**Instructions for Completing the Table**1. **Write a balanced equation for the half-reaction that happens at the cathode of this cell.** - [Your answer here]2. **Write a balanced equation for the half-reaction that happens at the anode of this cell.** - [Your answer here]3. **Of what substance is \(E_1\) made?** - [Your answer here]4. **Of what substance is \(E_2\) made?** - [Your answer here]5. **What are the chemical species in solution \(S_1\)?** - [Your answer here]6. **What are the chemical species in solution \(S_2\)?** - [Your answer here]The table above is designed to gather information about electrochemical reactions, specifically focusing on reactions occurring within an electrochemical cell. Students are asked to identify substances and chemical species involved in the process. The image illustrates a galvanic cell powered by the reaction: Zn(s) + NiSO₄(aq) → ZnSO₄(aq) + Ni(s).**Description of the Diagram:**- **Left Half-Cell (E1, S1):** - The left beaker contains a zinc electrode (E1) submerged in a zinc sulfate solution (S1). - This half-cell acts as the anode where oxidation occurs, releasing electrons (e⁻).- **Right Half-Cell (E2, S2):** - The right beaker contains a nickel electrode (E2) submerged in a nickel sulfate solution (S2). - This half-cell acts as the cathode where reduction takes place, gaining electrons (e⁻).- **External Circuit:** - A voltmeter is connected between the two electrodes, completing the external circuit and allowing electron flow from the anode to the cathode.- **Salt Bridge:** - A salt bridge connects the two solutions, maintaining ionic balance by allowing the flow of ions.In this electrochemical cell, zinc is oxidized, and nickel ions are reduced, resulting in the flow of electrons through the external circuit, providing electrical energy.

Answered: Image /qna-images/answer/1875fdf1-450f-4b08-8eba-27ce89c1240d.jpg

Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? 0 0 0 0

Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? 0 0 0 0

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...

See similar textbooks

Similar questions

Illustrate how electrochemical cell can be used as an alternative source of energy. Give examples.
Suppose the galvanic cell sketched below is powered by the following reaction: Mn(s) + SnCl2(aq) →>> E1 MnCl2(aq) + Sn(s) e- E2 S1 S2
Consider a galvanic electrochemical cell constructed using Cr/Cr³+ and Zn/Zn²+ at 25 °C. The following half-reactions are provided for each metal: Cr³+(aq) + 3 e →→ Cr(s) E°red = -0.744 V Zn²+ (aq) + 2 e →→ Zn(s) Eºred = -0.763 V Write the balanced equation for the overall reaction in acidic solution. 3 Zn(s) + 2 Cr³+ (aq) → 3 Zn²+(aq) + 2 Cr (s) 1 1 + 4- Reset 2 H₂O+ 0 3_ ( ) 3 03 04 4 H H+ 5 5 11 Zn 6 6 ²+ 7 07 (s) H₂O ● 3+ (1) 8 9 0 e 4+ x H₂O 9 (g) (aq) □o Cr Delete
A concentration cell consists of two Sn/Sn2+ half-cells. The electrolyte in compartment A is 0.21 M Sn(NO3)2. The electrolyte in B is 0.87 M Sn(NO3)2. Which half-cell houses the cathode? What is the voltage of the cell? Cathode: half-cell A half-cell B Voltage of cell: V
Explain the working of a Fuel cell and list the different types of Fuel cells with brief explanation of each type.
Match the components of an electrochemical cell with the appropriate function. Words: Voltmeter Cathode Anode Porous Bridge Electrode Definitions: Allows flow of ions that neutralize the charge buildup Measures the difference in electric potential as voltage Conductive surfaces through which electrons can enter or leave the half-cells Electrode where the reduction takes place Electrode where oxidation takes place
2.Write a balanced cell reaction. Include the phases of all species in the chemical equation.
A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.
Try Again Your answer is incorrect. Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+ SnSO4(aq) → NiSO4(aq) + Sn(s) E1 S1 Write a balanced equation for the half-reaction that happens at the cathode of this cell. E2 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? S2 2+ Sn (aq) + 2e Sn (s) 2+ Ni (s) → Ni²+ (aq) + 2e Nielectrode Snelectrode ロ→ロ 0,0,... X Ś
Use line notation to represent each electrochemical cell below a. 2Ag+(aq)+Pb(s)→2 Ag(s)+Pb2+(aq) b. 2ClO2(g)+2 I−(aq)→2 ClO2−(aq)+I2(s) c. O2(g)+4 H+(aq)+2 Zn(s)→2 H2O(l)+2 Zn2+(aq)
Would you expect delta ΔH° to be negative or positive for a voltaic cell? Briefly explain why. Think about the equation ΔG = ΔH – TΔS and the sign of ΔG for this type of cell.