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Calculate the e.m.f. of the following ce...

Calculate the e.m.f. of the following cell at `25^(@)C`
`Mg(s)//Mg^(2+)(0.01 M)||Sn^(2+)(0.1 M)//Sn(s)`
Given `" " E_(Mg^(2+)//Mg)^(@)=-2.34 V, E^(@)Sn^(2+)//Sn=-0.136 V`
Also calculate the maximum work that can be accomplished by the operation of the cell.

Text Solution

Verified by Experts

Calculate of the cell e.m.f.
According to Nernst equation,
`E_(cell)=E_(cell)^(@)-(0.0591)/(n)"log"([Mg^(2+)(aq)])/([Sn^(2+)(aq)])`
`E_(cell)^(@)=E_(cathode)^(@)-E_(anode)^(@)=-0.136-(-2.34)=2.204 V`
`E_(cell)=2.204 V-(0.0591)/(n)"log"(0.01)/(0.1)`
`=2.204V-(0.0591)/(2)"log"(10^(-1))`
=2.204 V+0.02955 V=2.23 V
Calculate of maximum work `(DeltaG^(@))`
`(-DeltaG^(@))=nFE_(cell)^(@)=(2"mol")xx(96500" C mol"^(-1))xx(2.204 V)`
`425372" CV"=425372 J=425.372 kJ`
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