Cu 2+/Cu=.34v Ag +/Ag=.8v Co 2+/Co=-.28v Nt 2+/Nt=/1.1v Zn 2+/Zn=-.76v Based on

Question

Cu 2+/Cu=.34v Ag +/Ag=.8v Co 2+/Co=-.28v Nt 2+/Nt=/1.1v Zn 2+/Zn=-.76v
Based on the data above , why is Zn (s) the best reducing agent?
How do you do this and HOW do you know. HEL Cu 2+/Cu=.34v Ag +/Ag=.8v Co 2+/Co=-.28v Nt 2+/Nt=/1.1v Zn 2+/Zn=-.76v

How do you do this and HOW do you know. HEL

Explanation / Answer

A reducing agent is the species that is oxidized (or gains positivecharge) the easiest. If you flip the Zn2+/Zn reaction around you get Zn --> Zn2+ + 2e-    with E=+.76v (note that thesign changes when you flip it around) If you flip all the reactions that have negative symbols, Zn(S)will have the highest E when the species is being oxidized. Nt2+ does have the highest E but it is being reduced (from 2+ to 0)so it is an oxidizing agent.

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