In the cell `Pt(s)|H_(2)(g,1bar)|HCl (aq)| AgCl(s)|Ag(S)|Pt(s)` the cell potential is 0.92V when a `10^(-6)` mola1 HCl Ssolution is used. The standard electrode potential of `(ACl//Ag,Cl^(-))` electrode is :
`{given, (2.30Rt)/(F) = 0.6V at 298K}`

In the cell Pt (s) | H_(2) (g, 1 " bar")| HCl (aq)| AgCl(s) | Ag(s) | Pt(s) the cell potential is 0.92 V when a 10^(-6) molal HCl solution is used. The standard electrode potential of (AgCl//Ag, Cl^(-)) electrode is {Given, (2.303RT)/(F) = 0.06V at 298 K}

In the cell Pt (s) | H_(2) (g, 1 " bar")| HCl (aq)| AgCl(s) | Ag(s) | Pt(s) the cell potential is 0.92 V when a 10^(-6) molal HCl solution is used. The standard electrode potential of (AgCl//Ag, Cl^(-)) electrode is {Given, (2.303RT)/(F) = 0.06V at 298 K}

Pt,H_(2) (1bar) |HCl_(aq)|AgCl(s)|Ag has cell potential 0.92V at 25^(@)C when 10^(-6)MHCl is used. What is the standard free energy change for the reaction H_(2(g))+2AgCl_((s))to2Ag_((s))+2H_(aq)^(+)+2Cl_(aq)^(-) ?

The measured emf of the cell- Pt(s)H_2(G,1bar)|H^+(aq,1M)|| Cu^(2+)(aq,1M)|Cu(s)is 0.34V . What is the standard electrode potential of the half cell corresponding to the reaction?

The standard potential of the following cell is 0.23 V at 15^(@)C and 0.21 V" at "35^(@)C: Pt|H_(2)(g)|HCl(aq)|AgCl(s)|Ag(s) (3) Calculate the solubility of AgCl in water at 25^(@)C . Given : Standard reduc-tion potential of Ag^(+)(aq)|Ag(s) is 0.80 V at 25^(@)C .