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  • Following reactions can occur at cathode during the electrolysis of aqueous silver nitrate solution using Pt electrodes : <img alt="\begin{aligned} &\mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}_{(\mathrm{s})}

Following reactions can occur at cathode during the electrolysis of aqueous silver nitrate solution using Pt electrodes :

\begin{aligned} &\mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}_{(\mathrm{s})} ; \mathrm{E}^{\circ}=0.80 \mathrm{V}\\ &\mathrm{H}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \longrightarrow \frac{1}{2} \mathrm{H}_{2(\mathrm{g})} ; \mathrm{E}^{\circ}=0.00 \mathrm{V} \end{aligned}

On the basis of their standard electrode potential values, which reaction is feasible at cathode and why?

 

 

 

 
 
 
 
 

Answers (1)

\begin{aligned} &(I) \ \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}_{(\mathrm{s})} ; \mathrm{E}^{\circ}=0.80 \mathrm{V}\\ &(II) \ \mathrm{H}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \longrightarrow \frac{1}{2} \mathrm{H}_{2(\mathrm{g})} ; \mathrm{E}^{\circ}=0.00 \mathrm{V} \end{aligned}

I reaction is feasible at cathode because higher the Eo value, more is the capacity to get reduced.

Posted by

Sumit Saini

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