In order for a reaction to happen spontaneously, which reaction (oxidation or reduction) needs to be higher on the redox table? Why?

Answer 1

Not sure what you mean by the "redox table". There are tables for standard reduction potentials, standard oxidation potentials and activity of metals, but I'm not familiar with oxidation reduction tables. If using the standard reduction potentials, a reaction will occur if the element being reduced is higher, and vice versa for the standard oxidation potential table. For example, if you had Cu(s) + ZnCl₂(aq), no reaction will occur, but if you have Cu(s) + ZnCl₂, then you will get a spontaneous redox reaction.

Not sure this answers your question, but hopefully points you in the right direction.