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- 15-59B- 15-45C- 19-5D- 15-93

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Industrial Preparation of Ammonia

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

No worries! We‘ve got your back. Try BYJU‘S free classes today!

15.59

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

15.93

No worries! We‘ve got your back. Try BYJU‘S free classes today!

19.5

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

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

Suggest Corrections

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

Join BYJU'S Learning Program

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.