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

The e.m.f. of cell for spontaneous cell reaction having two electrodes as Ag|Ag+||Cu2+|Cu containing 1MCu2+ and 1MAg+ ions after the passage of 9.65 ampere current for 1 hour will :

A
increase by 0.010V
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
decrease by 0.010V
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
increase by 0.020V
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
decrease by 0.020V
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A increase by 0.010V
Given,
Cu2++eCu+;ΔGo1=Eo1F×1
Cu++eCu;ΔGo2=Eo2F×1
----------------------------
by adding these equations
Cu2++2eCu;ΔGo3=[ΔGo1+ΔGo2]=[0.15F+0.5F]
or 2×Eo3F=0.65F
(as ΔG=nFEo)
Eo3=0.325V
So for reverse reaction.
CuCu2++2eEo=0.325V
CuCu2++2eEo=0.325V
2Ag++2e2AgEo=0.799V
Eocell=EoOPCu/Cu2++EoRPAg+/Ag
=0.325+0.799=0.474V

On passing the current through the given cell Ag will oxidise to Ag+ and Cu2+ will be reduced to Cu.
As same charge is passing throuth both solutions so
According to Faraday's law:
wE=i.t96500=9.65×360096500
=0.36 eq. of Ag+=0.36 mol of Ag+
=0.36 eq. of Cu2+
=0.362 mole of Cu2+ (as mole = equivalent/valency)
[Ag+]=1+0.36=1.36M
[Cu2+]=1.00.18=0.82M
For
Ag|Ag+||Cu2+|Cu cell,
$
E^o_{cell} = - 0.474 $
And according to Nernst equation,
E=EoOPAg+EoRPCu+0.0592log[Cu2+][Ag+]2
Initially Cu2+=1M and Ag+=1M
Ecell=Eocell=0.474
After electrolysis Cu2+=0.82M,Ag+=1.36M
Ecell=Eocell+0.0592log0.82(1.36)2
=Eocell0.010=0.4740.010=0.484V
Eocell is negative for Ag+|Ag||Cu2+|Cu and is 0.474V
As for spontaneous reaction E should be positive and it was 0.474 V in first case and 0.484 V in II case so it increases by
0.010 V.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Nernst Equation
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon