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For the cell Zn(s)|Zn^(2+)||Cu^(2+)|Cu(...

For the cell `Zn(s)|Zn^(2+)||Cu^(2+)|Cu(s)`, the standard cell voltage, `E^(c-)._(cell)` is `1.10V`. When a cell using these reagents was prepared in the lab, the measured cell voltage was `0.98V`. One possible explanatino for the observed voltage is

A

There were `2.00 mol ` of `Zn^(2+)` but only `1.00 mol ` of `Cu^(2+)`

B

The `Zn` electrode had twice the surface of the `Cu` electrode.

C

The `[Zn^(2+)]` was larger than the `[Cu^(2+)]`.

D

The volume of the `Zn^(2+)` solution was larger than the volume of the `Cu^(2+)` solution.

Text Solution

Verified by Experts

The correct Answer is:
c
`E_(cell)=E^(c-)._(cell)-(0.0591)/(2) log .([Zn^(2+)])/([Cu^(2+)])`
`E_(cell)ltE^(c-)._(cell)implies[Zn^(2+)]gt[Cu^(2+)]`
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