Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. Pb KCl(aq) Anode half-reaction: PbCl₂(s) Cathode half-reaction: | + 2CF = +2e¯ + 2 e Shorthand notation: V C راه + 2 CI™ AgCl(s) Ag KCl(aq)
Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. Pb KCl(aq) Anode half-reaction: PbCl₂(s) Cathode half-reaction: | + 2CF = +2e¯ + 2 e Shorthand notation: V C راه + 2 CI™ AgCl(s) Ag KCl(aq)
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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![**Image Transcription for Educational Website**
**Title: Electrochemical Cell Reactions**
In the diagram, an electrochemical cell setup is depicted with two beakers connected by a salt bridge. The left beaker contains a lead (Pb) electrode immersed in lead(II) chloride (PbCl₂) and potassium chloride (KCl) aqueous solution, serving as the anode. The right beaker contains a silver (Ag) electrode immersed in silver chloride (AgCl) and potassium chloride (KCl) aqueous solution, serving as the cathode. The setup includes an external circuit with a voltmeter connecting the two electrodes.
**Anode Reaction:**
\[ \text{___} + 2 \text{Cl}^- \rightarrow \text{___} + 2 \text{e}^- \]
**Cathode Reaction:**
\[ \text{___} + 2 \text{e}^- \rightarrow \text{___} + 2 \text{Cl}^- \]
**Shorthand Notation for the Cell:**
\[ \text{[ ]} \ | \ \text{[ ]} \ || \ \text{[ ]} \ | \ \text{[ ]} \]
**Answer Bank**:
- 2 Ag(s)
- Cl⁻ (aq)
- 2 AgCl(s)
- Ag(s)
- AgCl(s)
- PbCl₂(s)
- Pb(s)
Users are prompted to fill in the blanks using options from the answer bank to complete the half-reactions at the anode and cathode, as well as to write the shorthand notation for the electrochemical cell.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf8dd5bb-1368-4a10-9929-9294802d0b74%2F395103c2-941c-4ba8-ba1e-27f0c6a9aa19%2Fg2ca06f_processed.png&w=3840&q=75)
Transcribed Image Text:**Image Transcription for Educational Website**
**Title: Electrochemical Cell Reactions**
In the diagram, an electrochemical cell setup is depicted with two beakers connected by a salt bridge. The left beaker contains a lead (Pb) electrode immersed in lead(II) chloride (PbCl₂) and potassium chloride (KCl) aqueous solution, serving as the anode. The right beaker contains a silver (Ag) electrode immersed in silver chloride (AgCl) and potassium chloride (KCl) aqueous solution, serving as the cathode. The setup includes an external circuit with a voltmeter connecting the two electrodes.
**Anode Reaction:**
\[ \text{___} + 2 \text{Cl}^- \rightarrow \text{___} + 2 \text{e}^- \]
**Cathode Reaction:**
\[ \text{___} + 2 \text{e}^- \rightarrow \text{___} + 2 \text{Cl}^- \]
**Shorthand Notation for the Cell:**
\[ \text{[ ]} \ | \ \text{[ ]} \ || \ \text{[ ]} \ | \ \text{[ ]} \]
**Answer Bank**:
- 2 Ag(s)
- Cl⁻ (aq)
- 2 AgCl(s)
- Ag(s)
- AgCl(s)
- PbCl₂(s)
- Pb(s)
Users are prompted to fill in the blanks using options from the answer bank to complete the half-reactions at the anode and cathode, as well as to write the shorthand notation for the electrochemical cell.
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