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Calculate the emf of the cell in which t...

Calculate the emf of the cell in which the following reaction takes place,
`Ni(s) + 2Ag^(+) ( 0.002M) rarr Ni^(2+) ( 0.160M) + 2Ag(s) `
Given that `E_("cell")^(@) = 1.05V`

Text Solution

Verified by Experts

From the given cell reaction and Nernst equation,
`E^(@) = E_("cell")^(@) - ( 0.0591)/( n ) log ""([Ni^(2+)])/([Ag^(+)]^(2))`
`= 1.05 V - ( 0.0591)/( 2) log ""((0.160))/( (0.002)^(2))`
`= 1.05 - ( 0.0591)/( 2 ) log ( 4 xx 10^(4))`
`= 1.05 - ( 0.0591)/( 2) ( 4.6021)`
`= 1.05 - 0.14 = 0.91 V`
`E_("cell") = 0.91V`
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