Question

the Cu(No3)2 solution was diluted to 0.001 M. The voltage was measured against standard zinc electrode and found to be 0.89 volts..

1. write the cell reaction.
2. write the line notation for the reaction.
3. Use the nernst equation to calculate what the expected voltage should be, and compare to the measured voltage.

Answer 1

Zn + Cu^2+ ==> Cu + Zn^2+

2. I assume when you say standard Zn electrode you mean (Zn^2+) = 1 M.
Zn|Zn^2+(1M)||Cu^2+(0.001M)|Cu

3.
Ecell = Eocell - (0.05916/n)*log Q
n = 2 for the transfer of 2 electrons.
Q = (Zn^2+)(Cu)/(Cu^2+)(Zn)
Fo that (Zn^2+) = 1M; (Cu)=(Zn) = 1; (Cu^2+) = 0.001.

Answer 2

whats the answer for the nernst equation?

Answer 3

what was the value for this nernst equation?

Another question: How did the change in concentration of the copper ions affect the cell potential? Is this change in agreement (qualitatively) with that which would be predicted by LeChatelier's Principle? explain.