1.

Calculate the potential of the following cell reaction at 298K Sn^(4+)(1.50M)+Zn(s)toSn^(2+)(0.50M)+Zn^(2+)(2.0M) 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? (R=8.314JK^(-1)mol^(-1),F=96500" C "mol^(-1))

Answer»


Solution :`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.


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