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500 mL 450 - 100 25 See Molecular Scale 500 mL - 100 See Molecular Scale

500 mL 450 - 100 25 See Molecular Scale 500 mL - 100 See Molecular Scale

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter7: Statistical Data Treatment And Evaluation
Section: Chapter Questions
Problem 7.10QAP
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Redox is a type of chemical reaction in which the oxidation states of the substrate change. Electrons will move from the right electrode to the left. Describe the role/what happens to copper and silver in the redox process. Copper is in the left beaker and silver is in the right. Example attached
A voltaic cell is a device that converts the chemical energy of a spontaneous redox reaction into electrical energy. Let's consider Zinc and copper, copper is in the left beaker and zinc is in the right beaker. The anode is an electrode where oxidation occurs. The cathode is an electrode where reduction occurs. The zinc electrode is located in the anode and the cu electrode is located in the cathode. In a redox reaction, the reducing agent loses electrons and the oxidizing agent gains electrons. In this case, Zinc metal is the reducing agent because it loses electrons. In this case, zinc metal is the reducing agent because it loses electrons and gets oxidized to the Zn2+ ion. Cu2+ ion is an oxidizing agent because it gains electrons and gets reduced to Cu metal. Elemental zinc has an oxidation state of zero and loses two electrons which raises its oxidation state to +2. Cu2+ ion has an oxidation state of +2, and gains electrons from zinc, which reduces its oxidation state to zero. As zinc loses two of its electrons, it becomes ionized +2, and its ions move into the solution. At the same time, because the copper ions gain two electrons, they become neutral copper metal, which is deposited on the surface of the zinc. Zinc metal dissolves the electrolyte during the reaction and the Zn sheet thins. Oxidation half-reactions are represented as follows: Zn0 ➜ Zn+2+2e- (reducing agent). The reduction half-reaction is represented as follows: Cu+2+2e-→ Cu (oxidizing agent).
Transcribed Image Text:A voltaic cell is a device that converts the chemical energy of a spontaneous redox reaction into electrical energy. Let's consider Zinc and copper, copper is in the left beaker and zinc is in the right beaker. The anode is an electrode where oxidation occurs. The cathode is an electrode where reduction occurs. The zinc electrode is located in the anode and the cu electrode is located in the cathode. In a redox reaction, the reducing agent loses electrons and the oxidizing agent gains electrons. In this case, Zinc metal is the reducing agent because it loses electrons. In this case, zinc metal is the reducing agent because it loses electrons and gets oxidized to the Zn2+ ion. Cu2+ ion is an oxidizing agent because it gains electrons and gets reduced to Cu metal. Elemental zinc has an oxidation state of zero and loses two electrons which raises its oxidation state to +2. Cu2+ ion has an oxidation state of +2, and gains electrons from zinc, which reduces its oxidation state to zero. As zinc loses two of its electrons, it becomes ionized +2, and its ions move into the solution. At the same time, because the copper ions gain two electrons, they become neutral copper metal, which is deposited on the surface of the zinc. Zinc metal dissolves the electrolyte during the reaction and the Zn sheet thins. Oxidation half-reactions are represented as follows: Zn0 ➜ Zn+2+2e- (reducing agent). The reduction half-reaction is represented as follows: Cu+2+2e-→ Cu (oxidizing agent).
- 500 mL 450 - 100 25 See Molecular Scale - 500 mL Left Beaker <-450 - 100 See Molecular Scale Experiment Set Full Reset Copper (Cu) in Cu(NO3)2 (aq)
Transcribed Image Text:- 500 mL 450 - 100 25 See Molecular Scale - 500 mL Left Beaker <-450 - 100 See Molecular Scale Experiment Set Full Reset Copper (Cu) in Cu(NO3)2 (aq)
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