Consider the electrochemical cell at 35°C that has a redox reaction below: Zn(s) + A1³+ (aq) "(aq) + Al(s) The concentration of Al³+ is 0.200 M and Zn²+ is 0.125 M → Zn²+, Al³+ (aq) + 3e → Al(s) Zn²+ + 2e → Zn(s) (aq) note: R = 8.314 J/K mol T = 273.15 + °C F = 96500 C/mol Eº = -1.66 V Eº = -0.76 V (a) How many electrons were transferred in the electrochemical cell? (b) Calculate for the STANDARD Ecell. Express your answer in TWO DECIMAL places. (c) Use Nernst equation and calculate for the Ecell. Express your answer in three significant figures

Consider the electrochemical cell at 35°C that has a redox reaction below: Zn(s) + A1³+ (aq) "(aq) + Al(s) The concentration of Al³+ is 0.200 M and Zn²+ is 0.125 M → Zn²+, Al³+ (aq) + 3e → Al(s) Zn²+ + 2e → Zn(s) (aq) note: R = 8.314 J/K mol T = 273.15 + °C F = 96500 C/mol Eº = -1.66 V Eº = -0.76 V (a) How many electrons were transferred in the electrochemical cell? (b) Calculate for the STANDARD Ecell. Express your answer in TWO DECIMAL places. (c) Use Nernst equation and calculate for the Ecell. Express your answer in three significant figures

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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