For the concentration cell Cu|Cu^(2+)(C_(1))||Cu^(2+)(C_(2))|Cu,DeltaG will be negative if Pt(Cl_(2)-P_(1))|HCl(0.1M)| Pt(Cl_(2)-P_(2)) the cell reaction is spontaneous if
Ag//AgCl_((s)), Cl_((aq))^(-) Ag_((s))+Cl^(-) hArr ?+e^(-)
For the cell (at 298K) Ag(s) | AgCl(s) | Cl^(-)(aq)|| AgNO_(3)(aq) | Ag(s) Which of the following is correct?
Reduction electrode potentials of half cells (1) Pt(H_(2))|H^(+)(C_(f)),(2)Pt(cl_(2))|(Cl^(-))(C_(2)) and (3) Ag^(+)|Ag^(+)(C_(3)) on inc reasing C_(1)C_(2) , and C_(3) (all gases are at 1 atm pressure)
for the electrochemical cell: Ag|AgCl(s)|KCl(aq)||AgNO_(3)(aq)|Ag . The overall cell reaction is
For the following cell reaction {:(Ag|Ag^(+)|AgCl|Cl^(-)|Cl_(2),Pt),(DeltaG_(f)^(@)(AgCl)=-109kJ/mol,),(DeltaG_(f)^(@)(Cl^(-))=-129kJ/mol and),(DeltaG_(f)^(@)(Ag^(+))=78KJ/mol.E^(@)):} of the cell is