Determine the values of equilibrium constant `(K_(c))` and `DeltaG^(@)` for the reaction
`Ni(s)+2Ag^(+)(aq)rarrNi^(2+)(aq)+2Ag(s), E^(@)=1.05 V.` (`"Given " 1F=96500"C mol"^(-1))`

Explanation

To determine the values of the equilibrium constant \( K_c \) and the standard Gibbs free energy change \( \Delta G^\circ \) for the given reaction:

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

with a standard cell potential \( E^\circ = 1.05 \, \text{V} \), we can follow these steps:

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