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

Aspirin has a density of 1.40 g/cm3 what is the volume in cubic centimeters of a tablet weighing 320 mg ?

The following reaction shows the products when sulfuric acid and aluminum hydroxide react. al(oh)3 + h2so4 → al2(so4)3 + h2o the table shows the calculated amounts of reactants and products when the reaction was conducted in a laboratory. sulfuric acid aluminum hydroxide initial amount of reactant 40 g 15 g theoretical yield of water from reactant 14.69 g 10.38 g what is the approximate amount of the leftover reactant? 11.73 g of sulfuric acid 10.33 g of sulfuric acid 11.12 g of aluminum hydroxide 13.67 g of aluminum hydroxide

Amixture with the same composition throughout is!