1.

Calculate the cell e.m.f. at 25^(@)C for the cell: Mg(s)|Mg^(2+)(0.01M)||Sn^(2+)(0.1M)|Sn(s) Given E_(Mg^(2+)//Mg)^(@)=-2.34V,E_(Sn^(2+)//Sn)^(@)=-0.136V,1F=96,500" C "mol^(-1) Calculate the maximum work that can be accomplished by the operation of this cell.

Answer»


Solution :`MG+SN^(2+)toMg^(2+)+Sn,E_(cell)^(@)=-0.136-(-2.34)=2.204V`
`E_(cell)=E_(cell)^(@)-(0.0591)/(2)"log"([Mg^(2+)])/([Sn^(2+_)]), thereforeE_(cell)=2.204-(0.0591)/(2)"log"(0.01)/(0.1)=2.500V`
`w_(max)=-DeltaG^(@)=nFE_(cell)^(@)=2xx96500xx2.204=425372J` (Note that `w_(max)` is RELATED to `E_(cell)^(@)` and not `E_(cell)`).


Discussion

No Comment Found

Related InterviewSolutions