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Label the diagram according to the components and processes of a voltaic cell. Drag the appropriate labels to their respective targets. ▸ View Available Hint(s) Oxidation half- cell Zinc Cathode Zinc Anode Copper Cathode Flow of cations Flow of anions Copper Anode Flow of electrons Reduction half- cell 1.10 Salt Bridge Zn2+ CU Z 5042 Cu2+ S02 Zn(s) Zn²+(aq) +2e Cu2+ (aq) +2e+Cu(s) Reset ||| Help

Label the diagram according to the components and processes of a voltaic cell. Drag the appropriate labels to their respective targets. ▸ View Available Hint(s) Oxidation half- cell Zinc Cathode Zinc Anode Copper Cathode Flow of cations Flow of anions Copper Anode Flow of electrons Reduction half- cell 1.10 Salt Bridge Zn2+ CU Z 5042 Cu2+ S02 Zn(s) Zn²+(aq) +2e Cu2+ (aq) +2e+Cu(s) Reset ||| Help

Chemistry
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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Part A Label the diagram according to the components and processes of a voltaic cell. Drag the appropriate labels to their respective targets. ▸ View Available Hint(s) Oxidation half- cell Zinc Cathode Zinc Anode Copper Cathode Flow of cations Flow of anions Copper Anode Flow of electrons Reduction half- cell 1.10 SO₂² 2N* Salt Bridge Zn2+ Zn2+ SO42 Zn(s) → Zn²+ (aq) +2e C2+ Cu2+ S0₂2 Cu2+ (aq) +2e+ Cu(s) Reset Help
Transcribed Image Text:Part A Label the diagram according to the components and processes of a voltaic cell. Drag the appropriate labels to their respective targets. ▸ View Available Hint(s) Oxidation half- cell Zinc Cathode Zinc Anode Copper Cathode Flow of cations Flow of anions Copper Anode Flow of electrons Reduction half- cell 1.10 SO₂² 2N* Salt Bridge Zn2+ Zn2+ SO42 Zn(s) → Zn²+ (aq) +2e C2+ Cu2+ S0₂2 Cu2+ (aq) +2e+ Cu(s) Reset Help
Animation-Analysis of Copper-Zinc Voltaic Cell Zinc Some oxidation-reduction reactions are spontaneous, and the energy released by them can be used for electrical work. This principle is used in the working of a voltaic cell. Voltaic cells, or electrochemical cells, make use of the electrons that are transferred from the species that releases electrons and undergoes oxidation to the species that accepts electrons and undergoes reduction. If it is possible by any means to separate the oxidation reaction and the reduction reaction and then connect them externally so that the electrons flow from one compartment to the other, you can construct an electrochemical cell. Watch the video that describes the cell reaction and the cell components of a voltaic cell. 1.10 14 of 42 Na₂SO₂(aq) Review | Constants | Periodic Table Z 5042 Cu2+ $0,² In a copper-zinc voltaic cell, one half-cell consists of a Zn electrode inserted in a solution of zinc sulfate and the other half-cell consists of a Cu electrode inserted in a copper sulfate solution. These two half-cells are separated by a salt bridge. At the zinc electrode (anode), Zn metal undergoes oxidation y losing two electrons and enters the solution as Zn²+ ions. The oxidation half-cell reaction that takes place at the anode is Zn(s) Zn²+ (aq) + 20 The Cu ions undergo reduction by accepting two electrons from the copper electrode (cathode) and depositing on the electrode as Cu(s). The reduction half-cell reaction that takes place at the cathode is Cu²+ (aq) +2e Cu(s) The electrons lost by the Zn metal are gained by the Cu ion. The transfer of electrons between Zu metal and Cu ions is made possible by connecting the wire between the Zn electrode and the Cu electrode. Thus, in the voltaic cell, the electrons flow through an external circuit from the anode to the cathode. For a voltaic cell to work, the solution in the two half-cells must remain electrically neutral. This can happen only if the flow of ions is countered with the flow of electrons. The flow of ions is made possible with the use of a salt bridge. A salt bridge is a solution of some other metal that has common ions. If a copper-zinc voltaic cell utilizes ZnSO, and CuSO, solution, you will use a saturated Na2SO, solution in the salt bridge. Thus, the salt bridge will help the migration of ions across the two compartments, or two half-cells.
Transcribed Image Text:Animation-Analysis of Copper-Zinc Voltaic Cell Zinc Some oxidation-reduction reactions are spontaneous, and the energy released by them can be used for electrical work. This principle is used in the working of a voltaic cell. Voltaic cells, or electrochemical cells, make use of the electrons that are transferred from the species that releases electrons and undergoes oxidation to the species that accepts electrons and undergoes reduction. If it is possible by any means to separate the oxidation reaction and the reduction reaction and then connect them externally so that the electrons flow from one compartment to the other, you can construct an electrochemical cell. Watch the video that describes the cell reaction and the cell components of a voltaic cell. 1.10 14 of 42 Na₂SO₂(aq) Review | Constants | Periodic Table Z 5042 Cu2+ $0,² In a copper-zinc voltaic cell, one half-cell consists of a Zn electrode inserted in a solution of zinc sulfate and the other half-cell consists of a Cu electrode inserted in a copper sulfate solution. These two half-cells are separated by a salt bridge. At the zinc electrode (anode), Zn metal undergoes oxidation y losing two electrons and enters the solution as Zn²+ ions. The oxidation half-cell reaction that takes place at the anode is Zn(s) Zn²+ (aq) + 20 The Cu ions undergo reduction by accepting two electrons from the copper electrode (cathode) and depositing on the electrode as Cu(s). The reduction half-cell reaction that takes place at the cathode is Cu²+ (aq) +2e Cu(s) The electrons lost by the Zn metal are gained by the Cu ion. The transfer of electrons between Zu metal and Cu ions is made possible by connecting the wire between the Zn electrode and the Cu electrode. Thus, in the voltaic cell, the electrons flow through an external circuit from the anode to the cathode. For a voltaic cell to work, the solution in the two half-cells must remain electrically neutral. This can happen only if the flow of ions is countered with the flow of electrons. The flow of ions is made possible with the use of a salt bridge. A salt bridge is a solution of some other metal that has common ions. If a copper-zinc voltaic cell utilizes ZnSO, and CuSO, solution, you will use a saturated Na2SO, solution in the salt bridge. Thus, the salt bridge will help the migration of ions across the two compartments, or two half-cells.
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