Determine the values of equilibrium constant `(K_C) and DeltaG^o` for the following reaction :

Explanation

The cell reaction is
`Ni(s)+2Ag^+(aq)toNi^(2+)(aq) +2Ag(s)`,
`DeltaG^o=-nFE^o`
`E^o=1.05V,n=2,f=96500C//"mol"`.
`DeltaG^o=-(2mol)xx(96500C//mol)xx(1.05V)`.
`=-202650 CV (1CV=1)`
`=-202650J`
Colculation of K in the from `DeltaG^o`,
`DeltaG^o=-202650J,R=8.314J//mol//K`.
`T=298k`.
`logK=(DeltaG^o)/(2.303RT)=(-202650J)/((2.303)xx(8.314J//mol//K)xx(298K))`
`=K=(-202650)/5705.84832=35.51`
`or K=0.35xx10^2`