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

Explanation

The cell reaction is
`Ni(s) +2Ag^(+)(aq) to Ni^(2+) (aq) +2Ag(s) , DeltaG^(Theta) = -nFE^(Theta)`
`EQ = 1.05V, n =2, F=96500 C" mol"^(-1)` K
`:.DeltaG^(Theta) = -(2" mol") xx (96500 "C mol"^(-1)) xx 1.05V `
`= -202650 VC = -20265650J`
Now `DeltaG^(Theta) = -2.303 RT" log "K_( c )`
`DeltaG^(Theta)= -202650J`
`R=8.314J K^(-1)"mol"^(-1) , T=298K`
`:.-202650= -2.303 xx 8.314 xx 298"log K"_(c )`
`"log K"_(C ) = (202 xx 650)/(2.303 xx 8.314 xx 298)`
or `"log "K_(C )=(202650)/(5705.8) =35.51`
`K_(C ) ="Angilog" 35.51 = 3.24 xx 10^(35)`