Question

Given the standard reduction potentials (\( E^\Theta \)) for the half-cell reactions below, the standard Gibbs free energy of the dissolution of silver chloride in water, at 298 K, is __________ J mol\(^{-1}\) (rounded off to nearest integer).
(Given: Faraday constant, \( F = 96500 \, \text{C mol}^{-1} \); \( J = \text{C} \times \text{V} \))
\[\text{AgCl}(s) + e^{-} \rightarrow \text{Ag}(s) + \text{Cl}^{-}(\text{aq}); \quad E^\Theta = 0.22 \, \text{V at 298 K}\]
\[\text{Ag}^{+}(\text{aq}) + e^{-} \rightarrow \text{Ag}(s); \quad E^\Theta = 0.80 \, \text{V at 298 K}\]

Answer 1

Correct Answer: 55960

The correct Answer is: 55960 or 55980 Approx .