wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

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.


A

15.45

No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
15.59
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
15.93
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
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.

Ecell = Eo - 2.303 2.303RTnFlog Q

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

So, we have
0 = Eo 2.303 2.303RTnFlog K

Rearranging, Eo = 2.303 2.303RTnF log K

Now let us plug in the values given,
E0cell = 0.46 V

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

We would end up with,

0.46 = 0.0592log K

log K = 15.59

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Industrial Preparation of Ammonia
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon