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Standard IX

Chemistry

Electrolysis of Water

Using the sta...

Question

Using the standard electrode potentials given in the table, predict if the reaction between the following is possible.
$B r_{2} (a q)$ and $F e^{2 +} (a q)$

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Solution

At cathode: Oxidation half reaction is $[F e^{2 +} (a q) \to F e^{3 +} (a q) + e^{-}]; E_{F e^{3 +} / F e^{2 +}}^{0} = + 0.77 V$ .

At anode: Reduction half reaction is $[B r_{2} (a q) + 2 e^{-} \to 2 B r^{-} (a q)]; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$ .

The net cell reaction is $B r_{2} (a q) + 2 F e^{2 +} (a q) \to 2 B r^{-} (a q) + 2 F e^{3 +} (a q); E_{c e l l}^{0} = E_{c a t h o d e}^{o} - E_{A n o d e}^{o} = 1.09 - 0.77 = + 0.32 V$ .

Since, the cell potential is positive, the reaction is feasible.

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$E_{\frac{1}{2} \frac{t_{2}}{1^{-}}}^{\circ} = + 0.541 V E_{(\frac{C u^{2 +}}{C u})}^{\circ} = + 0.34 V E_{(\frac{1}{2} \frac{B r_{2}}{B r^{-}})}^{\circ} = + 1.09 V E_{(\frac{A g^{+}}{A g})}^{\circ} = + 0.80 V E_{(\frac{F e^{3 +}}{F e^{2 +}})}^{\circ} = + 0.77 V$

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Using the standard electrode potentials given in the table, predict if the reaction between the following is possible.Br2(aq) and Fe2+(aq)

Using the standard electrode potentials given in the table, predict if the reaction between the following is possible.
$B r_{2} (a q)$ and $F e^{2 +} (a q)$