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Gibb's Energy and Nernst Equation

Answer, wheth...

Question

Answer, whether under standard conditions, the following reactions are possible or not:
(i) Will copper reduce $A g^{+}$ to $A g$ ? Given: $E_{A g^{+} / A g}^{\circ} = 0.799 v o l t; E_{C u^{2 +} / C u}^{\circ} = 0.337 v o l t$ .
(ii) Will $F e^{3 +}$ be reduced to $F e^{2 +}$ by $S n^{2 +}$ ion? Given:
$F e^{3 +} / F e^{2 +} = 0.771 v o l t$ ;
$S n^{2 +} / S n^{4 +} = - 0.250 v o l t$
(iii) Would you use a silver spoon to stir a solution of $C u (N O_{3})_{2}$ ?

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Solution

$i)$ Yes copper will reduce $A g^{+}$ to $A g$ because reduction potential of $A g^{+} / A g$ is greater than that of $C u^{2 +} / C u .$
$i i)$ Yes, because $E ° F e^{3 +} / F e^{2 +} > E ° s n^{4 +} / s n^{2 +} .$
$i i i) .$ Yes, because silver can't reduce copper.

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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. Determine the equilibrium constant of the following reaction at

298 K

:

2 F e^{3 +} + S n^{2 +} \to 2 F e^{2 +} + S n^{4 +}

E_{S n^{4 +} / S n^{2 +}}^{\circ} = 0.15 v o l t; E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.771 v o l t

E^{\circ}

values to calculate

△ G^{\circ}

for the reaction

F e^{2 +} + A g^{+} \to F e^{3 +} + A g

E_{A g^{+} / A g}^{\circ} = 0.80 v o l t

E_{P t / F e^{3 +}, F e^{2 +}}^{\circ} = 0.77 v o l t

Q. The two half-cell reactions of an electrochemical cell is given as

{A g}^{+} + e^{-} ⟶ A g; E_{{A g}^{+} | A g}^{o} = - 0.3995 V

{F e}^{2 +} ⟶ {F e}^{3 +} + e^{-}; E_{{F e}^{3 +} | {F e}^{2 +}}^{o} = - 0.7120 V

The value of cell EMF will be:

Q. At equimolar concentration of

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

[A g^{+}]

be so that the voltage of the galvanic cell made from

(A g^{+} / A g and F e^{3 +} / F e^{2 +})

electrodes equals zero? The reaction is

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

E_{A g^{+} / A g}^{0} = 0.799

E_{F e^{+} / F e^{2 +}}^{0} = 0.771 volt., 10^{- 0.47} = 2.94)

Give your answer upto two decimal only.

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