Use E-circ- values to calculate triangle G-circ- the reactionFe-2- - Ag-rightarrow Fe-3- - AgE-circ-Ag-Ag- - 0-80 volt and E-circ-Pt- Fe-3- Fe-2- - 0-77 volt-

E-x2218-cell-0-03-xA0-volt-x25B3-G-x2218-x2212-nFE-x2218-cell-x2212-2895-xA0-J-

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Standard XII

Chemistry

Gibb's Energy and Nernst Equation

Question

Use $E^{\circ}$ values to calculate $△ G^{\circ}$ for the reaction
$F e^{2 +} + A g^{+} \to F e^{3 +} + A g$
$E_{A g^{+} / A g}^{\circ} = 0.80 v o l t$ and $E_{P t / F e^{3 +}, F e^{2 +}}^{\circ} = 0.77 v o l t$ .

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Solution

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$E_{c e l l}^{\circ} = 0.03 v o l t, △ G^{\circ} = - n F E_{c e l l}^{\circ}$
$- 2895 J$ .

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Similar Questions

Use

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

and

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

View Solution

At equimolar concentrations of

F e^{2 +}

and

F e^{3 +}

, what must

[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

. Determine the equilibrium constant at

25^{\circ} C

for the reaction. (Given:

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

and

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

View Solution

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:

View Solution

At equimolar concentrations of

F e^{2 +}

and

F e^{3 +}

, what must [

A g^{+}

] be so that the voltage of the galvanic cell made from the (

A g^{+} | A g)

and (

F e^{3 +} | F e^{2 +})

electrodes equals zero ?

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

E_{A g^{o} | A g}^{o} = 0.7991; E_{F e^{3 +} | F e^{2 -}}^{o} = 0.771

View Solution

Answer, whether under standard conditions, the following reactions are possible or not:
(i) Will copper reduce

A g^{+}

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 +}

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}

View Solution

Use E∘ values to calculate △G∘ for the reactionFe2++Ag+→Fe3++AgE∘Ag+/Ag=0.80 volt and E∘Pt/Fe3+,Fe2+=0.77 volt.

E∘cell=0.03 volt,△G∘=−nFE∘cell−2895 J.

Use $E^{\circ}$ values to calculate $△ G^{\circ}$ for the reaction
$F e^{2 +} + A g^{+} \to F e^{3 +} + A g$
$E_{A g^{+} / A g}^{\circ} = 0.80 v o l t$ and $E_{P t / F e^{3 +}, F e^{2 +}}^{\circ} = 0.77 v o l t$ .

$E_{c e l l}^{\circ} = 0.03 v o l t, △ G^{\circ} = - n F E_{c e l l}^{\circ}$
$- 2895 J$ .