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Calculate the e.m.f. of the cell in whic...

Calculate the e.m.f. of the cell in which the following reaction takes place :
`Ni(s) +2Ag^(+)(0.002 M)to Ni^(2+)(0.160 M)+2Ag(s)`
Given `E_(cell)^(@)`=1.05 v

Text Solution

Verified by Experts

Applying nernst equation to the given cell reaction,
`E_(cell)=E_(cell)^(@)-(0.0591)/(n)"log"([Ni^(2+)])/([Ag^(+)]^(2))=1.05V-(0.0591)/(2)"log"(0.160)/((0.002)^(2))=1.05-(0.0591)/(2)log(4xx10^(4))`
`=1.05-(0.0591)/(2)(4.6021)=1.05-0.14V=0.91V`
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