A 205.17 g sample of a solid is broken down into 120.55 g of aluminum and an unknown amount of oxygen. If a chemist wants to make 1,937 g of that solid without any leftovers, how much aluminum and oxygen should she react together?__

Hey how did you manage to type such a big lab report

I'm sorry i cant you if you don't list the elements : (

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.

Ithink that one is (c)