Consider the following electrochemical cell at 298 K A g ( s ) | A g I ( s ) | I - ( a q ) | | C l - ( a q ) | H g 2 C l 2 | H g ( l ) P t ( s ) [Given E C l - | H g 2 C l 2 | H g o = 0.26 V . E A g +

Question

Consider the following electrochemical cell at 298 K
$A g (s) | A g I (s) | I^{-} (a q) | | C l^{-} (a q) | H g_{2} C l_{2} | H g (l) P t (s)$
[Given $E_{C l^{-} | H g_{2} C l_{2} | H g}^{o} = 0.26 V . E_{A g^{+} / A g}^{o} = 0.8 V, K_{s p} (A g I) = 1 0^{- 16}$ and $\frac{2.303 R T}{F} = 0.06$ ]
The overall reaction occurring in the above cell is

TestHub · Accepted Answer

Anode A g + I - → A g I + e - Cathode H g 2 C l 2 + 2 e → 2 H g + 2 C l - Hence, The overall reaction occurring in the above cell is 1 2 H g 2 C l 2 ( s ) + A g ( s ) + I - ( a q ) → H g ( l ) + C l - ( a q ) + A g I ( s )

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