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For a standard cell, Cu(s)|Cu^(2+)(0.0...

For a standard cell,
`Cu(s)|Cu^(2+)(0.01M)||Ag^(+)(0.02M)|Ag(s)`
`E_(Cu^(2+)|Cu)^0=+0.34V,E_(Ag^+//Ag)^0=+0.80V`
Calculate EMF of the cell at `25^(@)C`.

Text Solution

Verified by Experts

`E_("cell")^0=E_(Ag^+|Ag)^0-E_(Cu^(2+)|Cu)^0`
`=(0.80-0.34)V`
=0.46V
`:.` From Nernst equation, we can write
`E_("cell")=E_("cell")^0-(0.059)/(2)log([Cu^(2+)])/([Ag^+]^2)`
`=0.46-(0.059)/(2)log(0.01)/((0.02)^2)`
`=0.46-(0.059)/(2)log25`
=0.46-0.04=0.42V
`:.` EMF of the cell at `25^(@)C` is 0.42V
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