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Write the reduction half-reaction for each half-cell. + V KCI(aq) Hg,Cl2(s) Pt Hg() ZNCI2(aq) Zn

Write the reduction half-reaction for each half-cell. + V KCI(aq) Hg,Cl2(s) Pt Hg() ZNCI2(aq) Zn

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter20: Electrochemistry
Section: Chapter Questions
Problem 49A
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### Galvanic Cell Diagram Explanation This diagram represents a galvanic cell composed of two half-cells, each playing a crucial role in redox reactions. The specific task is to write the reduction half-reaction for each half-cell. #### Left Half-Cell: - **Components:** - **KCl(aq):** An aqueous solution of potassium chloride. - **Hg₂Cl₂(s):** Solid mercury(I) chloride. - **Pt:** Platinum electrode. - **Hg(I):** Mercury in the +1 oxidation state. - **Explanation:** - The left half-cell contains a saturated solution of KCl and solid Hg₂Cl₂. The platinum electrode serves as an inert conductor for the electron transfer process. The reduction likely involves the reduction of Hg(I) ions. #### Right Half-Cell: - **Components:** - **ZnCl₂(aq):** An aqueous solution of zinc chloride. - **Zn:** Solid zinc electrode. - **Explanation:** - The right half-cell contains a solution of ZnCl₂ with a zinc metal electrode. The zinc electrode acts as a source of Zn²⁺ ions through oxidation, and this half-cell likely involves the reduction of Zn²⁺ ions. #### Circuit Details: - **Voltmeter (V):** The voltmeter is connected across the half-cells to measure the cell potential. The negative and positive terminals of the voltmeter indicate the flow direction of electrons. - **Salt Bridge:** The diagram includes a salt bridge that allows for ion flow between the two half-cells, maintaining electrical neutrality as the reactions proceed. ### Instructions: - Write the reduction half-reaction for each of the half-cells based on the components provided.
Transcribed Image Text:### Galvanic Cell Diagram Explanation This diagram represents a galvanic cell composed of two half-cells, each playing a crucial role in redox reactions. The specific task is to write the reduction half-reaction for each half-cell. #### Left Half-Cell: - **Components:** - **KCl(aq):** An aqueous solution of potassium chloride. - **Hg₂Cl₂(s):** Solid mercury(I) chloride. - **Pt:** Platinum electrode. - **Hg(I):** Mercury in the +1 oxidation state. - **Explanation:** - The left half-cell contains a saturated solution of KCl and solid Hg₂Cl₂. The platinum electrode serves as an inert conductor for the electron transfer process. The reduction likely involves the reduction of Hg(I) ions. #### Right Half-Cell: - **Components:** - **ZnCl₂(aq):** An aqueous solution of zinc chloride. - **Zn:** Solid zinc electrode. - **Explanation:** - The right half-cell contains a solution of ZnCl₂ with a zinc metal electrode. The zinc electrode acts as a source of Zn²⁺ ions through oxidation, and this half-cell likely involves the reduction of Zn²⁺ ions. #### Circuit Details: - **Voltmeter (V):** The voltmeter is connected across the half-cells to measure the cell potential. The negative and positive terminals of the voltmeter indicate the flow direction of electrons. - **Salt Bridge:** The diagram includes a salt bridge that allows for ion flow between the two half-cells, maintaining electrical neutrality as the reactions proceed. ### Instructions: - Write the reduction half-reaction for each of the half-cells based on the components provided.
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