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

The cell in which the following cell reaction occurs, `2Fe _((aq))^(3+

1.	The cell in which the following cell reaction occurs, `2Fe _((aq))^(3+)+2I_((aq))^(-)to 2Fe _((aq))^(2+)+I_(2(s))` has `E_(cell)^(0)=0.236V` at 298 K. Calculate the standard Gibbs energy and the equilibrium costant of the cell reaction.
Answer» Two half reactions for the given redox reaction may be written as : `2Fe_((aq))^(3+)+2e^(-)to2Fe_((aq))^(2+),2I^(-)to I_(2)+2e^(-)` 2 moles of electrons are involved in the reactin, so `n=2` `DeltaG^(0)=-nFE_(cell)^(0)=(-2mol)xx(96500mol ^(-1))(0.236V)` `=- 45548CV=-454548J` `Delta_(r)G^(0) =-45. 55kj` `log K_(c)=(DeltaG^(0))/(2.303RT)` `=((-45.55kj))/(2.303xx(8.314xx10^(-3)kJK^(-1))xx(298K))=7.983` `K_(c)="Antilig"(7.983)=9.616xx10^(7)` `K_(c)=9.616xx10^(7)`

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

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