**Cathode Reaction of the Cell:**- Write a balanced equation for the half-reaction that occurs at the cathode.**Anode Reaction of the Cell:**- Write a balanced equation for the half-reaction that occurs at the anode.**Substance Composition:**- Of what substance is \( E_1 \) made?- Of what substance is \( E_2 \) made?**Chemical Species in Solutions:**- What are the chemical species in solution \( S_1 \)?- What are the chemical species in solution \( S_2 \)? ### Galvanic Cell Reaction**Chemical Reaction:**\[ \text{Zn(s)} + \text{NiSO}_4\text{(aq)} \rightarrow \text{ZnSO}_4\text{(aq)} + \text{Ni(s)} \]**Diagram Explanation:**The diagram illustrates a galvanic cell setup consisting of two half-cells linked by a salt bridge.- **Half-Cell Descriptions:** - **Left Beaker (S1):** Contains a zinc electrode (E1) submerged in a solution of zinc sulfate. This is the anode, where oxidation occurs, releasing electrons into the solution. - **Right Beaker (S2):** Contains a nickel electrode (E2) submerged in a solution of nickel sulfate. This is the cathode, where reduction takes place as nickel ions gain electrons to form solid nickel.- **Electron Flow:** - Electrons flow from the zinc electrode to the nickel electrode through an external wire, indicating conventional current direction. This electron flow is shown by green arrows labeled \( e^- \).- **Salt Bridge:** - The two solutions are connected by a salt bridge, which allows the flow of ions to maintain charge balance. The salt bridge is depicted as a horizontal grey tube connecting the two beakers.- **Voltmeter:** - A voltmeter is connected in the circuit to measure the voltage difference between the two electrodes.This setup demonstrates the spontaneous redox reaction between zinc and nickel sulfate, converting chemical energy into electrical energy.

Answered: Image /qna-images/answer/b8313c7f-f67a-4b0d-bac0-7f839a31ce15.jpg

Answered: Suppose the galvanic cell sketched…

Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+NiSO4(aq) ZnSO4(aq)+Ni(s) E1 S1 → 1.1 E2 S2

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

A galvanic cell is powered by the following redox reaction: 2+ + 3 Cu²+ (aq) + Cr(OH)3(s) + 5OH¯(aq) → 3 Cut (aq) + Cro (aq) + 4H₂O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 0 E = v V ロ→ロ X 5
Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq) + 2 e– → Fe(s); E° = –0.41 V Pt2+(aq) + 2 e– → Pt(s); E° = 1.18 V Cr2O72–(aq) + 14 H+(aq) + 6 e– → 2 Cr3+(aq) + 7 H2O(); E° = 1.33 V Which of the following is the strongest oxidizing agent? Fe Pt Cr^3+ Fe^2+ Cr2O7^2-
Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 A£NO3(aq) → Cu(NO,),(aq)+2 Ag(s) E1 E2 sí S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. O-0 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? O DD
Consider these two entries from a fictional table of standard reduction potentials. X+ (aq) + e¯ Y+ (aq) + e- →Y(s) E = 2.01 V →X(s) O X and Y O X+ and Y+ O X and Y+ O X+ and Y E = 2.62 V Which pair of species will react under standard conditions at 25 °C?
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction + 21O3(aq)+ 12 H¹ (aq)+10e¯ Cl₂(g) +2e 1₂(s) + 6H₂O(1) → 2 C1 (aq) standard reduction potential E=+1.195 V 'red E 70 = +1.359 V red
This galvanic cell uses the reaction: Cu(s) + 2 Ag*(aq) → 2 Ag(s) + Cu2+(aq). f a C oxidation half cell reduction half cell Identify the composition of electrodes and the direction of electron flow. O a is Ag, c is Cu and electrons flow from c to a O a is Ag, c is Cu and electrons flow from a to c O a is Cu, c is Ag and electrons flow from c to a. O a is Cu, c is Ag and electrons flow from a to c. an
Consider the following standard reduction potentials: Zn2*(aq) + 2 e → Zn(s) E° = -0.76 V Mg2*(aq) + 2 e → Mg(s) E° = -2.37 V Ag*(aq) + e → Ag(s) E° = +0.80 V Which is the strongest oxidizing agent? Mg2*(aq) Zn2*(aq) Ag*(aq) 5:08 PM 90°F Partly sunny P Type here to search 8/6/2021
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V
Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- → Mt (s), and R2+ (aq) + 2 e1- → R (s), have standard reduction potentials of 1.09 V and 0.34 V respectively