[aaliyah.011]

Given these half-reactions, which can oxidize Pb(s)? There is 2 answers

Ag+ (aq) + e- -->Ag (s) where Eo=+0.80 V

Cu2+(aq)+2e- -->Cu(s) where Eo=+0.34 V

Pb2+(aq)+2e- -->Pb(s) where Eo= -0.13 V

Fe2+(aq) +2e- -->Fe(s) where Eo= -0.44 V

Al3+ (aq)+ 3e --> Al(s) where Eo= -0.166 V



I am not sure how to approach this problem or even where to start. Here is what I know: oxidation is losing electrons, the Eo is electric potential and the half reaction takes into consideration the change in oxidation state, the electrons have to be balanced and two half reactions are put together for one reaction. Is it trial and error to see what happens when this is done? I truly don't know how to do this problem so if someone could walk me through the steps it would be helpful so I have an understanding of the concept. I have tried similar problems as practice as well with no luck.

[Borek]

Hint: it is all about oxidation potentials.

[Babcock_Hall]

I like to think of oxidation potentials as describing how much the oxidized form wants to have an electron.