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In the reaction: 2 Fe + 3 CuCl₂ →2 FeCl3 + 3 Cu
Which element is oxidized?Which element is reduced?Which substance is the oxidizing agent?
Which substance is the reducing agent?

Sagot :

amysun2025

Answer:

Fe - oxidized, reducing agent

Cu - reduced, oxidizing agent

Explanation:

Pre-Solving

We are given the following reaction:

2Fe + 3CuCl₂ →2FeCl3 + 3Cu

We want to figure out which element is oxidized and which one is reduced. Furthermore, we want to figure out which substance would be the oxidizing agent, and which one would be the reducing agent.

Remember that if a substance is being oxidized, it is also the reducing agent. The same goes for the substance being reduced; it is also the oxidizing agent.

Recall that in order to figure out which element is oxidized or reduced, we need to look at the changes in their oxidation numbers. If an element's oxidation number increases, then it is oxidized, but if it decreases, it is reduced.

In order to help us, remember that any element by itself will always have an oxidation number of 0, and halogens usually have an oxidation number of -1. In a compound, the total sum of the oxidation numbers will equal the charge. Similarly, ions always have the same oxidation number as their charge.

Solving

Based on the rules, for the left side of the equation, we can determine that:

  • Fe has an oxidation number of 0
  • Cl has an oxidation number of -1
  • Cu has an oxidation number of +2
    This is because Cu + 2(-1) = 0, so Cu = +2.

For the right side of the equation, we can determine that:

  • Fe has an oxidation number of +3
  • Cl has an oxidation number -1
  • Cu has an oxidation number of 0

Notice how Fe's number increased. This means that Fe is oxidized. It is also the reducing agent.

Furthermore, notice how Cu's oxidation number went down. This means that Cu is reduced, and is therefore the oxidizing agent.

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