To determine the oxidizing agent in the reaction
[tex]\[
Fe + Cu(NO_3)_2 \rightarrow Cu + Fe(NO_3)_2,
\][/tex]
let's follow these steps:
### Step 1: Identify the Initial Oxidation States
1. Iron (Fe): Initially, iron (Fe) is in its elemental form, so its oxidation state is 0.
2. Copper in Copper Nitrate (Cu(NO_3)_2): Copper forms ions Cu^2+ in Cu(NO_3)_2, so the oxidation state of copper here is +2.
### Step 2: Identify the Final Oxidation States
1. Copper (Cu): In the product, copper (Cu) is in its elemental form, so its oxidation state is 0.
2. Iron in Iron Nitrate (Fe(NO_3)_2): Iron forms ions Fe^2+ in Fe(NO_3)_2, so the oxidation state of iron here is +2.
### Step 3: Determine Changes in Oxidation States
1. Iron (Fe):
- Initial oxidation state: 0
- Final oxidation state: +2
- Change: 0 to +2 (oxidation, loss of electrons)
2. Copper (Cu):
- Initial oxidation state: +2
- Final oxidation state: 0
- Change: +2 to 0 (reduction, gain of electrons)
### Step 4: Identify the Substance that is Reduced
The substance that is reduced undergoes a decrease in oxidation state. Here, the copper ion (Cu^2+) is reduced from +2 to 0.
### Step 5: Identify the Oxidizing Agent
An oxidizing agent is a substance that causes oxidation by accepting electrons and, in the process, it itself is reduced. Since Cu^2+ is reduced, it is the oxidizing agent.
### Final Answer
Therefore, the oxidizing agent in the reaction is:
[tex]\[
\text{Cu}^{2+} \text{ (supplied by Cu(NO}_3\text{)}_2)
\][/tex]
