Following reactions occur at cathode during electrolysis of aqueous silver chloride solution :
`Ag^(+)(aq)+e^(-) to Ag(s),E^(@)=+0.80" V"`
`H^(+)(aq)+e^(-) to 1//2 H_(2)(g), E^(@)=0.00" V"`
On the basis of standard reduction potential (`E^(@)` value), which reaction is feasible at cathode and why ?

Options

A. `Ag^(+)(aq)+e^(-) to Ag(s)" "E^(@)=+0.80V`
B. `H^(+)(aq)+e^(-) to (1)/(2)H_(2)(g)" "E^(@)=0.00V`
C. Both reactions are feasible
D. None of these

Answer

A

Explanation

`Ag^(+)(aq)+e^(-) to Ag(s),E^(@)=+0.80V`
`H^(+)(aq)+e^(-) to (1)/(2)H_(2)(g),E^(@)=0.00V`
On the basis of their standard reduction potential `(E^(@))` values, cathode reaction is given by the one with higher `E^(@)` values.
Thus, `Ag^(+)(aq)+e^(-) to Ag(s)` reaction will be more feasible at cathode.