During the electrolysis of dilute sulphuric acid, the following process is possible at anode.

Options

A. `2H_2O_((l)) to O_(2(g)) + 4H_((aq))^(+) + 4e^(-)`
B. `2SO_(4(aq))^(2-) to S_2O_(8(aq)) + 2e^(-)`
C. `H_2O_((l)) to H_((aq))^+ + OH_((aq))^-`
D. `H_2O_((l)) + e^(-) to 1/2H_(2(g)) + OH_((aq))^-`

Answer

To solve the question regarding the electrolysis of dilute sulfuric acid and the processes that occur at the anode, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Electrolysis**:
- Electrolysis is a process that uses electrical energy to drive a non-spontaneous chemical reaction. In the case of dilute sulfuric acid (H2SO4), we are interested in the reactions occurring at both the anode and cathode.

2. **Identifying the Anode Reaction**:
- At the anode, oxidation occurs. The anode is the positive electrode where electrons are released. In dilute sulfuric acid, the possible species that can be oxidized are hydroxide ions (OH⁻) and water (H2O).

3. **Considering the Stability of Sulfate Ions**:
- The sulfate ions (SO4²⁻) are quite stable and do not readily participate in oxidation reactions under these conditions. Therefore, they do not contribute to the reaction at the anode.

4. **Oxidation of Water or Hydroxide Ions**:
- Since hydroxide ions are attracted to the anode, they can be oxidized. The oxidation of hydroxide ions leads to the formation of oxygen gas (O2) and protons (H⁺).

5. **Writing the Anode Reaction**:
- The balanced reaction for the oxidation of hydroxide ions at the anode can be written as:
\[ 4OH⁻ \rightarrow 2H2O + O2 + 4e⁻ \]
- Alternatively, water can also be oxidized:
\[ 2H2O \rightarrow O2 + 4H⁺ + 4e⁻ \]

6. **Conclusion**:
- Both reactions indicate that oxygen gas is produced at the anode during the electrolysis of dilute sulfuric acid. The correct reaction at the anode can be summarized as the oxidation of hydroxide ions or water to produce oxygen gas.

### Final Answer:
The correct process at the anode during the electrolysis of dilute sulfuric acid is:
\[ 4OH⁻ \rightarrow 2H2O + O2 + 4e⁻ \]
or
\[ 2H2O \rightarrow O2 + 4H⁺ + 4e⁻ \]