Homework Help: Chemistry/Electrochem

Posted by Andres on Monday, October 1, 2012 at 2:17pm.

Consider a cell at 255 K:
line notation
Pb-Pb2+(1.27M)--Fe3+(2.29M)-Fe
Given the standard reduction potentials calculate the cell potential after the reaction operated long enough for Fe3+ to have changed by 1.432M?

I know that Fe3+ is the cathode which will decrease in concentration and Pb2+ is the anode which increases in concentration. The overall electrons transferred is 6 and Q is (Pb2+)^3 over (Fe3+)^2. After calculating the potential i keep getting 0.08195V but the answer is 0.0794V, i don't know where im going wrong, can anyone help.

No one has answered this question yet.

Answer this Question

Related Questions

Chemistry - Consider a cell at 255 K: line notation Pb-Pb2+(1.27M)--Fe3+(2.29M)-...
Chemistry - Consider a cell at 255 K: line notation Pb-Pb2+(1.27M)--Fe3+(2.29M)-...
Chemistry - Consider a cell at 255 K: line notation Pb-Pb2+(1.27M)--Fe3+(2.29M)-...
Chemistry - Consider a cell at 255 K: line notation Pb-Pb2+(1.27M)--Fe3+(2.29M)-...
Chemistry - Consider a cell at 255 K: line notation Pb-Pb2+(1.27M)--Fe3+(2.29M)-...
Chemistry/Electrochem - Consider a cell at 299K: line notation Fe-Fe2+(1.39)--...
chemistry - Could I get some help with these please? Thanks Calculate the ...
Chemistry - A cell is set up with copper and lead electrodes in contact with ...
Chemistry - A cell is set up with copper and lead electrodes in contact with ...
Chemistry - 1) Assume that the reference half-cell is changed to a standard ...

For Further Reading

First Name:
School Subject:
Answer: