Mercury cell gives a constant potential.

True

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False

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Solution

The correct option is A True

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Similar questions

1.35 V

K O H

Z n O

1.35

Z n (H g) + H g O_{(s)} \to Z n O_{(s)} + H g_{(l)}

(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^{-} ⟶ 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})

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