Calculate the equilibrium constant for the reaction- at 25oC Cus - 2Ag- aq - Cu2- aq - 2Ag s Eocell - 0-47 V- R - 8-134 JK-1 F - 96500 C is

The correct option is D 8.5× 10^15 ...

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Gibb's Energy and Nernst Equation

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Question

Calculate the equilibrium constant for the reaction, at $25^{o} C$

$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$

$E_{c e l l}^{o} = 0.47 V, R = 8.134 J K^{- 1} F = 96500 C$ is

1.8 \times 10^{15}

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8.5 \times 10^{15}

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1.8 \times 10^{10}

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85 \times 10^{15}

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K_{c}

C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)

10 \times 10^{15}

E_{c e l l}^{o}

298 K

[2.303 \frac{R T}{F} a t 298 K = 0.059 V]

C u (s) + 2 {A g}^{+} (a q .) ⇌ {C u}^{2 +} (a q) + 2 A g (s)

25^{o} C

E_{c e l l}^{o} = 0.47 v o l t, R = 8.314 J K^{- 1} {m o l}^{- 1}, F = 96500 c o u l o m b

E^{\circ}

C u (S) + 2 A g^{+} (a q) \to C u^{2} (a q) + 2 A g (S)

Calculate the equilibrium constant of the reaction.
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$ , $E_{c e l l}^{⊖} = 0.46 V$

C u (s) + 2 A g^{+} (a q) ⇋ C u^{2 +} (a q) + 2 A g (s),

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