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Equilibrium Constant from Nernst Equation

The standard ...

Question

The standard potential for the reaction,
${A g}^{+} (a q .) + {F e}^{2 +} (a q .) ⟶ {F e}^{3 +} (a q .) + A g (s)$
is $0.028 V$ . What is the standard free energy change for this reaction?

- 3.702 k J {m o l}^{- 1}

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- 2.702 k J {m o l}^{- 1}

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- 5.702 k J {m o l}^{- 1}

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- 4.702 k J {m o l}^{- 1}

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Solution

The correct option is B $- 2.702 k J {m o l}^{- 1}$
Standard Free energy:-
$△ G^{\circ} = - n F E^{\circ}$
$n = n u m b e r o f e l e c t r o n s$
$F = F a r a d a y = 96500 C o u l o m b$
$E^{\circ} = S t a n d a r d P o t e n t i a l$
$J = C \times V$
$∴ △ G^{\circ} = - 1 \times 96500 C \times 0.028 V$
$∴ △ G^{\circ} = - 2702 J m o l^{- 1}$
$∴ △ G^{\circ} = - 2.702 k J m o l^{- 1}$

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Similar questions

Δ G^{o}

A g^{+} (a q) + \frac{1}{2} H_{2} (g) \to H^{+} (a q) + A g (s)

0.8 V

Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible:

(a) Fe³⁺(aq) and I^–(aq)

(b) Ag⁺(aq) and Cu(s)

(d) Ag(s) and Fe³⁺(aq)

(e) Br₂(aq) and Fe²⁺(aq)

Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible:

(i) Fe³⁺(aq) and I⁻(aq)

(ii) Ag⁺ (aq) and Cu(s)

(iii) Fe³⁺ (aq) and Br⁻(aq)

(iv) Ag(s) and Fe³⁺ (aq)

(v) Br₂(aq) and Fe²⁺(aq).

2 C r (s) + 3 C d^{2 +} (a q) \to 2 C r^{3 +} (a q) + 3 C d

F e^{2 +} (a q) + A g^{+} (a q) \to F e^{3 +} (a q) + A g (s)

Δ_{r} G^{⊖}

Calculate the standard cell potentials of galvanic cell in which the following reactions take place :

(i) $2 C r (s) + 3 C d^{2 +} (a q) \to 2 C r^{3 +} (a q) + 3 C d$

(ii) $F e^{2 +} (a q) + A g^{+} (a q) \to F e^{3 +} (a q) + A g (s)$

Calculate the $Δ_{r} G^{\circ}$ and equilibrium constant for the reactions

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