[" 10.(a) Following reactions occur at cathode during the clectrolysis of aquoous sher "],[" chloride solution: "],[qquad [Ag'(aq)+c longrightarrow,Ag(s),E''=+0.80V],[H'(aq)+e,longrightarrow(1)/(2)H_(2)(B),E''=0.00V],[" Conthe basis of their standard reduction dectrode potatioll "],[" reaction is fasible at the cathode and why? "]]

Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution : Ag^(+)(aq)+e rarr Ag(s)E^(@)=+0.80V H^(+)(aq)+erarr(1)/(2)H_(2)(g)E^(@)=+0.00V Onn the basis of their standard reduction electrode potential (E^(@)) values, which reaction is feasible at the cathode and why?

Following reactions occur at cathode during the electrolysis of aqueous copper (II) chloride solution: CU_((aq))^(2+)+ 2e^(-)rightarrow Cu_(s), E^(@) = + 0.34V H_((aq))^(+) +e^(-) rightarrow (1)/(2)H_(2(s)), E^(@) = 0.00V On the basis of their standard reduction electrode potential (E^(@)) values, which reaction is feasible at the cathode and why?

Following reactions occur at cathode during the electrolysis of aqueous copper (II) chloride solution: CU_((aq))^(2+)+ 2e^(-)rightarrow Cu_(s), E^(@) = + 0.34V H_((aq))^(+) +e^(-) rightarrow (1)/(2)H_(2(s)), E^(@) = 0.00V On the basis of their standard reduction electrode potential (E^(@)) values, which reaction is feasible at the cathode and why?

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 ?

Following reactions can occur at cathode during the electrolysis of aqueous silver nitrate solution using Pt electrodes : Ag^(+)""_((aq)) ""^(+e^(-))to Ag""_((s)),E^(@)=0.80V H^(+)""_((aq)) ""^(+e^(-))to 1/2H_(2(g)),E^(@)=0.00V On the basis of theri standars electrode protential values, which reaction is feasible at cathode and why ?

Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.80V Co^(2+)(aq) + 2e(-) rightarrow Co(s) E^(@) = -0.28V Use the standard reduction potentials to determine the standard potential for the reaction: Co(s) + 2Ag^(+)(aq_) rightarrow Co^(2+)(aq) + 2Ag(s)