`Mg(s)+H_(2)O(l) overset("warm")toMg(OH)_(2)+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

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- The reactants are magnesium (Mg) and water (H₂O).
- The products formed are magnesium hydroxide (Mg(OH)₂) and hydrogen gas (H₂).

2. **Write the Balanced Chemical Equation**:
- The reaction can be represented as:
\[ \text{Mg(s)} + \text{H}_2\text{O(l)} \xrightarrow{\text{warm}} \text{Mg(OH)}_2\text{(aq)} + \text{H}_2\text{(g)} \]

3. **Determine the Type of Reaction**:
- This reaction is a **displacement reaction** because magnesium displaces hydrogen from water. Magnesium is more reactive than hydrogen, allowing it to take the place of hydrogen in the reaction.

4. **Analyze Oxidation States**:
- In elemental magnesium (Mg), the oxidation state is 0.
- In magnesium hydroxide (Mg(OH)₂), magnesium has an oxidation state of +2.
- In water (H₂O), hydrogen has an oxidation state of +1, and in hydrogen gas (H₂), the oxidation state is 0.
- Therefore, magnesium is oxidized (0 to +2), and hydrogen is reduced (+1 to 0).

5. **Identify the Redox Nature of the Reaction**:
- Since one species (Mg) is oxidized and another species (H) is reduced, this reaction is classified as an **intermolecular redox reaction**.

6. **Conclusion**:
- The correct classification of this reaction is an **intermolecular redox reaction** or a **displacement reaction**.