`2FeCl_(3)+SnCl_(2)to2FeCl_(2)+SnCl_(4)` is an example of

Options

A. non redox reaction
B. double displacement reaction
C. redox reaction
D. None of these

Explanation

To determine the type of reaction represented by the equation \(2FeCl_3 + SnCl_2 \rightarrow 2FeCl_2 + SnCl_4\), we will analyze the changes in oxidation states of the elements involved.

### Step 1: Identify the oxidation states of the reactants and products
- In \(FeCl_3\), iron (Fe) has an oxidation state of +3.
- In \(SnCl_2\), tin (Sn) has an oxidation state of +2.
- In \(FeCl_2\), iron (Fe) has an oxidation state of +2.
- In \(SnCl_4\), tin (Sn) has an oxidation state of +4.

### Step 2: Determine the changes in oxidation states
- Iron (Fe) changes from +3 in \(FeCl_3\) to +2 in \(FeCl_2\). This indicates a reduction (decrease in oxidation state).
- Tin (Sn) changes from +2 in \(SnCl_2\) to +4 in \(SnCl_4\). This indicates an oxidation (increase in oxidation state).

### Step 3: Conclude the type of reaction
Since we have identified that:
- Iron is being reduced (gaining electrons).
- Tin is being oxidized (losing electrons).

This simultaneous occurrence of oxidation and reduction indicates that the reaction is a **redox reaction**.

### Final Answer
The reaction \(2FeCl_3 + SnCl_2 \rightarrow 2FeCl_2 + SnCl_4\) is an example of a **redox reaction**.

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