1.

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

Answer»

Solution :`2Fe^(3+)+2e^(-)to2Fe^(2+)` or `2I^(-)toI_(2)+2e^(-)`
`Delta_(r)G^(@)=nFE_(cell)^(@)=-2xx96500xx0.236J=-45.55kJ" "MOL^(-1)`
`Delta_(r)G^(@)=-2.303RT" LOG "K_(c)` or `"log "K_(c)=(Delta_(r)G^(@))/(2.303RT)=(-45.55" kJ "mol^(-1))/(2.303xx8.314xx10^(-3)" kJ "K^(-1)xx298K)=7.983`
`thereforeK_(c)=`ANTILOG `(7.983)=9.616xx10^7`


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