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

The correct Answer is: 55960 or 55980 Approx .