Calculate the electrode potential for
`underset(1 atm)((Pt)H_2) | H^(+) (c = 0.1)`

Explanation

To calculate the electrode potential for the half-cell reaction given as \( \text{Pt} | \text{H}_2 (1 \text{ atm}) | \text{H}^+ (c = 0.1) \), we will use the Nernst equation. Here are the steps to solve the problem:

### Step 1: Write the half-cell reaction
The half-cell reaction for the reduction of hydrogen ions is:
\[ \text{2H}^+ + 2e^- \rightarrow \text{H}_2 \]

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