Consider the daniell cell where the cell reaction and

Question

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