Standard Hydrogen Electrode.Watch
My text book says that in an electrochemical cell where the LH electrode is the Standard Hydrogen Electrode (SHE), the equation in this half cell is 2H+(aq) + 2e- <-> H2(g). However, I thought oxidation occurred at the negative electrode, i.e hydrogen gas which is bubbled in would form 2H+ and 2e-. S, basically I thought the main reaction would be the reverse of the one shown above. Can someone explain why my text book has it in that format?
The standard is an exception! When you write the conventional representation, it is always oxidised (on the left). It's just convention I guess.
But then how would the reaction occur if there is no oxidation at the negative electrode?