Calculate Eº, E, and AG for the following cell reaction:2+2+Mg(s) + Sn²+ (aq) = Mg²+ (aq) + Sn (s)2+2where [Mg²+] =[Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers to 4 significant digits.Note: Reference the Standard reduction potentials at 25 °C table for additional information.Note: The Faraday constant is 9.649 × 10ªPart: 0 / 3Part 1 of 3Eº = vVx10JV. molSI

We will use the Nernst equation to calculate Ecell. and using Ecell we can calculate ΔG. Ecell=Eocell-RTnFlnQ F=9.649×104JV.mol R=8.314JK-1mol-1▴G=-nFEcell The standard cell potential ofEocell(Mg2+/Mg)=-2.38vEocell(Sn2+/Sn)=-0.14vHalf cell reactions areCathode: Sn2+(aq)+2e-→Sn(s) so number of electron transfer n =2Anode: Mg(s)→Mg2+(aq)+2e-Overall reaction: Sn2+(aq) + Mg(s)→Sn(s) +Mg2+(aq)so reaction quotient Q=[Mg2+][Sn2+]=0.0400.030Cathode: Sn2+(aq)+2e-→Sn(s) Eocell(Sn2+/Sn)=-0.14v Anode: Mg(s)→Mg2+(aq)+2e- Eocell(Mg/Mg2+)=-(-2.38v)=+2.38v Overall reaction: Sn2+(aq) + Mg(s)→Sn(s) +Mg2+(aq) Eocell= Eocell(Sn2+/Sn)+ Eocell(Mg/Mg2+) = -0.14+2.38=2.24v So Eocell=2.24vNow we will use Nernst equation to calculate Ecell Ecell=Eocell-RTnFlnQ F=9.649×104JV.mol R=8.314JK-1mol-1 Ecell=2.24-8.314×298.152×9.649×104ln0.0400.030 so, Ecell=2.236V▴G=-nFEcell Ecell=2.236V, n=2▴G=-2×9.649×104×2.236▴G=-431503J =-431.5KJ So ▴G=-431.5KJ

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Chemistry

Calculate E, E, and AG for the following cell reaction: 2+ 2+ Mg(s) + Sn²+ (aq) ⇒ Mg²+ (aq) + Sn (s) where [Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers 4 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 10¹ J V.mol

Calculate E, E, and AG for the following cell reaction: 2+ 2+ Mg(s) + Sn²+ (aq) ⇒ Mg²+ (aq) + Sn (s) where [Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers 4 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 10¹ J V.mol

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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Calculate Eº, E, and AG for the following cell reaction: 2+ Mg(s) + Sn²+ (aq) ⇒ Mg²+ (aq) + Sn (s) where [Mg²+] = 0.040 M and [Sn²+] = 0.060 M. Round each of your answers to 4 significant digits. 2+ 2+ Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 10ª J V.mol
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