`Fe(s)+H_(2)O(l) overset(Boil) to Fe_(3)O_(4)+H_(2)uarr`

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 \( \text{Fe}(s) + \text{H}_2\text{O}(l) \overset{\text{Boil}}{\rightarrow} \text{Fe}_3\text{O}_4 + \text{H}_2 \), we will follow these steps:

### Step 1: Identify the oxidation states of the reactants
- **Iron (Fe)** is in its elemental state, so its oxidation state is 0.
- **Water (H2O)** has hydrogen in the +1 oxidation state and oxygen in the -2 oxidation state.

### Step 2: Identify the oxidation states of the products
- In **Fe3O4**, let the oxidation state of iron be \( x \). The equation can be set up as follows:
\[ 3x + 4(-2) = 0 \]
Solving for \( x \):
\[ 3x - 8 = 0 \implies 3x = 8 \implies x = \frac{8}{3} \]
Thus, the oxidation state of iron in Fe3O4 is \( \frac{8}{3} \).
- **Hydrogen (H2)** in its elemental state has an oxidation state of 0.

### Step 3: Determine the changes in oxidation states
- **Iron (Fe)** goes from 0 to \( \frac{8}{3} \) (oxidation).
- **Hydrogen (H)** goes from +1 to 0 (reduction).

### Step 4: Classify the reaction
- Since iron is oxidized and hydrogen is reduced, this reaction is classified as a **redox reaction**.
- It involves two different substances changing their oxidation states, which makes it an **intermolecular redox reaction**.

### Step 5: Eliminate other reaction types
- It is not a **disproportionation reaction** because there is no single species that is both oxidized and reduced.
- It is not a **comproportionation reaction** because there are not two different oxidation states of the same species in the reactants.
- It is not a **combination reaction** because two reactants are forming two products.

### Conclusion
The correct classification of the reaction is an **intermolecular redox reaction**.

### Final Answer
The correct answer is option 3: Intermolecular redox reaction.

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