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Representation of Cell

Construct gal...

Question

Construct galvanic cells from the following pairs of half cells and calculate their emf at $25^{o} C .$

$F e^{3 +} (a q, 0.1 M), F e^{2 +} (a q, 1 M) | P t (s); E_{F e^{3 +} / F e^{2 +}}^{0} = 0.77 V$

$A g (s) | A g C l (s) ∣ C l^{-} (a q, 0.001 M); E_{A g C l / A g}^{0} = 0.22 V$

E_{c e l l} = 0.313 V

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E_{c e l l} = 0.567 V

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E_{c e l l} = 0.023 V

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E_{c e l l} = 1.13 V

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Solution

The correct option is A $E_{c e l l} = 0.313 V$
For the half - cell reaction,
From the standard reduction potential values we can see $A g (s)$ will act as anode in the galvanic cell.
Applying nernst eq. for individual half cells:
$F e^{3 +} (a q) + e^{-} ⇌ F e^{2 +} (a q)$
By Nernst equation,

$E_{F e^{3 +} / F e^{2 +}} = E_{F e^{3 +} / F e^{2 +}}^{0} - \frac{0.0591}{1} l o g \frac{[F e^{2 +}]}{[F e^{3 +}]}$

$= 0.77 - \frac{0.0591}{1} l o g \frac{1}{0.1} = 0.71 V$

And, for the half - cell reaction,

$A g C l (s) + e^{-} ⇌ A g (s) + C l^{-} (a q)$

$E_{C l^{-} / A g C l / A g} = E_{C l^{-} / A g C l / A g}^{0} - \frac{0.0591}{1} l o g [C l^{-}]$

$E_{C l^{-} / A g C l / A g} = 0.22 - \frac{0.0591}{1} l o g 0.001$

$E_{C l^{-} / A g C l / A g} = 0.22 - \frac{0.0591}{1} l o g 10^{- 3}$

$E_{C l^{-} / A g C l / A g} = 0.22 + \frac{3 \times 0.0591}{1}$

$E_{C l^{-} / A g C l / A g} = 0.397 V$

$∴$ Cell may be represented as

$A g (s) | A g C l (s) ∣ C l^{-} (a q) ∣∣ F e^{3 +} (a q), F e^{2 +} (a q) | P t (s)$

$E_{c e l l} = reduction potential of RHS electrode - reduction potential of LHS electrode$

$E_{c e l l} = 0.71 - 0.397 E_{c e l l} = 0.313 V$

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Similar questions

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

(i) 2Cr(s) + 3Cd²⁺(aq) → 2Cr³⁺(aq) + 3Cd

(ii) Fe²⁺(aq) + Ag⁺(aq) → Fe³⁺(aq) + Ag(s)

Calculate the Δ_rG^θ and equilibrium constant of the reactions.

298 K

C d (s) | C d_{(a q)} {(0.001 M) | | H^{+}}_{(a q)} (0.01 M) | H_{2} (g), 1 a t m | P t

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

25^{o} C .

C d^{2 +} (a q, 1 M) ∣ C d (s); E_{C d^{2 +} / C d}^{0} = - 0.40 V

H g_{2} C l_{2} (s) ∣ H g (l) ∣ C l^{-} (a q, 0.1 M); E_{C l^{-} / H g_{2} C l_{2} / H g}^{0} = 0.28 V

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