**Galvanic Cell Diagram Description**This diagram illustrates a galvanic cell setup composed of two half-cells. - **Left Half-Cell (Lead Half-Cell):** - Contains a lead (Pb) electrode. - The electrolyte solution is potassium chloride (KCl) aqueous solution. - A solid lead(II) chloride (PbCl₂) precipitate is in contact with the lead electrode, indicating a reaction involving lead ions.- **Right Half-Cell (Silver Half-Cell):** - Contains a silver (Ag) electrode. - The electrolyte solution is also potassium chloride (KCl) aqueous solution. - Solid silver chloride (AgCl) is present, indicating a reaction involving silver ions.- **Salt Bridge:** - A U-shaped tube filled with electrolyte (often KCl) connects the two beakers, allowing the transfer of ions to maintain electrical neutrality.- **External Circuit:** - The setup includes an external wire connecting the Pb and Ag electrodes. A voltmeter is placed in the circuit to measure the potential difference between the electrodes. - The flow of electrons is from the lead electrode to the silver electrode through the external circuit.This setup demonstrates a typical galvanic cell, showing the electrochemical processes that occur between two metal electrodes in different electrolyte solutions, driven by their chemical reactions. ### Electrochemical Cell ReactionsComplete the half-reactions for the cell shown, and provide the shorthand notation for the cell. The electrode on the left is the anode, while the electrode on the right is the cathode.#### Anode Half-Reaction:\[ \underline{\phantom{Ag(s)}} + 2 \text{Cl}^- \rightleftharpoons \underline{\phantom{AgCl(s)}} + 2e^- \]#### Cathode Half-Reaction:\[ \underline{\phantom{PbCl_2(s)}} + 2e^- \rightleftharpoons \underline{\phantom{Pb(s)}} + 2 \text{Cl}^- \]#### Shorthand Notation:\[ \underline{\phantom{}} \,|\, \underline{\phantom{}} \,||\, \underline{\phantom{}} \,|\, \underline{\phantom{}} \]#### Answer Bank:- Ag(s)- Pb(s)- PbCl₂(s)- 2 Ag(s)- 2 AgCl(s)- Cl⁻(aq)- AgCl(s)### Explanation:- **Anode:** In electrochemical cells, the anode is where oxidation occurs. In this half-cell reaction, a solid reacts with chloride ions to form a solid compound and release electrons.- **Cathode:** The cathode is where reduction occurs. A compound gains electrons, releasing chloride ions, and forms a solid metal.- **Shorthand Notation:** This notation summarizes the entire cell reaction, separating the anode and cathode components by a double vertical line, indicating the salt bridge or membrane.### Diagram Explanation:The bottom image depicts a voltmeter connected to the electrodes, indicating that a current is flowing, which is typical for galvanic cells generating electrical energy through spontaneous redox reactions.

The electrode on the left side is anode and the electrode on right side is anode At anode oxidation of reaction takes place means loss of electron At cathode reduction will take place means gain of electron

Science

Chemistry

Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is anode, and the one on the right is the cathode. Anode half-reaction: + 2 Cl¯ 2 + 2 e- Cathode half-reaction: + 2 e- 2 + 2 Cl- Shorthand notation: Answer Bank Ag(s) Pb(s) PBCI,(s) 2 Ag(s) 2 AgCI(s) CI"(aq) AgCl(s) V

Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is anode, and the one on the right is the cathode. Anode half-reaction: + 2 Cl¯ 2 + 2 e- Cathode half-reaction: + 2 e- 2 + 2 Cl- Shorthand notation: Answer Bank Ag(s) Pb(s) PBCI,(s) 2 Ag(s) 2 AgCI(s) CI"(aq) AgCl(s) V

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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