setup.This table could be used in educational settings to explain concepts of electrochemistry, galvanic cells, and the nature of redox reactions within different metal pairings.

A question based on electrochemistry, which is to be accomplished.

3. Was there a metal which was oxidized by each of the others? (Anode in a cell producing + voltage with all other metals) Compare the voltages for the cell above and arrange the metals in order from most easily oxidized to least.

3. Was there a metal which was oxidized by each of the others? (Anode in a cell producing + voltage with all other metals) Compare the voltages for the cell above and arrange the metals in order from most easily oxidized to least.

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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Concept explainers

Science behind corrosion-test

Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.

Corrosion

Question

**3. Was there a metal which was oxidized by each of the others? (Anode in a cell producing + voltage with all other metals) Compare the voltages for the cell above and arrange the metals in order from most easily oxidized to least.**

The image displays a table detailing the electrochemical cells, with columns labeled Cell, Anode, Cathode, and Volts.

### Table Breakdown:

- **Cell:** Denotes the label for each electrochemical cell, ranging from A to H.
- **Anode:** Indicates the metal used at the anode for each cell.
- **Cathode:** Indicates the metal used at the cathode for each cell.
- **Volts:** Displays the voltage output for each cell, which represents the potential difference between the anode and cathode.

### Table Data:

| Cell | Anode | Cathode | Volts |
|------|-------|---------|-------|
| A | Mg | Zn | 1.31 |
| B | Zn | Cu | -0.83 |
| C | Mg | Cu | +0.85 |
| D | Zn | Sn | -0.34 |
| E | Mg | Sn | +0.92 |
| F | Sn | Zn | +0.34 |
| G | Sn | Cu | -0.46 |
| H | Zn | Mg | -1.28 |

### Explanation:
- Positive voltages indicate a spontaneous reaction in the galvanic cell configuration with electrons flowing from the anode to the cathode.
- Negative voltages could imply non-spontaneous reactions, requiring external potential to drive the reaction in the given direction under a galvanic setup.

This table could be used in educational settings to explain concepts of electrochemistry, galvanic cells, and the nature of redox reactions within different metal pairings.

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