1.

a) Calculate the e.m.f. of the cell represented below: Ni_((s))|Ni_(0.1M)^(2+)||Ag_(0.01M)^(+)|Ag_((s))" at 298Given,"E_("cell")^(@)=1.05V,

Answer»

SOLUTION :Cell REPRESENTATION
`Ni|Ni^(2+)||Ag^(+)|Ag`
Applying nernst EQUATION,
`E_("cell")=E_("cell")^(@)-(0.0591)/(n)LOG""([Ni^(2+)])/([Ag^(+)]^(2))`
`=1.05-0.02955 log=(0.1)/((0.01)^(2))`
`=1.05-0.02955log=(0.1)/((0.01)^(2))`
`=1.05-0.02955log""(0.1)/(0.0001)`
`=10.5-0.02955 log100`
`=1.05-0.02955log10^(2)rArr 2LOG10`
`=1.05-0.02955[2log10]`
`=1.05-0.059rArr 0.459V`


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