Consider the Daniell Cell Where the Cell Reaction and Standard $\rarr$

Multiple Choice

Consider the Daniell cell where the cell reaction and standard potential are:Zn(s) + Cu²⁺ (aq) $\rarr$ Zn²⁺ (aq) + Cu (s) $\quad$ E° = 1.10 VIf 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, use the following equation: $\Delta$ G° = -nFE°, E° , E = E° - , moles e^- = (If needed, refer to Table 17-1in the text)

A) [Cu²⁺]= 8.5 x 10^-2 M; [Zn²⁺]=1.91 M
B) [Cu²⁺]= 0.94 M; [Zn²⁺]= 1.06 M
C) [Cu²⁺]= 1.91 M; [Zn²⁺]=8.5 x 10^-2 M
D) [Cu²⁺]= 0.50 M; [Zn²⁺]=1.50 M
E) [Cu²⁺]= 0.90 M; [Zn²⁺]=1.10 M