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Redox Reactions and Couple

ntGiven elect...

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ntGiven electrode potentials:n ntFe3+ plus e ---------Fe2+ ; Eo=0.771n ntI2+2e ----------------2I- ; Eo =0.536n ntEo cell for the cell reactionn nt2Fe3+ plus 2I- ----------2Fe2+ plus I2 is -n nt1. (2x0.771-0.536) =1.006 voltsn nt2. (0.771-0.5x0.536)=0.503 voltsn nt3. 0.771-0.536=0.253 voltsn nt4. 0.536-0.771=-0.235 voltsn

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{F e}^{3 +} + {3 e}^{-} ⟶ F e; E^{o} = - 0.036 v o l t

{F e}^{2 +} + {2 e}^{-} ⟶ F e; E^{o} = - 0.440 v o l t

E^{o}

{F e}^{3 +} + e^{-} ⟶ {F e}^{2 +}

F e^{2 +} + 2 e^{-}

⟶

F e; E^{o} = - 0.440 V

F e^{3 +} + 3 e^{-}

⟶

F e; E^{o} = - 0.036 V

(E^{o}

F e^{3 +} + e^{-}

\to

F e^{2 +}

F e^{2 +} + 2 e^{-} \to F e, E^{o} = - 0.440

F e^{3 +} + 3 e^{-} \to F e, E^{o} = - 0.036

(E^{o})

F e^{3 +} + e^{-} \to F e^{2 +}

I_{2} + 2 e^{-} \to 2 I^{-} (1 M)

E^{o} = + 0.54

B r_{2} + 2 e^{-} \to 2 B r^{-} (1 M); E^{o} = + 1.09

(E^{o})

A

E^{o} (V

I_{2} + 2 e^{-} \to 2 I^{-}; E^{o} = 0.54

C l_{2} + 2 e^{-} \to 2 C l^{-}; E^{o} = 1.36

M n^{3 +} + e^{-} \to M n^{2 +}; E^{o} = 1.50

F e^{3 +} + e^{-} \to F e^{2 +}; E^{o} = 0.77

O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O; E^{o} = 1.23

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