1.

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.

Answer»

Solution :`n=2`
`DeltaG^(@)=-nFE_("CELL")^(@)=-2xx96500xx0.236J=-45.55kJ//mol`
`DeltaG^(@)=-2.303"RT LOG K"_(c)`
`logK_(c)=(DeltaG^(@))/(-2.303RT)=(45.55xx10^(3))/(2.303xx8.314xx298)=7.983`
`K_(c)="antilog (7.982)"=9.616xx10^(7)`


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