Calculate the equilibrium constant for the following reaction at `25^@C` .
`Ag^(+)(aq) + Fe^(2+)(aq) to Ag(s) + Fe^(3+)(aq)`
The standard emf of the corresponding voltaic cell is 0.03 V.

Explanation

To calculate the equilibrium constant (K) for the reaction:

\[ \text{Ag}^+(aq) + \text{Fe}^{2+}(aq) \rightleftharpoons \text{Ag}(s) + \text{Fe}^{3+}(aq) \]

at \( 25^\circ C \) given that the standard emf (\( E^\circ \)) of the corresponding voltaic cell is \( 0.03 \, V \), we can follow these steps:

### Step 1: Identify the number of electrons transferred (N)
In the given reaction, silver ion (\( \text{Ag}^+ \)) is reduced to solid silver (\( \text{Ag} \)), and iron ion (\( \text{Fe}^{2+} \)) is oxidized to iron ion (\( \text{Fe}^{3+} \)). The transfer of electrons can be represented as follows:
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