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Consider the following half-reactions:   Hg2+(aq) + 2e– → Hg(l) E°red = +0.854 V Cu2+(aq) + 2e– → Cu(s)E°red = +0.337 V Ni2+(aq) + 2e– → Ni(s) E°red = -0.250 V Fe2+(aq) + 2e– → Fe(s) E°red = -0.440 V Zn2+(aq) + 2e– → Zn(s) E°red = -0.763 V   What is the best oxidizing agent shown above (i.e., the substance that is most likely to be reduced)?

Consider the following half-reactions:   Hg2+(aq) + 2e– → Hg(l) E°red = +0.854 V Cu2+(aq) + 2e– → Cu(s)E°red = +0.337 V Ni2+(aq) + 2e– → Ni(s) E°red = -0.250 V Fe2+(aq) + 2e– → Fe(s) E°red = -0.440 V Zn2+(aq) + 2e– → Zn(s) E°red = -0.763 V   What is the best oxidizing agent shown above (i.e., the substance that is most likely to be reduced)?

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.8: Counting Electrons
Problem 1RC: 1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how...
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  • Consider the following half-reactions:

 

Hg2+(aq) + 2e– → Hg(l) E°red = +0.854 V

Cu2+(aq) + 2e– → Cu(s)E°red = +0.337 V

Ni2+(aq) + 2e– → Ni(s) E°red = -0.250 V

Fe2+(aq) + 2e– → Fe(s) E°red = -0.440 V

Zn2+(aq) + 2e– → Zn(s) E°red = -0.763 V

 

  1. What is the best oxidizing agent shown above (i.e., the substance that is most likely to be reduced)?
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