An electrochemical cell is based on the following two half-reactions: Oxidation: Pb(s) → Pb²+ (aq, 0.28 M) + 2e¯, Eº = -0.13 V Reduction: MnO4¯¯ (aq, 1.80 M) + 4H+ (aq, 2.3 M) +3e¯ → MnO₂ (s) + 2H₂O(1), E° = 1.68 V Part A Compute the cell potential at 25 °C. Express the cell potential in volts to three significant figures. 17 ΑΣΦ Ecell = 1.8 Submit Previous Answers Request Answer ? V X Incorrect; Try Again; 4 attempts remaining Begin by calculating the standard cell potential using the Eº values of both half-reactions. Then use the Nernst equation to calculate the cell potential at 25 °C: Ecell = E cell where Ecell is the cell potential in volts, E cell is the standard cell potential in volts, n is the number of moles of electrons transferred in the redox reaction, and is the reaction quotient. 0.0592 V n -log Q

An electrochemical cell is based on the following two half-reactions: Oxidation: Pb(s) → Pb²+ (aq, 0.28 M) + 2e¯, Eº = -0.13 V Reduction: MnO4¯¯ (aq, 1.80 M) + 4H+ (aq, 2.3 M) +3e¯ → MnO₂ (s) + 2H₂O(1), E° = 1.68 V Part A Compute the cell potential at 25 °C. Express the cell potential in volts to three significant figures. 17 ΑΣΦ Ecell = 1.8 Submit Previous Answers Request Answer ? V X Incorrect; Try Again; 4 attempts remaining Begin by calculating the standard cell potential using the Eº values of both half-reactions. Then use the Nernst equation to calculate the cell potential at 25 °C: Ecell = E cell where Ecell is the cell potential in volts, E cell is the standard cell potential in volts, n is the number of moles of electrons transferred in the redox reaction, and is the reaction quotient. 0.0592 V n -log Q

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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