Question

Relationship between thermodynamic quantities and electrochemistry.
A follow up from @C9H8O4 's question:
(http://openstudy.com/study#/updates/51f52acde4b0c8f6bc368792 )

Answer 1

A spontaneous redox reaction is characterized by a negative value of ΔG°, which corresponds to a positive value of E°cell.

Answer 2

http://2012books.lardbucket.org/books/general-chemistry-principles-patterns-and-applications-v1.0m/section_23_04.html
this book really help u guys

Answer 3

When the electrodes (half-cells) are connected by a cable, a current flows.
Electrons can carry out electrical work in their path from one electrode to the other:
\[\LARGE w _{e}=q*E _{cell}\]
The charge are corresponding to q is shifted from one electrode to the other.
Let us look upon a reaction where v electrons transferred an infinitesimal change in the degree of the reaction ζ [mol^(-1)]:
\[\LARGE q=-veN _{A} d \zeta = -vFd \zeta\]
The electrical work is thus:
\[\LARGE dw _{e}=-vFE _{cell} d \zeta\]
However, the maximum electric work operating at constant T and p is:
\[\LARGE dw _{e}=dG _{T,p}=\Delta _{r}Gd \zeta\]
We therefor get:
\[\LARGE \Delta _{r}G=-vFE _{cell}\]
The very equation you used.

Answer 4

electrochem cells convert chemical energy to electrical energy and vice versa. total amount of energy produced by an electrochemical cell, and thus the amount of energy available to do electrical work, depends on both the cell potential and the total number of electrons that are transferred from the reductant to the oxidant during the course of a reaction