Question

Calculate the potential of the following cell reaction at 298 K
`Sn^(4+)(1.50 M)+Zn(s) to Sn^(2+)(0.50 M)+Zn^(2+)(2.0 M)`
The standard potential, `E^(@)` of the cell is 0.89 V. Whether the potential of the cell will increase or decrease if the concentration of `Sn^(4+)` is increased in the cell.

Answer 1

Correct Answer - 0.8952 V
Cell reaction : `Zn(s)+Sn^(4+)(1.5" M") to Sn^(2+)(0.5" M")+Zn^(2+)(2.0" M")`
`E_(cell)=[E_(Sn^(4+)//Sn^(2+))^(@)-E_(Zn^(2+)//Zn)^(@)]-(0.059)/(n)"log"([Zn^(2+)][Sn]^(2+))/([Sn^(4+)])`
`=E_(cell)^(@)-(0.0591)/(2)"log"((2.0)xx(0.5))/((1.50))=0.89-0.02955 log (0.6666)`
`=0.89-0.02955(-0.1761)=0.89+0.0052=0.8952" V "`