Question

Write the cell representation and calculate equilibrium constant for the following redox reaction:

`Ni_((s))+2Ag_((aq))^+ (1M)->Ni_((aq))^(2+)(1M)+2Ag_((s)) " at "25^@ C`

`E_(ni)^+`=-0.25V and `E_(Ag)^+=0.799V`

Answer 1

`Ni_((s))+2Ag_((aq))^+ (1M)->Ni_((aq))^(2+)(1M)+2Ag_((s)) " at "25^@ C`

`E_(ni)^+`=-0.25V and `E_(Ag)^+=0.799V`

Cell representation :

`Ni_((s))|Ni_((aq))^(2+)(1M)||Ag_(aq)^+(1M)|Ag(s)`

Calculation of equilibrium constant

`E_(cell)^@=0.0592/n log_10K`

`E_"cell"^@=E_"Ag"^@-E_"Ni"^@`

=0.799-(-0.25)=1.049 V

Hence `1.049=(0.0592)/2 log_10K`

`log_10K=(1.049xx2)/0.0592=35.44`

`K=antilog(35.44)`

`=2.754xx10^35`