`Fe(s)+2HCl to FeCl_(2)+H_(2)`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To analyze the reaction \( \text{Fe}(s) + 2\text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2 \) and determine its type, we can follow these steps:

### Step 1: Identify the Reactants and Products
- The reactants are iron (Fe) in solid form and hydrochloric acid (HCl).
- The products are iron(II) chloride (FeCl2) and hydrogen gas (H2).

### Step 2: Determine the Oxidation States
- In the reactants:
- The oxidation state of Fe (solid) is 0.
- In HCl, the oxidation state of H is +1 and Cl is -1.

- In the products:
- In FeCl2, the oxidation state of Fe is +2 and Cl is -1.
- In H2, the oxidation state of H is 0.

### Step 3: Analyze the Changes in Oxidation States
- For Fe:
- The oxidation state changes from 0 (in Fe) to +2 (in FeCl2). This indicates that Fe is being oxidized (losing electrons).

- For H:
- The oxidation state changes from +1 (in HCl) to 0 (in H2). This indicates that H is being reduced (gaining electrons).

### Step 4: Identify the Type of Reaction
- Since there is a simultaneous oxidation (Fe) and reduction (H) occurring in the reaction, it qualifies as a redox reaction.
- Specifically, this reaction involves the transfer of electrons between different species, which makes it an intermolecular redox reaction.

### Conclusion
The reaction \( \text{Fe}(s) + 2\text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2 \) is classified as an **intermolecular redox reaction**.

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