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Oxidising Reagent and Reducing Reagent

A solution co...

Question

A solution contains ${F e}^{2 +}, {F e}^{3 +}$ and $I^{-}$ ions. This solution was treated with iodine at $35^{o} C$ . $E^{0}$ for ${F e}^{3 +} / {F e}^{2 +}$ is $+ 0.77 V$ and $E^{o}$ for $I_{2} / 2 I^{-} = 0.536 V$ . The favourable redox reaction is:

I_{2}

will be reduced to

I^{-}

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there will be no redox reaction

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I^{-}

will be oxidised to

I_{2}

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{F e}^{2 +}

will be oxidised to

{F e}^{3 +}

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Solution

The correct option is C $I^{-}$ will be oxidised to $I_{2}$
The favorable reaction is the oxidation of iodide ion to iodine.
$I^{-}$ will be oxidised to $I_{2}$

$2 e^{-} + {F e}^{+ 3} ⟶ {F e}^{2 +}; E = 0.77 V$
$2 I^{-} ⟶ I_{2} + 2 e^{-}; E = 0.536 V$
___________________________________________
$2 {F e}^{+ 3} + 2 I^{-} ⟶ 2 {F e}^{+ 2} + I_{2}; E = E_{o x} + E_{r e d}$
$= 0.77 - 0.536$
$= 0.164 V$
Since the value of the cell potential is positive, the reaction will take place.

Option C is correct.

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