I don't really understand these questions and their processes. And I am a bit iffy on redox reactions. For problem 3, can you show a step by step process how to do the problem?

Question

Problem 2, I do not fully understand how to do it at all. How would you know the resulted products?
And for problem 1, can you help me go over it? Reducing and oxidizing agent..I want to understand.

1. Could you produce bromine, Br2, by the electrolysis of a CuBr2(aq) solution?

What are the products of this electrolysis at the anode? At the cathode? (Show your work).

2. Cd^2+(aq) + 2e^- ----> Cd(s)
Eo = 0.40 V
Al(OH)4^-(aq) + 3e^- ----> 4OH^-(aq) + Al(s)
Eo = -2.310 V

A galvanic cell created using the above components will have a standard cell potential, Eocell, of _______ and an overall reaction of:

Which component of the above cell

Is the best reducing agent?
Undergoes oxidation?

Is the best oxidizing agent?
Undergoes reduction?

3. Balance the following reaction in acidic solution:

PbO2(s) + Hg(l) ----> Hg2^2+ + Pb^2+

Answer 1

#1.
Br2 + 2e ==> 2Br^- written as a reduction. (Reduction is the gain of electrons and this gained e). Look in the table of standard reduction potentials (tabulated I suspect in your text). If Br2 + 2e ==> 2Br^- is more less positive than 1.23 (volts for electrolysis of H2O at that electrode), then Br2 will not be produced there. Instead you will obtain 2H2O ==> O2 + 4H^+ + 4e.
At the cathode, Cu^2+ will be attracted and will be plated out if Eo Cu is more positive than zero.