`CuO+H_(2) to Cu darr+H_(2)O`

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 \( \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} \), we will follow these steps:

### Step 1: Assign Oxidation States
- **CuO**: Copper (Cu) has an oxidation state of +2, and oxygen (O) has an oxidation state of -2.
- **H2**: Hydrogen (H) in its diatomic form has an oxidation state of 0.
- **Cu**: In its elemental form, copper has an oxidation state of 0.
- **H2O**: In water, hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2.

### Step 2: Identify Changes in Oxidation States
- **Copper (Cu)** changes from +2 in CuO to 0 in Cu. This indicates a reduction (gain of electrons).
- **Hydrogen (H)** changes from 0 in H2 to +1 in H2O. This indicates an oxidation (loss of electrons).

### Step 3: Determine the Type of Reaction
- Since Cu is reduced (gaining electrons) and H is oxidized (losing electrons), this reaction is a redox reaction.
- It involves two different molecules reacting with each other, which classifies it as an intermolecular redox reaction.

### Step 4: Evaluate the Options
- **Option A**: Disproportionation reaction - Not applicable, as no single element undergoes both oxidation and reduction.
- **Option B**: Comproportionation reaction - Not applicable, as there are no two same elements with different oxidation states.
- **Option C**: Intermolecular redox reaction - Correct, as it involves two different molecules reacting.
- **Option D**: Thermal decomposition - Not applicable, as there is no heat involved in this reaction.

### Conclusion
The correct answer is **Option C: Intermolecular redox reaction**.

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