Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution:Ag+(aq)+e−→Ag(s) E∘=+0.80VH+(aq)+e−→12H2(g) E∘=0.00VOn the basis of their standard reduction electrode potential (Eo) values, which reaction is feasible at the cathode ?

Ag + ( aq ) + e − → Ag ( s ) E ∘ = + 0.80 V

Ag + ( aq ) + e − → Ag ( s ) E ∘ = + 0.80 V

H + ( aq ) + e − → 1 2 H 2 ( g ) E ∘ = 0.00 V

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Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution:
$\begin{array}{l} {Ag}^{+} (aq) + e^{-} \to Ag (s) E^{\circ} = + 0.80 V \\ H^{+} (aq) + e^{-} \to \frac{1}{2} H_{2} (g) E^{\circ} = 0.00 V \end{array}$
On the basis of their standard reduction electrode potential (E^o) values, which reaction is feasible at the cathode ?

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${Ag}^{+} (aq) + e^{-} \to Ag (s)$ $E^{\circ} = + 0.80 V$

$H^{+} (aq) + e^{-} \to \frac{1}{2} H_{2} (g) E^{\circ} = 0.00 V$

Both reactions are feasible

None of the above

answer is A.

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${Ag}^{+} (a q) + e^{-} \to Ag (s); E^{\circ} = + 0.80 V$

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

On the basis of their standard reduction potential (E^o) values, cathode reaction is given by the one with higher E^o values.

Thus, ${Ag}^{+} (a q) + e^{-} \to Ag (s)$ reaction will be more feasible at cathode.

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