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

`0.895V`, Increase

Explanation

`E=E_(cell)^(@)-(0.0591)/(n)"log"([Sn^(2+)][Zn^(2+)])/([Sn^(4+)])=0.89-(0.0591)/(2)"log"((0.5)(2.0))/(1.5)=0.895V`
if `[Sn^(4+)]` is incrased, the second factor will decrease or `E_(cell)` will increase.