Redox Reaction Chemistry Example 2

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Example 2

medium
In the reaction Zn(s)+CuSO4(aq)→ZnSO4(aq)+Cu(s)\text{Zn(s)} + \text{CuSO}_4\text{(aq)} \rightarrow \text{ZnSO}_4\text{(aq)} + \text{Cu(s)}, identify the oxidizing agent and the reducing agent.

Solution

  1. 1
    Assign oxidation numbers: Zn goes from 00 to +2+2 (oxidized — lost electrons). Cu goes from +2+2 to 00 (reduced — gained electrons).
  2. 2
    The oxidizing agent is the species that gets reduced (and causes oxidation in the other): Cu2+\text{Cu}^{2+} is the oxidizing agent.
  3. 3
    The reducing agent is the species that gets oxidized (and causes reduction in the other): Zn is the reducing agent.

Answer

Oxidizing agent: Cu2+. Reducing agent: Zn.\text{Oxidizing agent: Cu}^{2+}\text{. Reducing agent: Zn.}
A common source of confusion: the oxidizing agent itself gets reduced, and the reducing agent itself gets oxidized. Think of it as: the reducing agent 'gives' electrons, the oxidizing agent 'takes' them.

About Redox Reaction

A chemical reaction in which electrons are transferred from one substance (the reducing agent, which is oxidized) to another (the oxidizing agent, which is reduced).

Learn more about Redox Reaction →

More Redox Reaction Examples

Example 1 easy

Define a redox reaction and explain the relationship between oxidation and reduction.

Example 3 medium

Determine whether the following reaction is a redox reaction: [formula]. Justify your answer.

Example 4 hard

Balance the following redox reaction in acidic solution using the half-reaction method: [formula].

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