Write the reaction equations in molecular and ionic forms with which you can carry out the transformations according to the scheme

Write the reaction equations in molecular and ionic forms with which you can carry out the transformations according to the scheme:
Fe -> Fe (SO4) 3 —> FeCI3 —> Fe (NO3) 3 —> Fe2O3.
For redox reactions, indicate oxidizing agent and reducing agent.

Decision:
chemical reaction equations:
1). 2Fe + 6H2SO4 = Fe2 (SO4) 3 + 3SO2 ↑ + 6H2O – In this reaction, iron is oxidized to oxidation state +3, i.e. iron is a reducing agent. In this reaction, sulfur (VI) is reduced to sulfur (IV). those. sulfur is an oxidizing agent.
The full ionic form of the reaction equation:
2Fe0 + 12H0 + SO42- = 2Fe3 + + 3SO42- + 3SO2 ↑ + 6H2O.
2). Fe2 (SO4) 3 + 3ВаCl2 -> 2FeCl3 + 3ВаSO4 ↓ – exchange reaction; 
The full ionic form of the reaction equation:
2Fe3 + + 3SO42- + 3Ва2 + + 6Cl- = 2Fe3 + + 6Cl- + 3ВаSO4 ↓;
The abbreviated ionic reaction equation:
3Ва2 + + 3SO42- = 3ВаSO4 ↓.
3). FeCl3 + 3HNO3 -> Fe (NO3) 3 + 3HCl – exchange reaction;
The full ionic form of the reaction equation:
Fe3 + + 3Cl- + 3Ag + + 3NO3- = Fe3 + + 3NO3- + 3AgCl ↓.
The abbreviated ionic reaction equation:
3Ag + + 3Cl- = 3AgCl ↓.
4). 4Fe (NO3) 3 —> Fe2O3 + NO2 ↑ + O2 ↑ – decomposition of iron (III) nitrate upon heating. In this case, oxidation-reduction occurs. – In this reaction, oxygen is oxidized to oxidation state 0, i.e. oxygen is a reducing agent. In this reaction, nitrogen (V) is reduced to nitrogen (IV). those. nitrogen is an oxidizing agent

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