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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_((0.002M))^(+) to Ni_((0.160M))^(2+) + 2Ag_((s)) , "Given " E_("cell")^@ = 1.05 V `

Text Solution

Verified by Experts

`E_(cell)=E_(cell)^@-0.059/n log""(pro ducts)/(reactants)`
`=1.05-0.059/2log""([Ni^(2+)][Ag]^2)/([Ag^+]^2[Ni])`
`=1.05-0.0295log""0.160/((0.0024)^2)`
`=1.05-0.0295log 1 times 10^-3 - log40`
`=1.05-0.0295 times -3-1.6`
`=1.05-0.0295 times 4.6`
=0.9143 V
`1.0V`
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(a) Calculate the e.m.f. of the cell in which the following reactions takes place : Ni + 2Ag_((0.002M))^(+) rarr Ni^(2+) + Ag_((0.160M)(s)) Given E_("cell")^(0) - 1.05 V . (i) State kohlrausch's law of Independent Migration of ions. (ii) What is meant by limiting molar conductivity ?

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