A voltaic cell is set up at `25^(@)C` with following half cells : `Ag^(+)(0.001 M)|Ag` and `Cu^(2+)(0.10 M)|Cu` What would be the voltage of this cell
A voltaic cell is set up at `25^(@)C` with following half cells : `Ag^(+)(0.001 M)|Ag` and `Cu^(2+)(0.10 M)|Cu` What would be the voltage of this cell ? `(E_(cell)^(@)=0.45 V)`
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The cell reaction is :
`Cu(s) +2Ag^(+)(aq) to Cu^(2+)(aq)+2Ag(s)`
According to Nernst equation,
`E_(cell)=E_(cell)^(@)-(0.0591)/(n)"log"([Cu^(2+)])/([Ag^(+)]^(2))=0.46-(0.0591)/(2)"log"((0.10))/(0.001)^(2)`
`=0.46-(0.0591)/(2)"log"10^(5)`
=0.46-0.02955 (5 log 10) =0.46-0.1477=0.3125 V
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