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In the reaction: 2FeC1(2) + C1 to 2FeC1(...

In the reaction: `2FeC1_(2) + C1 to 2FeC1_(3)` Chlorine may be regarded as

A

an oxidising agent

B

a reducing agent

C

a catalyst

D

providing an inert medium

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The correct Answer is:
To determine the role of chlorine in the reaction \(2FeCl_2 + Cl_2 \rightarrow 2FeCl_3\), we can analyze the changes in oxidation states of the elements involved. ### Step-by-Step Solution: 1. **Identify the Reactants and Products:** - The reactants are \(FeCl_2\) (iron(II) chloride) and \(Cl_2\) (chlorine gas). - The product is \(FeCl_3\) (iron(III) chloride). 2. **Determine the Oxidation States:** - In \(FeCl_2\), the oxidation state of iron (Fe) is +2 (since each Cl has an oxidation state of -1, and there are two Cl atoms). - In \(FeCl_3\), the oxidation state of iron (Fe) is +3 (since there are three Cl atoms with an oxidation state of -1 each). - For chlorine gas (\(Cl_2\)), the oxidation state is 0 (as it is in its elemental form). - In \(FeCl_3\), the oxidation state of chlorine is -1. 3. **Identify Oxidation and Reduction:** - **Oxidation**: The oxidation state of iron increases from +2 in \(FeCl_2\) to +3 in \(FeCl_3\). This means iron is being oxidized. - **Reduction**: The oxidation state of chlorine decreases from 0 in \(Cl_2\) to -1 in \(FeCl_3\). This means chlorine is being reduced. 4. **Define the Role of Chlorine:** - Since chlorine is being reduced (its oxidation state decreases), it acts as an oxidizing agent because it facilitates the oxidation of iron by accepting electrons. 5. **Conclusion:** - In this reaction, chlorine is regarded as an **oxidizing agent** because it causes the oxidation of iron while itself being reduced.
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