In the cell `Pt_((s)) |H_2 (8,1 bar) |HCl_((aq))| AgCl_((s)) |Ag_((s))| Pt_(fs)`
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 ______ V.
(Given, `(2.303 RT)/F `= 0.06V at 298 K)

Answer

`0.2`

Explanation

At anode: `H_(2(g)) rarr 2H_((a))^(+) + 2e^(-) xx1`
At Cathode: `AgCl_((s)) + e^(-) rarrAg_((s)) + Cl_((a))^(-)xx 2`
Net reaction: `H_(2(g)) +2 AgCl_((s))overset((o))rarr 2H_((a))^(+) + 2 Ag_((s))+2Cl_(("ial"))^(-)`
`E_("cell")=E_("cell")^(s)-(0.06)/2log_(10)[H^(+)]^2[Cl]^2`
`0.92 - (E_(H_2M^(+))^(a)+E_(A_BC)iAgCr)`
`-(0.06)/2log_(10)[(10^(-6))^2xx(10^(-6))^2]`
`0.92 -(01E_("AgCiAe.C^(-)))0`
`.03log_(10)(10^(-6))^4`
`E_(AgCl//Ag,Cl^(-))^(0)=0.92+0.03xx(-24)`
= 0.2 V