**Galvanic Cell Problem Set****Problem Description:**A galvanic cell consists of a Ni/Ni²⁺ half-cell and a Co/Co²⁺ half-cell with initial concentrations: \([Ni^{2+}] = 0.80 \, M\) and \([Co^{2+}] = 0.20 \, M\) at 298.15 K.**Half-reactions and Standard Electrode Potentials:**| **Half-Reaction** | **E° (V)** ||--------------------------------------|------------|| \( Ni^{2+}(aq) + 2e^- \rightarrow Ni(s) \) | -0.25 || \( Co^{2+}(aq) + 2e^- \rightarrow Co(s) \) | -0.28 |**Question 1: Write the balanced overall reaction that powers the cell.***Provided answer:* \[ Co(s) + Ni^{2+}(aq) \rightarrow Co^{2+}(aq) + Ni(s) \]**Question 2: Calculate \( E_{cell} \) for the redox reaction. (Round to 2 decimal places)****Question 3: What is \(\left[ Ni^{2+} \right]\) when \( E_{cell} \) reaches 0.03V? (Round to 2 sig figs)**Below the questions, there are empty boxes labeled:**V** (for voltage) and **M** (for molarity) respectively, to write the answers for questions 2 and 3.**Explanation of the diagram:**- The table presents the half-reactions for Nickel and Cobalt with their respective standard electrode potentials in volts.- There is a photograph showing the handwritten balanced overall reaction.- There are two questions where learners are expected to calculate the cell potential and determine the concentration of \( Ni^{2+} \) for a given cell potential.This problem set is intended for students to apply their knowledge of electrochemistry, specifically in writing balanced reactions, calculating cell potentials, and understanding the Nernst equation.

Answered: Image /qna-images/answer/56b7fb81-04e4-404f-a393-db907d5e624d.jpg

oncentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni2+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28 Write the balanced overall reaction that powers the cell. EVE [Co(s) + Ni ²+ (aq) →) Co²+ (aq) + Ni (s) Calculate Ecell for the redox reaction. (round to 2 decimal places) What is [Ni2+] when Ecell when reaches 0.03V? (round to 2 sig figs) V

oncentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni2+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28 Write the balanced overall reaction that powers the cell. EVE [Co(s) + Ni ²+ (aq) →) Co²+ (aq) + Ni (s) Calculate Ecell for the redox reaction. (round to 2 decimal places) What is [Ni2+] when Ecell when reaches 0.03V? (round to 2 sig figs) V

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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