The equilibrium constant of the reaction Cus-2Ag- aq - Cu2- aq -2Ag s -E0-0-46V at 298 K is-

The correct option is A 4.0× 10^15 nFE=RT ln(K) #160; #160; #160;where n=2 (2 electrons are exchanged) 2× 96500× 0.46=8.314× 298×ln K ...

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Equilibrium Constant from Nernst Equation

The equilibri...

Question

The equilibrium constant of the reaction
$C_{u} (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s); E^{0} = 0.46 V a t 298 K$ is:

4.0 \times 10^{15}

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2.4 \times 10^{10}

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2.0 \times 10^{10}

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4.0 \times 10^{10}

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Solution

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The equilibrium constant of the reaction:

$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s); E^{\circ} = 0.46 V$ at 298K is :

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),

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

E^{0} = 0.46 V

C u + 2 A g^{+} (a q) ⟶ {C u}^{2 +} (a q) + 2 A g

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