In the reaction Cl2 + 2Fe2+ - 2Cl^- + 2Fe3+, which species is the oxidizing agent?

Question

In the reaction Cl2 + 2Fe2+ -> 2Cl^- + 2Fe3+, which species is the oxidizing agent?

ScanSolve AI Tutor · Accepted Answer

To identify the oxidizing agent, we need to determine the change in oxidation states for each species in the reaction. An oxidizing agent is the species that gets reduced (gains electrons) and causes another species to be oxidized.

The given reaction is:

Cl_2 + 2Fe^{2+} \rightarrow 2Cl^{-} + 2Fe^{3+}

Determine the oxidation states of each species.
- For $Cl_2$ : Chlorine is in its elemental form, so its oxidation state is 0.
- For $Fe^{2+}$ : The oxidation state of iron is +2.
- For $Cl^{-}$ : The oxidation state of chlorine is -1.
- For $Fe^{3+}$ : The oxidation state of iron is +3.
Identify which species is oxidized and which is reduced.
- Chlorine: The oxidation state of chlorine changes from 0 in $Cl_2$ to -1 in $Cl^{-}$ . This is a decrease in oxidation state, meaning $Cl_2$ has gained electrons and undergone reduction.
- Iron: The oxidation state of iron changes from +2 in $Fe^{2+}$ to +3 in $Fe^{3+}$ . This is an increase in oxidation state, meaning $Fe^{2+}$ has lost electrons and undergone oxidation.
Identify the oxidizing agent.
Since $Cl_2$ is reduced, it acts as the oxidizing agent (it causes the oxidation of $Fe^{2+}$ ).

Comparing this with the given options:
A. $Fe^{2+}$ (reducing agent)
B. $Cl_2$ (oxidizing agent)
C. $Fe^{3+}$ (product of oxidation)
D. $Cl^{-}$ (product of reduction)

The correct option is B.

The species that acts as the oxidizing agent is $\boxed{\text{B. } Cl_2}$ .

In the reaction Cl2 + 2Fe2+ -> 2Cl^- + 2Fe3+, which species is the oxidizing agent?

Answer

Step-by-step solution

Determine the oxidation states of each species.

Identify which species is oxidized and which is reduced.

Identify the oxidizing agent.

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