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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`. Ca

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The cell in whiCHM the following reaction occurs : 2Fe3+(aq)+2Ic-(aq)→2Fe2+(aq)+I2(s) has Ec- _(cell)=0.2136V at 298K . Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction. Select the correct answer from above options

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Correct Answer - 9.616×107 2Fe3++2e-→2Fe2+or2Ic-→I2+2e- Hence, for the given cell reaction, n=2 . ΔrGc-=-nFE c- cell -2×96500×0.236J =-45.55kJmol-1 ΔrGc-=-2.303RTlogKc logKc= ΔrGc- 2.303RT = -45.55kJmol-1 2.303×8.314×10-3kJK-1mol-1×298K =7.983 ∴Kc=Antilog(7.983)=9.616×107

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