A) \[Pt|{{H}_{2}}(g)|HCl(sol.n)|l\,AgN{{O}_{3}}(sol.n)|Ag\]
B) \[Ag|AgCl(s)|KCl(sol.n)|l\,HCl(sol.n)\]\[,\,{{H}_{2}}(g)|Pt\]
C) \[Pt|{{H}_{2}}(g)|KCl(sol.n)|l\,AgCl(s)\,l\,Ag\]
D) \[Pt|{{H}_{2}}(g)|HCl(sol.n)|l\,AgCl(s)\,l\,Ag\]
Correct Answer: D
Solution :
The cell reaction is : \[\frac{1}{2}{{H}_{2}}(g)+AgCl(s)\]\[{{H}^{+}}(aq)\]\[+C{{l}^{-}}(aq)+Ag(s)\] Obviously, here hydrogen is being oxidised and \[AgCl\] is getting reduced. Hence the correct cell representation will be: \[Pt|{{H}_{2}}(g),\,HCl\] (solution) \[|\,\,|\,AgCl(s)|Ag\]You need to login to perform this action.
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