Given the table of standard reduction potentials E_cell Fe3+(aq) + e- --> Fe2+(a

Question

Given the table of standard reduction potentials E_cell
Fe3+(aq) + e- --> Fe2+(aq) +0.77V
Cu2+(aq) + e- --> Cu+(aq) +0.15V

Of the ions Fe3+, Fe2+, Cu2+ and Cu+, Cu+ is the best reducing agent. I need an explanation as to why this is and how I would have figured this out. Thanks!

Explanation / Answer

A reducing agent is the one that donates a pair of e-. Out of the 4 options Fe3+ and Cu2+ cannot be a reducing agent since they cannot donate e- Now the left out options are Fe2+ and Cu+ Cu+ - e- ------> Cu2+ or Cu+ ------> Cu2+ + e- ---------- (-0.15 V) and Fe2+ --------> Fe3+ + e- ------------------- ( -0.77 V) The first reaction has higher potential that is -0.15 as compared to -0.77 V hence Cu+ is a better reducing agent

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