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Consider the Daniell cell where the cell reaction and standard potential are:

Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) E° = 1.10 V

If the cell is initially at standard conditions ([Cu2+] = [Zn2+] = 1.00 M), what are the concentrations of Cu2+ and Zn2+ when the cell potential has fallen to 1.06 V?

(If needed, refer to Table 17-1.)

  • [Cu2+]= 0.90 M; [Zn2+]=1.10 M
  • [Cu2+]= 0.94 M; [Zn2+]= 1.06 M
  • [Cu2+]= 0.50 M; [Zn2+]=1.50 M
  • [Cu2+]= 8.5 x 10-2 M; [Zn2+]=1.91 M
  • [Cu2+]= 1.91 M; [Zn2+]=8.5 x 10-2 M

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