In the cell Pt(s),H2(g)| 1bar HCl (aq) | Ag(s) | Pt(s) the cell potential is 0.92V when 10⁻² molal HCl solution is used. The standard electrode potential of (AgCl/Ag,Cl⁻) electrode is: [Given: 2.303RT/F = 0.06V at 298K] 0.20V 0.076V 0.040V 0.94V

The half-cell reactions are,
At Anode: 1/2H2(g) →H+(aq)+e⁻
At Cathode: AgCl(s)+e⁻ →Ag(s)+Cl⁻(aq)
Complete reaction: AgCl(s)+1/2H2(g) →Ag(s)+Cl⁻(aq)+H+(aq)
We know, E⁰cell=E⁰cathode−E⁰anode=(SRP)cathode−(SRP)anode
We know standard hydrogen potential is assumed to be zero.
So,(SRP)anode=0
Let,(SRP)cathode=x
So,E⁰cell=x
Now we use the Nernst equation,
Ecell=E⁰cell−(2.303RT/nF)log(Q) ⇒Ecell=E⁰cell−(0.06/1)log([Cl⁻][H+])
n=1; 0.92=x−0.06log(10⁻²×10⁻²)
⇒x=0.20V