Identify the disproportionation reaction.

Options

A. `CH_(4)+2O_(2)toCO_(2)+2H_(2)O`
B. `CH_(4)+4Cl_(2)toC Cl_(4)+4HCl`
C. `2F_(2)+2OH^(-)to2F^(-)+OF_(2)+H_(2)O`
D. `2NO_(2)+2OH^(-)toNO_(2)^(-)+NO_(3)^(-)+H_(2)O`

Explanation

To identify the disproportionation reaction among the given options, we need to understand what a disproportionation reaction is. A disproportionation reaction is a type of redox reaction where the same substance is both oxidized and reduced, resulting in two different products.

### Step-by-Step Solution:

1. **Understand Oxidation and Reduction**:
- **Oxidation**: Loss of electrons (increase in oxidation state).
- **Reduction**: Gain of electrons (decrease in oxidation state).

2. **Identify the Reactions**:
- We have four reactions to analyze. We will determine the oxidation states of the relevant elements in each reaction.

3. **Analyze Each Reaction**:
- **Reaction 1**: Methane to Carbon Dioxide and Water
- Carbon in methane (C) has an oxidation state of -4.
- In carbon dioxide (CO2), carbon has an oxidation state of +4.
- Oxygen in CO2 is -2, and in water (H2O) it is -2.
- Here, carbon is oxidized (from -4 to +4) and oxygen is reduced (from 0 to -2).
- **Conclusion**: This is not a disproportionation reaction.

- **Reaction 2**: Methane to Carbon Tetrachloride and Hydrochloric Acid
- Carbon in methane (C) has an oxidation state of -4.
- In carbon tetrachloride (CCl4), carbon has an oxidation state of +4.
- Chlorine in Cl2 is 0, and in HCl it is -1.
- Carbon is oxidized, and chlorine is reduced.
- **Conclusion**: This is not a disproportionation reaction.

- **Reaction 3**: Fluorine and Hydroxide Ion to Water
- Fluorine (F2) has an oxidation state of 0.
- In hydroxide (OH-), oxygen is -2 and hydrogen is +1.
- In water (H2O), oxygen is -2 and hydrogen is +1.
- Fluorine is reduced (from 0 to -1), and oxygen is oxidized (from -2 to +2).
- **Conclusion**: This is not a disproportionation reaction.

- **Reaction 4**: Nitrogen Compounds
- Nitrogen in the reaction has different oxidation states:
- In one compound, it is +4, in another it is +3, and in another it is +5.
- The same nitrogen species is being oxidized (from +4 to +5) and reduced (from +4 to +3).
- **Conclusion**: This is a disproportionation reaction.

4. **Final Answer**:
- The disproportionation reaction is **Reaction 4**, where nitrogen is both oxidized and reduced.