Go To Your Study Dashboard

Get Answers to all your Questions

header-bg

In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?

$(i) Na^{+}(aq) + e^{-} \rightarrow Na (s); E^{o}_{Cell} = -2.71V$

$(ii) 2H_{2}O (l) \rightarrow O_{2}(g) + 4H^+(aq) + 4e^{-} ; E^{o}_{Cell} = 1.23V$

$(iii) H^{+}(aq) + e^{-}\rightarrow \frac{1}{2}H_{2} (g); E^{o}_{Cell} = 0.00V$

$(iv) Cl^{-}(aq) \rightarrow \frac{1}{2} Cl_{2}(g) + e^{-} ; E^{o}_{Cell} = 1.36V$

Answers (1)

The answer is the option (ii) Upon electrolysis H₂O gives-

$2H_2 O\rightarrow O_2+4H^++4e^-;E_{cell}^{0}=1.23V$

Since, $E_{cell}^{0}=1.23V$ . Hence this half cell reaction occurs at anode.

Posted by

infoexpert23

View full answer

Similar Questions

Latest Question