. Calculate the Gibbs free energy changes, AG, by using the potential differences measured in Part I andII by using the formula, AG = -nFɛ. n is the number of electrons transferred in the reaction. F is the Faraday'sconstant and equals to 96500 Coulomb.|3|Total cell reaction: Zn(s) + Cu"(aq) -Zn*(aq) + Cu(s)Part I. 1. Beaker: 0.1 M CUSO4 solution, 2. Beaker: 0.1M ZnSO4 solution.Part II. 1. Beaker: 0.1 M CuSO4 solution, 2. Beaker: 0.01M ZNSO4 solution.2. Find percent errors for part I and II. The theoretical value of standard cell potential, e, is 1.100 VCell >

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1. Calculate the Gibbs free energy changes, AG, by using the potential differences measured in Part I and II by using the formula, AG = -nFɛ. n is the number of electrons transferred in the reaction. F is the Faraday's constant and equals to 96500 Coulomb. Total cell reaction: Zn(s) + Cu*(aq) - - Zn*(aq) + Cu(s) Part I. 1. Beaker: 0.1 M CuSO4 solution, 2. Beaker: 0.1M ZNSO4 solution.

1. Calculate the Gibbs free energy changes, AG, by using the potential differences measured in Part I and II by using the formula, AG = -nFɛ. n is the number of electrons transferred in the reaction. F is the Faraday's constant and equals to 96500 Coulomb. Total cell reaction: Zn(s) + Cu(aq) - - Zn(aq) + Cu(s) Part I. 1. Beaker: 0.1 M CuSO4 solution, 2. Beaker: 0.1M ZNSO4 solution.

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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