Calculate the electrode potential of given electrode
`Pt, Cl_(2)` (1.5 bar) `2Cl^(-) (0.01M), E_(Cl_(2)//2Cl^(-))^(@) = 1.36V`

Explanation

To calculate the electrode potential of the given electrode system \( \text{Pt, Cl}_2 (1.5 \, \text{bar}) | 2\text{Cl}^- (0.01 \, \text{M}) \) with the standard reduction potential \( E^\circ_{\text{Cl}_2/2\text{Cl}^-} = 1.36 \, \text{V} \), we will use the Nernst equation.

### Step-by-Step Solution:

1. **Identify the Reaction**:
The half-reaction for the reduction of chlorine gas to chloride ions is:
\[
\text{Cl}_2 + 2e^- \rightarrow 2\text{Cl}^-
...