Following reactions can occur at cathode during the electrolysis of aqueous silver nitrate solution using Pt electrodes :
`Ag^(+)""_((aq)) ""^(+e^(-))to Ag""_((s)),E^(@)=0.80V`
`H^(+)""_((aq)) ""^(+e^(-))to 1/2H_(2(g)),E^(@)=0.00V`
On the basis of theri standars electrode protential values, which reaction is feasible at cathode and why ?

Explanation

To determine which reaction is feasible at the cathode during the electrolysis of aqueous silver nitrate solution using platinum electrodes, we need to analyze the standard electrode potentials (E°) of the given reactions.

### Step-by-Step Solution:

1. **Identify the Reactions and Their Standard Electrode Potentials**:
- Reaction 1: \( \text{Ag}^+ (aq) + e^- \rightarrow \text{Ag} (s) \) with \( E^\circ = +0.80 \, \text{V} \)
- Reaction 2: \( \text{H}^+ (aq) + e^- \rightarrow \frac{1}{2} \text{H}_2 (g) \) with \( E^\circ = 0.00 \, \text{V} \)

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