(a) Following reactions occur at cathode during the electrolysis of aq

1.	(a) Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution: Na+(aq)+e−→Na(s) E∘=−2.71V H+(aq)+e−→12H2(g)E∘=0.00V On the basis of their standard reduction electrode potential (E∘) values, which reaction is feasible at the cathode and why? (b) Why does the cell potential of mercury cell remain constant throughout its life?
Answer» (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?

(a) Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution: Na+(aq)+e−→Na(s) E∘=−2.71V H+(aq)+e−→12H2(g)E∘=0.00V On the basis of their standard reduction electrode potential (E∘) values, which reaction is feasible at the cathode and why? (b) Why does the cell potential of mercury cell remain constant throughout its life?

Answer»

(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?