The cell in which the following reaction occurs
`2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(aq)+I_(2)(s)` has `E_(cell)^(0)=0.236V` at 298 K.
Calculate the stadard gibbs energy and the equilibrium constant of the cell reaction.

Explanation

`Delta_(r )G^(Theta) = -nF E_("cell")^(Theta)`
`n = 2, E_("cell")^(Theta) = 0.236 V , F=96487" C mol"^(-1)`
`:.Delta_(r ) G^(Theta) = -2 xx 96487 "C mol"^(-1) xx 0.236V`
`= -45541 CV " mol"^(-1) = -45541" J mol"^(-1)`
`= -45.54" kJ mol"^(-1)`
`Delta G^(Theta) = -2.303 "RT log K"`
`:.logK= +(45541)/(2.303 xx 8.314 xx298) = 7.98`
`K=95.5 xx 10^(6)`