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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![**Writing the Cell Diagram for the Given Electrochemical Cell**
The diagram illustrates a galvanic (voltaic) cell, consisting of two half-cells connected by a salt bridge. The components of this electrochemical cell are detailed below:
### Components:
- **Left Half-Cell:**
- **Electrode:** A platinum (Pt) electrode, used as an inert conductor.
- **Solutions/Compounds:**
- Potassium chloride (\(\text{KCl(aq)}\)) is the electrolyte.
- Mercurous chloride (\(\text{Hg}_2\text{Cl}_2(s)\)) is a solid.
- Elemental mercury (\(\text{Hg(l)}\)), which is in liquid form.
- **Right Half-Cell:**
- **Electrode:** Zinc (\(\text{Zn}\)) metal.
- **Solution:** Zinc chloride (\(\text{ZnCl}_2(aq)\)) serving as the electrolyte.
### Connections:
- An external circuit connects the two electrodes shown by the wires leading from the \(-\) terminal (left) to the \(+\) terminal (right) through a voltmeter (V), allowing electron flow.
- A salt bridge is included between the two solutions to maintain electrical neutrality by allowing the migration of ions.
### Cell Diagram:
The cell diagram, representing the reaction occurring in the galvanic cell, is written as follows:
\[
\text{Pt} | \text{Hg}_2\text{Cl}_2(\text{s}) | \text{Hg}(\text{l}) || \text{ZnCl}_2(\text{aq}) | \text{Zn}
\]
**Explanation:**
- The single vertical lines (\(|\)) represent phase boundaries.
- The double vertical line (\(||\)) signifies the salt bridge separating the two half-cells.
- The left side denotes the anode side (oxidation occurs, \(-\) electrode).
- The right side denotes the cathode side (reduction occurs, \(+\) electrode).
This cell generates electrical energy through a spontaneous redox reaction, which can be measured with the voltmeter in the circuit. Using a diagrammatic representation such as this is crucial for visualizing the components and reactions of galvanic cells in electrochemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9974d8b3-5991-4e97-8565-bd43e478c91b%2Fb3316994-9d81-4393-b3fd-74be636726ff%2F9ojvg13zc_processed.png&w=3840&q=75)
Transcribed Image Text:**Writing the Cell Diagram for the Given Electrochemical Cell**
The diagram illustrates a galvanic (voltaic) cell, consisting of two half-cells connected by a salt bridge. The components of this electrochemical cell are detailed below:
### Components:
- **Left Half-Cell:**
- **Electrode:** A platinum (Pt) electrode, used as an inert conductor.
- **Solutions/Compounds:**
- Potassium chloride (\(\text{KCl(aq)}\)) is the electrolyte.
- Mercurous chloride (\(\text{Hg}_2\text{Cl}_2(s)\)) is a solid.
- Elemental mercury (\(\text{Hg(l)}\)), which is in liquid form.
- **Right Half-Cell:**
- **Electrode:** Zinc (\(\text{Zn}\)) metal.
- **Solution:** Zinc chloride (\(\text{ZnCl}_2(aq)\)) serving as the electrolyte.
### Connections:
- An external circuit connects the two electrodes shown by the wires leading from the \(-\) terminal (left) to the \(+\) terminal (right) through a voltmeter (V), allowing electron flow.
- A salt bridge is included between the two solutions to maintain electrical neutrality by allowing the migration of ions.
### Cell Diagram:
The cell diagram, representing the reaction occurring in the galvanic cell, is written as follows:
\[
\text{Pt} | \text{Hg}_2\text{Cl}_2(\text{s}) | \text{Hg}(\text{l}) || \text{ZnCl}_2(\text{aq}) | \text{Zn}
\]
**Explanation:**
- The single vertical lines (\(|\)) represent phase boundaries.
- The double vertical line (\(||\)) signifies the salt bridge separating the two half-cells.
- The left side denotes the anode side (oxidation occurs, \(-\) electrode).
- The right side denotes the cathode side (reduction occurs, \(+\) electrode).
This cell generates electrical energy through a spontaneous redox reaction, which can be measured with the voltmeter in the circuit. Using a diagrammatic representation such as this is crucial for visualizing the components and reactions of galvanic cells in electrochemistry.
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