The cell in which the following reaction occurs
`2Fe^(3+)(aq)+2I^(-)(aq) to 2Fe^(2+)(aq)+2I_(2) " has "E_(cell)^(@)=0.236 V " at "298 K`.
Calculate standard Gibbs energy and equilibrium constant for the reaction.

Explanation

To solve the problem, we need to calculate the standard Gibbs energy change (ΔG°) and the equilibrium constant (K) for the given electrochemical reaction:

**Reaction:**
\[ 2Fe^{3+}(aq) + 2I^{-}(aq) \rightarrow 2Fe^{2+}(aq) + I_{2}(s) \]

**Given:**
- Standard cell potential, \( E_{cell}^\circ = 0.236 \, V \)
- Temperature, \( T = 298 \, K \)
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