Electra needs to answer this question to master this topic- Help her calculate the equilibrium constant of the following reaction-Cu s -2 Ag - aq - Cu 2- aq -2 Ag s E cell 0-0-46 VThe options below are log K values where K is the equilibrium constant-A- 15-45B- 15-59C- 15-93D- 19-5

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Le Chatelier's Principle for Del N Equals to 0

Electra needs...

Question

Electra needs to answer this question to master this topic.
Help her calculate the equilibrium constant of the following reaction:
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E_{c e l l}^{0} = 0.46 V$

The options below are $l o g K$ values where $K$ is the equilibrium constant.

15.45

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15.59

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15.93

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19.5

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Solution

The correct option is B 15.59
The first step is to write down the half-cell reactions

Reduction: 2Ag⁺ (aq) + 2e^- → 2Ag(s)

Oxidation: Cu(s) → Cu²⁺ (aq) + 2e^-

From this we get, n = 2

Let us first look at the general form of Nernst equation and try to derive our result.

E_cell= E^o - 2.303 $\frac{2.303 R T}{n F}$ log Q

But at equilibrium, E_cell goes to 0 and Q is replaced by K, which is the equilibrium constant.

So, we have
0 = E^o – 2.303 $\frac{2.303 R T}{n F}$ log K

Rearranging, E^o = 2.303 $\frac{2.303 R T}{n F}$ log K

Now let us plug in the values given,
E⁰_cell = 0.46 V

R = 8.314 JK^-1mol^-1
T = 25^o C = 298 K and n = 2

We would end up with,

0.46 = $\frac{0.059}{2}$ log K

log K = 15.59

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Similar questions

Electra needs to answer this question to master this topic.
Help her calculate the equilibrium constant of the following reaction:
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E_{c e l l}^{0} = 0.46 V$

The options below are $l o g K$ values where $K$ is the equilibrium constant.

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 :

Q. Given the equilibrium constant,

K_{c}

of the reaction :

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

10 \times 10^{15}

, calculate the

E_{c e l l}^{o}

of this reaction at

298 K

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

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

Q. The equilibrium constant for the equation:

E^{0} = 0.46 V

at 298 K is:

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

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Electra needs to answer this question to master this topic. Help her calculate the equilibrium constant of the following reaction: Cu(s)+2Ag+(aq)→Cu2+(aq)+2Ag(s) E0cell=0.46V The options below are logK values where K is the equilibrium constant.

Electra needs to answer this question to master this topic.
Help her calculate the equilibrium constant of the following reaction:
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E_{c e l l}^{0} = 0.46 V$

The options below are $l o g K$ values where $K$ is the equilibrium constant.