Following reactions occur at cathode during electrolysis of aqueous silver chloride solution Ag+(aq) + e` Ag(s) Eo=+0.80V H+(aq) + e` H2(g) Eo= 0.00V On the basis of their standard reduction electrode potential values, which reaction is feasible at cathode and why?

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A g^{+} (a q) + e \to A g (s) E^{\circ} = + .80 V

H^{+} (a q) + e^{-} \to \frac{1}{2} H_{2} (g) E^{o} = 0.00 V

(E^{o})

{N a}^{+} (a q) + e^{-} ⟶ N a (s) E^{0} = - 2.71 V

H^{+} (a q) + e^{-} ⟶ \frac{1}{2} H_{2} (g) E^{0} = 0.00 V

(E^{0})

N a^{+} (a q) + e^{-} \to N a (s) E^{0} = - 2.71 V

H^{+} (a q) + e^{-} \to \frac{1}{2} H_{2} (g) E^{0} = 0.00 V

(E^{0})

(a) Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution:

$N a^{+} (a q) + e^{-} \to N a (s) E^{\circ} = - 2.71 V$
$H^{+} (a q) + e^{-} \to \frac{1}{2} H_{2} (g) E^{\circ} = 0.00 V$

On the basis of their standard reduction electrode potential $(E^{\circ})$ values, which reaction is feasible at the cathode and why?

(b) Why does the cell potential of mercury cell remain constant throughout its life?

N a^{+} (a q) + e^{-} \to N a (s) E^{0} = - 2.71 V

H^{+} (a q) + e^{-} \to \frac{1}{2} H_{2} (g) E^{0} = 0.00 V

(E^{0})

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