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For the reaction, AgCl(s)+H(2)(g)"(1 a...

For the reaction,
`AgCl(s)+H_(2)(g)"(1 atm)"rarr Ag(s)+2H^(+)(0.1M)+2Cl^(-)(0.1M)`
`DeltaG^(@)=-43600J` at `25^(@)C`. Calculate the emf of the cell `[log 10^(-n)=-n]`

Text Solution

Verified by Experts

Gibbs free energy of reaction, `DeltaG^(@)=-nFE_("cell")^(@)`
`DeltaG^(@)=-43600J, n=2, E_("cell")^(@)=?, F="96500 C.mol"^(-1)`
`-43600J=-2xxE_("cell")^(@)xx96500, E_("cell")^(@)=0.22V`
`E_("cell")=E_("cell")^(@)-(0.0591)/(n)log(("[Product]")/("[Reactant]"))`
`E_("cell")=E_("cell")^(@)-(0.0591)/(n)log.([H^(+)]^(2).[Cl^(-)]^(2))/([H_(2)])`
Putting all the values,
`E_("cell")=0.22-(0.0591)/(2)log.((0.1)^(2)(0.1)^(2))/(1)`
`=0.22-(0.0591)/(2)log(10^(-4))=0.3382V`
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