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

Explanation

Data: `E_("cell")^(0)=0.236V, T=298K, n=2, F=96500, R=8.314J//K mol`
Formula 1 . `DeltaG^(0)=-n E_("cell")^(0)F`
`=-2 xx 0.236 xx 96500 =-45.55kJ`
Formula 2. `DeltaG^(0)=-2.303 RRT log K_(C)`
`-45.55=-2.303 xx 8.314 xx 298 xx log K_(C)`
`log k_(c)=(4550)/(2.303 xx 8.314 xx 298)`
`log k_(c)=7.983`
`k_(C)="Antilog "7.983=9.62 xx 10^(7)`