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Reactivity with Halogens and Hydrogen (Group 2)

In a cell, th...

Question

In a cell, the following reactions take place
$F e^{2 +} \to F e^{3 +} + e^{-} E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.77 V$
$2 I^{-} \to I_{2} + 2 e^{-} E_{I_{2} / I^{-}}^{\circ} = 0.54 V$

The standard electrode potential for the spontaneous reaction in the cell is $x \times 10^{- 2} V$ at 208 K. The value of $x$ is (Nearest Integer)

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Solution

$F e^{2 +} \to F e^{3 +} + e^{-} E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.77 V$
$2 I^{-} \to I_{2} + 2 e^{-} E_{I_{2} / I^{-}}^{\circ} = 0.54 V$
The cell reaction is,
$2 F e^{2 +} + I_{2} \to 2 F e^{3 +} + 2 I^{-}$

$E_{c e l l}^{\circ} = E_{c a t h o d e}^{\circ} - E_{a n o d e}^{\circ}$
$= 0.77 - 0.54$
$= 0.23 V$
$= 23 \times 10^{- 2} V$

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