Reaction 1:

Cu (strongest reducing agent)
I-
Ag
Br- (weakest reducing agent)

Reaction 2:
Zn(strongestreducing agent)
Pb
Cu
Ag(weakest reducing agent)

Reaction 3:
Cl2 (strongest oxidizing agent)
Br2
I2 (wekest oxidizing agent)

Using these results, how am I supposed to prepare a single table of relative strengths of oxidizing and reducing agents?

Thanks

Reaction 1.

Cu (strongest reducing agent)
I-
Ag
Br- (weakest reducing agent)

Reaction 2:
Zn(strongestreducing agent)
Pb
Cu
Ag(weakest reducing agent)

Reaction 3:
Cl2 (strongest oxidizing agent)
Br2
I2 (wekest oxidizing agent)

Using these results, how am I supposed to prepare a single table of relative strengths of oxidizing and reducing agents?
What happens if you put 1 and 2 together?
#1.
Cu (strongest reducing agent)
I-
Ag
Br- (weakest reducing agent)
#2.
Zn(strongestreducing agent)
Pb
Cu
Ag(weakest reducing agent)

So it seems to me, forgetting #3 for the moment, that it's almost done for you.#2 tells you Zn, and Pb are at the top (above Cu and Ag) and follow that from #2 with Cu, I^-, Ag, Br^-. Then a look at #3 tells you that Br2 and I2 are already in the series as I^- and Br^-. The only one left for you to do is Cl^-. Since Cl2 is stronger than Br2 and I2, wouldn't Cl^- be the weakest of the three. Check my thinking.

One other quick note. Make sure you want to list these with the strongest reducing agent at the top and the weakest at the bottom; otherwise, you need to reverse the order.

One other quick note. Make sure you want to list these with the strongest reducing agent at the top and the weakest at the bottom; otherwise, you need to reverse the order.

So Cl2
Br2
I2

becomes

I2
Br2
Cl2

?

With them listed as

Zn
Pb
Cu etc, we are looking at the half reactions as
Zn ==> Zn^+2 + 2e
Pb ==> Pb^+2 + 2e
Cu ==> Cu^+2 + 2e
These are written as oxidations and Zn is the strongest reducing agent with Pb and Cu following in order. Written as reductions (oxidizing agents) these would be Cu^+2 + 2e ==> Cu
Pb^+2 + 2e ==> Pb.
I don't remember the instructions from the original problem so I don't know how you want them arranged. The way the tables are arranged with the reactions, I THINK (but you must be the judge of that) that Zn, Pb, Cu, Ag, etc are the way it is to be done.

To prepare a single table of relative strengths of oxidizing and reducing agents, you need to compare the reactions given and arrange the elements in order of decreasing strength for both oxidizing agents and reducing agents separately.

For oxidizing agents, observe the reactions 3:

Reaction 3:
Cl2 (strongest oxidizing agent)
Br2
I2 (weakest oxidizing agent)

Based on this reaction, we can conclude that Cl2 is the strongest oxidizing agent, followed by Br2, and then I2 is the weakest oxidizing agent.

For reducing agents, observe reactions 1 and 2:

Reaction 1:
Cu (strongest reducing agent)
I-
Ag
Br- (weakest reducing agent)

Reaction 2:
Zn(strongest reducing agent)
Pb
Cu
Ag(weakest reducing agent)

From reaction 1, we can conclude that Cu is the strongest reducing agent, followed by I-, then Ag, and finally, Br- is the weakest reducing agent. From reaction 2, we can conclude that Zn is the strongest reducing agent, followed by Pb, then Cu, and finally, Ag is the weakest reducing agent.

Now, combine the information from both reactions:

Relative strengths of oxidizing agents:
1. Cl2 (strongest oxidizing agent)
2. Br2
3. I2 (weakest oxidizing agent)

Relative strengths of reducing agents:
1. Cu (strongest reducing agent)
2. I-
3. Ag
4. Br- (weakest reducing agent)

By combining the information from both reactions, you can create a single table of relative strengths of oxidizing and reducing agents.