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Electrolytic Cell

40. At 25 deg...

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40. At 25 degree celcius the value of K for the equilibrium (F^{+3}) +(Ag) \xrightarrow{} (Fe^{+2}) + (Ag+) is 0.531mol/litre. The standard electrode potential for (Ag^+) + e^-\xrightarrow{} (Ag) is 0.799V. what is the standard potential for (Fe^{+3}) +(e)^-> (Fe^{+2})? Use log(0.531)=-0.275

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E_{F e^{3 +} / F e^{2 +}}^{o} = 0.771 V

E_{A g^{+} / A g}^{o} = 0.799 V

The minimum conc. of Ag

^{+}

that would remain unreduced by a standard

F e^{3 +} / F e^{2 +}

electrode at equilibrium is:

Q. Using the standard electrode potential , find out the pair between which redox reaction is not feasible .

E^{0}

F e^{3 +} / F e^{2 +}

I_{2} / I^{-}

C u^{2 +} / C u

A g^{+} / A g

Q. At equimolar concentrations of

F e^{2 +}

F e^{3 +}

[A g^{+}]

be so that the voltage of the galvanic cell made from

A g^{+} / A g

F e^{3 +} / F e^{2 +}

electrodes equals zero? The reaction is

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

. Determine the equilibrium constant at

25^{\circ} C

for the reaction. (Given:

E_{A g^{+} / A g}^{\circ} = 0.799 v o l t

E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.771 v o l t

Q. The standard potential for the reaction,

{A g}^{+} (a q .) + {F e}^{2 +} (a q .) ⟶ {F e}^{3 +} (a q .) + A g (s)

0.028 V

. What is the standard free energy change for this reaction?

Given standard electrode potentials:

$F e^{3 +} + 3 e^{-} \to F e; E^{0} = - 0.036 V$

$F e^{2 +} + 2 e^{-} \to F e; E^{0} = - 0.440 V$

The standard electrode potential $E^{o}$ for $F e^{3 +} + e^{-} \to F e^{2 +}$ is:

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