Choose the correct option(s) for the following concentration cell at 298K:
Zn(s)|Zn2+(aq,C1)||Zn2+(aq,C2)|Zn(s)
C1&C2 are concentrations of Zn2+ ions of each half-cell.
A
E0cell=0
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B
For a spontaneous reaction to take place, C1>C2
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C
For a spontaneous reaction to take place, C1<C2
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D
E0cell>0
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Solution
The correct option is C For a spontaneous reaction to take place, C1<C2 Zn(s)|Zn2+(aq,C1)||Zn2+(aq,C2)|Zn(s)
C1&C2 are concentrations of Zn2+ ions of each half-cell.
Anode: Zn(s)⇌Zn2+(aq)+2e−
Cathode: Zn2+(aq)+2e−⇌Zn(s)
Net cell reaction: Zn2+(C2)⇌Zn2+(C1)
Since in concentration cells, same metal and its solution is present.
Cathode and anode consist of same electrode. E0cathode=E0anode
For all concentrationc cells E0cell=E0cathode−E0anode E0cell=0
Putting the value in Nernst equation at 298K : Ecell=0−0.0591nlogC1C2
For a spontaneous reaction to take place, Ecell>0 −0.0591nlogC1C2>0
For C2>C1
the above equation is valid.
So, (b) and (d) are correct