44) Use the Nernst equation to determine Ecell at 25°C for the following voltaic cell.(E° cell = +1.100 V)Zn (s) / Zn2+ (0.10 M) // Cu2+ (1.0 M) / Cu (s)A) 1.10B) 1.07C) 1.17D) 1.04E) 1.16

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Answered: 44) Use the Nernst equation to…

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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Consider the following line notation: Cu(s)│Cu(NO3)2 (aq) (0.00678 M)║ Al(NO3)3 (aq) (0.00345M)│Al(s) Calculate E for this electrochemical cell set up ignoring activity coefficients. Recalculate E for the electrochemical cell with activity coefficients. (
5) For this problem refer to the electrochemical cell below a) Which electrode is the cathode and which is the anode? b) Is this cell electrolytic or galvanic? Explain. c) If the concentration of dissolved zinc ions were increased, how would this change the measured voltage? Volumeter so so; Znisi - Zntag) - 2e Cagl + 2e -Cuis)
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Enter electrons as e A voltaic cell is constructed from a standard Zn2+ Zn half cell (E°red= -0.763V) and a standard Br₂ Bri half cell (Ered 1.080V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is Submit Answer (sky Another Vorstan
8

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44) Use the Nernst equation to determine Ecell at 25°C for the following voltaic cell. (E° cell = +1.100 V) Zn (s) / Zn2+ (0.10 M) // Cu2+ (1.0 M) / Cu (s) A) 1.10 B) 1.07 C) 1.17 D) 1.04 E) 1.16