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

Options

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.

Answer

c

Explanation

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