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Vrite the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is not pontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.) ollow the general format of a cell diagram: Anode II Cathode a. Nics) + Sn²* (aq) Ni2* (aq) + Sn(s) b. Curs) + Fe2* (aq) Cu2"(ag) + Fe(s) elow are standard reduction potential: Cu2+ (aq) + 2e- Cu (s) E° = +0.34 Sn2+ (aq) + 2e- Sn (s) E° = -0.14 Ni2+ 2e- Ni (s) E° = -0.26 + Fe2* (aq)+ 2e- Fe (s) Eo = -0.45

Vrite the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is not pontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.) ollow the general format of a cell diagram: Anode II Cathode a. Nics) + Sn²* (aq) Ni2* (aq) + Sn(s) b. Curs) + Fe2* (aq) Cu2"(ag) + Fe(s) elow are standard reduction potential: Cu2+ (aq) + 2e- Cu (s) E° = +0.34 Sn2+ (aq) + 2e- Sn (s) E° = -0.14 Ni2+ 2e- Ni (s) E° = -0.26 + Fe2* (aq)+ 2e- Fe (s) Eo = -0.45

Chemistry
Chemistry
9th Edition
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Steven S. Zumdahl
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 83E: Consider a concentration cell that has both electrodes made of some metal M. Solution A in one...
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Write the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is not spontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.) Follow the general format of a cell diagram: Anode II Cathode a. Nics) + Sn2+ (aq) Ni2+ (ag) + Sn(s) b. Cu(s) + Fe2+ Cu2"(ag) + Fe(s) (ag) Below are standard reduction potential: Cu2+ (aq)+ 2e- Cu (s) E° = +0.34 Sn2+ (ag) + Sn (s) E° = -0.14 2e- Ni2+ (ag) + Ni (s) E° = -0.26 2e- Fe2* (aq) + Fe (s) Eo = -0.45 2e-
Transcribed Image Text:Write the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is not spontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.) Follow the general format of a cell diagram: Anode II Cathode a. Nics) + Sn2+ (aq) Ni2+ (ag) + Sn(s) b. Cu(s) + Fe2+ Cu2"(ag) + Fe(s) (ag) Below are standard reduction potential: Cu2+ (aq)+ 2e- Cu (s) E° = +0.34 Sn2+ (ag) + Sn (s) E° = -0.14 2e- Ni2+ (ag) + Ni (s) E° = -0.26 2e- Fe2* (aq) + Fe (s) Eo = -0.45 2e-
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