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+] = 0.060 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 × 10ªPart: 0 / 3Part 1 of 3Eº-2.220 Vx10xJV.mol'S

Answer: In the galvanic cell oxidation always takes place at anode and reduction always takes place…

Calculate Eº, 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+] = 0.060 M. Round each of your answers to 4 significant digits. 2+ Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 104 J V.mol

Calculate Eº, 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+] = 0.060 M. Round each of your answers to 4 significant digits. 2+ Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 104 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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Calculate the cell potential for the reaction as written at 25.00 degrees * C , given that [Zn^ 2+ ]=0.81 and [Sn^ 2+ ]=0.0190M M. Use the standard reduction potentials in this table. Zn(s)+ Sn ^ 2+ (aq) rightleftharpoons Zn^ 2+ (aq)+Sn(s)
Cu = reduction potential of +0.52. Mg is in pic. Thanks
Calculate the K and AG for the following reaction at 25 °C: Mg(s) + Pb2+(aq)=Mg2+(aq) + Pb (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Кс Part 2 of 2 G Round your answer to 4 significant digits. AG° kJ mol
Calculate Eº, E, and AG for the following cell reaction: 2+ 2+ Mg(s) + Sn²+ (aq) = Mg²+ (aq) + Sn (s) 2+ 2 where [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 × 10ª Part: 0 / 3 Part 1 of 3 Eº = v V x10 J V. mol S I
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2+ Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² ]=0.761 Mand [Ni²+]=0.0180 M. Use the standard reduction potentials from the 2+ appendix in the book. 2+ ↔ Mg²+ (aq) + Ni(s) Give the numeric value only assuming a measurement in V Mg(s) + Ni²+ (aq) → 2+ (aq)
Based on the sign of the standard cell potential, El classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Ni² (aq) + S² (aq) - Ni(s) + S(s) Answer Bank Al (aq) + 3 Na(s) Al(s) + 3 Na+ (aq) Nonspontaneous as written Pb (aq) + H₂(g)- Pb(s) + 2 H+ (aq)
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