Calculate the emf of the cell with the cell reaction `Ni _((s))+2Ag ^(+)(0.002M)to Ni^(2+)(0.160M) +2 Ag_((s))` `E_(cell)^(0)=1.05V.`

Calculate the emf of the cell with the cell reaction `Ni _((s))+2Ag ^(

1.	Calculate the emf of the cell with the cell reaction `Ni _((s))+2Ag ^(+)(0.002M)to Ni^(2+)(0.160M) +2 Ag_((s))` `E_(cell)^(0)=1.05V.`
Answer» From the given cell reaction and Nernst equation `E_(cell) =E_(cell)^(0) -(0.0591)/(n )log ""([Ni^(2+)])/([Ag^(+)]^(2))` `=1.05 V- (0.0591)/(2)log ""([0.160])/([0.002]^(2))` `=1.05 V-(0.0591)/(2)log (4xx 10^(4))` `=1.05 -(0.0591)/(2)(4.6021)` `=1.05 -0.14=0.91V=0.91V`

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