In the given chemical reaction:
[tex]\[ \ce{Fe + Cu(NO3)2 -> Cu + Fe(NO3)2} \][/tex]
we need to determine the reducing agent.
To identify the reducing agent, let’s follow these steps:
1. Assign Oxidation States:
- Iron (Fe) in the reactants is in its elemental form, so its oxidation state is 0.
- Copper (Cu) in [tex]\(\ce{Cu(NO3)2}\)[/tex] starts with a +2 oxidation state (since nitrate ([tex]\(\ce{NO3}^-\)[/tex]) has a -1 charge, and there are two nitrate ions).
- Copper (Cu) in the products is in its elemental form, so its oxidation state is 0.
- Iron (Fe) in [tex]\(\ce{Fe(NO3)2}\)[/tex] has a +2 oxidation state (similar reasoning as for copper, with each nitrate contributing -1 charge).
2. Determine the Changes in Oxidation States:
- Fe goes from an oxidation state of 0 to +2.
- Cu goes from +2 in [tex]\(\ce{Cu(NO3)2}\)[/tex] to 0 in the products.
3. Identify Oxidation and Reduction:
- Since Fe’s oxidation state increases from 0 to +2, Fe is being oxidized (loses electrons).
- Since Cu’s oxidation state decreases from +2 to 0, Cu is being reduced (gains electrons).
4. Find the Reducing Agent:
- The reducing agent is the substance that gets oxidized because it loses electrons and thus donates electrons to another species.
Since iron (Fe) is being oxidized (loses electrons), it is the substance that causes the reduction of Cu and thus acts as the reducing agent.
Therefore, the reducing agent in this reaction is:
[tex]\[ \boxed{\text{Fe}} \][/tex]
