In the electrolysis of aqueous sodium chloride solution which of the hall cell reaction will occur at anode?

Options

A. `Na^(+)(aq)+e^(-)rarrNa(s):E_("cell")^(@)=-2.71V`
B. `2H_(2)O(l)rarrO_(2)(g)+4H^(+)(aq) +4e^(-) E_("cell")^(@)-123V`
C. `H^(+)(aq)+e^(-)rarr(1)/(2)H_(2)(g):E_("cell")^(@)=0.00V`
D. `Cl^(-)(aq)rarr(1)/(2)Cl_(2)(g)+e^(-),E_("cell")^(@)=1.36V`

Explanation

To determine which half-cell reaction occurs at the anode during the electrolysis of an aqueous sodium chloride solution, we need to analyze the possible reactions and their standard electrode potentials.

### Step-by-Step Solution:

1. **Identify the Electrolysis Process**:
In the electrolysis of aqueous sodium chloride (NaCl), two main reactions can occur at the anode: the oxidation of chloride ions (Cl⁻) and the oxidation of water (H₂O).

2. **Write the Half-Reactions**:
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