`C(s)+O_(2)(g) overset(Delta)toCO_(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 of carbon with oxygen to form carbon dioxide, we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- The reactants are solid carbon (C) and gaseous oxygen (O₂).
- The product formed is carbon dioxide (CO₂).

2. **Write the Balanced Chemical Equation**:
- The unbalanced equation is:
\[ C(s) + O_2(g) \rightarrow CO_2(g) \]
- This equation is already balanced as one carbon atom reacts with one molecule of oxygen to produce one molecule of carbon dioxide.

3. **Determine the Type of Reaction**:
- This reaction involves the combination of carbon and oxygen to form a single product (CO₂).
- It is an oxidation-reduction (redox) reaction because:
- Carbon is oxidized from an oxidation state of 0 in C to +4 in CO₂.
- Oxygen is reduced from an oxidation state of 0 in O₂ to -2 in CO₂.

4. **Classify the Reaction**:
- Since the reaction involves the combination of elements to form a compound and involves oxidation and reduction, it is classified as a **thermal combination redox reaction**.
- It is not a disproportionation reaction, comproportionation reaction, or a displacement reaction since those definitions do not apply here.

5. **Conclusion**:
- The correct classification for the reaction \( C(s) + O_2(g) \rightarrow CO_2(g) \) is a **thermal combination redox reaction**.

### Final Answer:
The reaction \( C(s) + O_2(g) \rightarrow CO_2(g) \) is classified as a **thermal combination redox reaction**.

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