`NaH(s)+H_(2)O to NaOH+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 determine the type of reaction represented by the equation:

\[ \text{NaH(s)} + \text{H}_2\text{O} \rightarrow \text{NaOH} + \text{H}_2 \]

we will analyze the oxidation states of the elements involved and identify the type of reaction based on the changes in these states.

### Step-by-Step Solution:

1. **Identify Reactants and Products:**
- Reactants: Sodium hydride (NaH) and water (H₂O).
- Products: Sodium hydroxide (NaOH) and hydrogen gas (H₂).

2. **Assign Oxidation States:**
- In NaH:
- Sodium (Na) is in the +1 oxidation state.
- Hydrogen (H) is in the -1 oxidation state.
- In H₂O:
- Each hydrogen (H) is in the +1 oxidation state.
- Oxygen (O) is in the -2 oxidation state.
- In NaOH:
- Sodium (Na) is in the +1 oxidation state.
- Oxygen (O) is in the -2 oxidation state.
- Hydrogen (H) is in the +1 oxidation state.
- In H₂:
- Each hydrogen (H) is in the 0 oxidation state.

3. **Analyze Changes in Oxidation States:**
- The hydrogen in NaH changes from -1 to 0 (oxidation).
- The hydrogen in H₂O changes from +1 to 0 (reduction).

4. **Determine Reaction Type:**
- **Redox Reaction:** Since there is both oxidation (H from -1 to 0) and reduction (H from +1 to 0), this is a redox reaction.
- **Comproportionation Reaction:** The same element (hydrogen) is present in two different oxidation states (-1 in NaH and +1 in H₂O) and is converted into two different products (H₂ and NaOH). This qualifies as a comproportionation reaction.

5. **Conclusion:**
- The reaction is both a redox reaction and a comproportionation reaction. Therefore, the correct answers are that it is a redox reaction and a comproportionation reaction.

### Final Answer:
The reaction is a **redox reaction** and a **comproportionation reaction**.