[GPhab]

Is the below interpretation correct?

Hydrogen electrode is a given a standard potential of 0 V. So to carry out the reaction

2H⁺ + 2e^-  H₂ successfully at standard conditions, suppose X Joules of energy is required. Obviously some Y joules of energy will be required if this were to happen several times and 1 coulomb of charge is used up(I know how to find Y in terms of X, but that is not the question). Li⁺ has a standard reduction potential of -3.03 V. Does it mean that to carry out

Li⁺  + e^- Li so that one coulomb of charge is used, Y+3.03 Joules of energy is required? If the above interpretation is true, then for very good oxidising agents, the required energy is Y-(its electrode potential's magnitude) Joules, which may turn out to be negative(I'm not sure about this). Supplying negative energy means what?

[Astrokel]

hey GPhab,

i don't really get what you mean, can you explain the point on Y+3.03? and a negative energy would probably mean work done by the system.

[GPhab]

The Y Joules/Coulomb means that I was defining the absolute potential of the half-cell(which we know is very difficult to measure). Li⁺(like the members of its group) will be more reluctant to accept the electron and hence will require more energy. That is why I said (Y+3.03)Joules will be required per Coulomb. What I was trying to do is link the potential ideas which we learnt in Physics and what these potentials mean.

Can anybody give me a link for the derivation of  :delta:G=-nFE (or maybe if it is short, do it here). I'm sorry to ask for this here but this derivation and the above interpretation MAY have something in common(both deal with work).

[Astrokel]

hey,

http://www.science.uwaterloo.ca/~cchieh/cact/applychem/gibbsenergy.html