3Fe + 4H₂O ⎯→ Fe₃O₄ + 4H₂ identify reducing and oxidising agent
In the given reaction:
3Fe + 4H₂O → Fe₃O₄ + 4H₂
The reducing agent is Fe because it is being oxidized from Fe to Fe₃O₄.
The oxidizing agent is H₂O because it is being reduced from H₂O to H₂.
To identify the reducing agent and the oxidizing agent in the given chemical reaction:
1. Write down the balanced equation:
3Fe + 4H₂O → Fe₃O₄ + 4H₂
2. Identify the element or compound that loses electrons and undergoes oxidation. This is the reducing agent.
In this case, Fe (iron) loses electrons and is oxidized from an oxidation state of 0 to +3 in Fe₃O₄. Thus, Fe is the reducing agent.
3. Identify the element or compound that gains electrons and undergoes reduction. This is the oxidizing agent.
In this case, H₂O (water) gains electrons and is reduced from an oxidation state of 0 to -2 in H₂. Thus, H₂O is the oxidizing agent.
So, in the given reaction:
- Fe is the reducing agent
- H₂O is the oxidizing agent.