Answer:
3.22 * 10^-4 M
Step-by-step explanation:
The cell reaction equation is;
2Al(s) + 3Cu^2+(aq) ------> 2Al^3+(aq) + 3Cu(s)
E° = 0.337 V - (-1.66 V)
E° = 1.997 V
Given that the cell potential is 2.067 V, from Nernst's equation;
E = E° - 0.0592/n log Q
Substituting values;
2.067 = 1.997 - 0.0592/6 log [Al^3+]^2/[1.07]^3
0.07 = - 0.0592/6 log [Al^3+]^2/[1.07]^3
- 7.07 = log [Al^3+]^2/[1.07]^3
Antilog (- 7.07) = [Al^3+]^2/[1.07] ^3
8.5 * 10^-8 = [Al^3+]^2/[1.07]^3
[Al^3+]^2 = 8.5 * 10^8 * 1.07 ^3
[Al^3+]^2 = 1.04 * 10^-7
[Al^3+] = √1.04 * 10^-7
[Al^3+] = 3.22 * 10^-4 M