`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 solve the question regarding 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 analyze the oxidation states of the elements involved and determine the type of reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- Reactants: Iron (Fe) in solid state and water (H2O) in liquid state.
- Products: Iron(II,III) oxide (\( \text{Fe}_3\text{O}_4 \)) and hydrogen gas (\( \text{H}_2 \)).

2. **Assign Oxidation States:**
- For \( \text{Fe}(s) \): The oxidation state is 0 (elemental form).
- For \( \text{H}_2\text{O}(l) \):
- Hydrogen (H) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- For \( \text{Fe}_3\text{O}_4 \):
- Let the oxidation state of Fe be \( x \).
- The equation for oxidation states is:
\[ 3x + 4(-2) = 0 \implies 3x - 8 = 0 \implies 3x = 8 \implies x = \frac{8}{3} \]
- Thus, the oxidation state of Fe in \( \text{Fe}_3\text{O}_4 \) is \( \frac{8}{3} \).

3. **Determine Changes in Oxidation States:**
- Iron (Fe) changes from 0 to \( \frac{8}{3} \) (oxidation).
- Hydrogen (H) changes from +1 in water to 0 in hydrogen gas (reduction).

4. **Classify the Reaction:**
- Since oxidation (loss of electrons) and reduction (gain of electrons) occur simultaneously, this reaction is classified as a **redox reaction**.
- Specifically, it is an **intermolecular redox reaction** because it involves two different reactants (Fe and H2O).

5. **Eliminate Other Options:**
- It is not a **disproportionation reaction** because no single species is being oxidized and reduced simultaneously.
- It is not a **comproportionation reaction** as there is no single species present in two different oxidation states in the reactants.
- It is not a **combination or decomposition reaction** as it does not fit those definitions.

### Conclusion:
The reaction \( \text{Fe}(s) + \text{H}_2\text{O}(l) \overset{\text{Boil}}{\rightarrow} \text{Fe}_3\text{O}_4 + \text{H}_2 \) is classified as an **intermolecular redox reaction**.

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