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

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 standard gibbs energy and the equilibrium constant of the cell reaction.

The cell in whiCHM the following reaction occurs : 2Fe^(3+)(aq)+2I^(c-)(aq) rarr 2Fe^(2+)(aq)+I_(2)(s) has E^(c-) _(cell)=0.2136V at 298K . Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

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

(a) The cell in which the following reactions occurs: 2Fe^(3+)(aq)=2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s) has E_(cell)^(@)=0.236V at 298 K. Calculate the standard Gibbs energy of the cell reaction. (Given: 1F=96,500" C "mol^(-1) ) (b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F=96,500" C "mol^(-1) )

The cell in which the following reaction occurs : 2Fe_(aq)^(3+) + 2I_(aq)^(-) to 2Fe_(aq)^(2+) + I_(2(s)) "has" E_("cell")^(o) = 0.236 V "at" 298 K The equilibrium constnat of the cell reaction is