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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. |
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Answer» Solution :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)` |
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