In the above diagram, the standard electrode potentials are given in volts (over the arrow). The value of is [2025]

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Solution

Q.
${FeO}_{4}^{2 -} \overset{+ 2.0 V}{\to} {Fe}^{3 +} \overset{0.8 V}{\to} {Fe}^{2 +} \overset{- 0.5 V}{\to} {Fe}^{0}$

In the above diagram, the standard electrode potentials are given in volts (over the arrow).

The value of $E_{{FeO}_{4}^{2 -} / {Fe}^{2 +}}^{⊝}$ is [2025]

1 2.1 V

2 1.7 V

3 1.2 V

4 1.4 V

Ans.
(2)

When two reactions are added their Gibbs energy change is added, as Gibbs energy change is an extensive property.

$Δ G_{4}^{\circ} = Δ G_{1}^{\circ} + Δ G_{2}^{\circ}$

$- n_{4} F E_{4}^{\circ} = - n_{1} F E_{1}^{\circ} - n_{2} F E_{2}^{\circ}$

$- 4 F E_{4}^{\circ} = - 3 F \times 2 - 1 F \times 0.8$

$E_{4}^{\circ} = \frac{6.8}{4} V = 1.7 V$

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