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 ?

Explanation

Higher the standard reduction potential of a species, more easily it is reduced at the cathode. As `Ag^(+)(aq)` has greater standard reduction potential, therefore, the reaction that will occur at the cathode is
`Ag^(+)(aq)+e^(-)toAg(s)`.