The reaction `2FeCl_2 + SnCl_2 to 2FeCl_2 + SnCl_4` is an example of

Options

A. First order reaction
B. Second order reaction
C. Third order reaction
D. None of these

Answer

To determine the type of reaction represented by the equation \( 2FeCl_2 + SnCl_2 \rightarrow 2FeCl_3 + SnCl_4 \), we will analyze the reaction step by step.

### Step 1: Identify the Reactants and Products
The reactants in the reaction are:
- \( 2FeCl_2 \) (Iron(II) chloride)
- \( SnCl_2 \) (Tin(II) chloride)

The products of the reaction are:
- \( 2FeCl_3 \) (Iron(III) chloride)
- \( SnCl_4 \) (Tin(IV) chloride)

### Step 2: Analyze the Change in Oxidation States
Next, we need to analyze the oxidation states of the elements involved in the reaction:
- In \( FeCl_2 \), iron (Fe) has an oxidation state of +2.
- In \( FeCl_3 \), iron (Fe) has an oxidation state of +3.
- In \( SnCl_2 \), tin (Sn) has an oxidation state of +2.
- In \( SnCl_4 \), tin (Sn) has an oxidation state of +4.

From this, we can see that:
- Iron (Fe) is oxidized from +2 to +3.
- Tin (Sn) is reduced from +2 to +4.

### Step 3: Determine the Type of Reaction
Since one element (iron) is oxidized and another element (tin) is reduced, this reaction is classified as a **redox reaction** (oxidation-reduction reaction).

### Step 4: Conclusion
Thus, the reaction \( 2FeCl_2 + SnCl_2 \rightarrow 2FeCl_3 + SnCl_4 \) is an example of a **redox reaction**.

### Final Answer
The reaction is an example of a **redox reaction**.

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