Given the following half-reactions: 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

Which can oxidize Pb(s)? Hint: there is 2 answers

I have tried to work on similar problems to this but am confused, I know the oxidation states matter as well as the elements involved but I have no clue how to solve. Please explain how to approach these types of problems

Suppose a pair of chemical compounds a and b can react in two different ways: a + b -> c reaction 1 gives product c. a + b -> d reaction 2 gives product d. the following facts are known about the two reactions: . reaction 1 is endothermic and reaction 2 is exothermic. if a reaction vessel is charged (filled) with a and b , then at first d is produced faster than c. use these facts to sketch a qualitative reaction energy diagram for both reactions. note: because these sketches are only qualitative, the energies don? t have to be exact. they only have to have the right relationship to each other. for example, if one energy is less than another, that fact should be clear in your sketch.