Help Redox Reactions

For each of the following reactions:

1) Write a balanced net ionic equation for the reaction.
2) Identify which reactant is oxidized and which one is reduced.
3) Identify which reactant is the oxidizing agent and which one is the reducing agent.
4) Write balanced half reactions for the oxidation and reduction.

Zn(s) + FeCl2(aq)  Fe(s) + ZnCL2(aq)

Zn(s) + Pb(NO3)2(aq)  Pb(s) + Zn(NO3)2(aq)

3Ag(s) + Au(NO3)3(aq)  Au(s) + 3AgNO3(s)

3Mg(s) + Al2(SO4)3(aq)  2AL(s) + 3MgSO4(aq)

If someone could please help me with this it would REALLY help and i would REALLY appreciate it!! (10 points for best answer!)

Thank you!!!

(I'll use {n} to mean an oxidation state of n, since I can't get all the superscripts I need.)

1. Zn(s) + FeCl₂(aq) → Fe(s) + ZnCL₂(aq)

Zn{0} + Fe{2+} + 2Clˉ → Fe{0} + Zn{2+} + 2Clˉ
Zinc is oxidized, iron is reduced.
Iron is the oxidizer, zinc is the reducer.
Zn → Zn{2+} + 2eˉ
Fe{2+} + 2eˉ → Fe{0}


2. Zn(s) + Pb(NO₃)₂(aq) → Pb(s) + Zn(NO₃)₂(aq)

Zn{0} + Pb{2+} + 2(NO₃)ˉ → Pb{0} + Zn{2+} + 2(NO₃)ˉ
Zinc is oxidized, lead is reduced.
Lead is the oxidizer, zinc is the reducer.
Zn → Zn{2+} + 2eˉ
Pb{2+} + 2eˉ → Pb{0}


3. 3Ag(s) + Au(NO₃)₃(aq) → Au(s) + 3AgNO₃(s)

Ag{0} + Au{3+} + 3(NO₃)ˉ → Au{0} + Ag{3+} + 3(NO₃)ˉ
Silver is oxidized, gold is reduced.
Gold is the oxidizer, silver is the reducer.
3Ag → 3Ag{+} + 3eˉ
Au{3+} + 3eˉ → Au{0}


4. 3Mg(s) + Al₂(SO₄)₃(aq) → 2AL(s) + 3MgSO₄(aq)

3Mg{0} + 2Al{3+} + 3(SO₄)²ˉ → 2Al{0} + 3Mg{2+} + 3(SO₄)²ˉ
Magnesium is oxidized, aluminum is reduced.
Aluminum is the oxidizer, magnesium is the reducer.
3Mg → 3Mg{2+} + 6eˉ
2Al{3+} + 6eˉ → 2Al{0}