Whys is the standard electrode potential (-) for electrolytic cells but positive for (+) galvanic cells.
- If E°cell > 0, then the process is spontaneous (galvanic cell)
- If E°cell < 0, then the process is non-spontaneous (electrolytic cell)
Thus in order to have a spontaneous reaction, E°cell must be positive, where:
E°cell = E°cathode − E°anode
^ above taken form wiki.
Also can someone please explain the follow:
In both cells is the electron flow from
anode -> cathode ??
For electrolytic cells isn't the electron flow from the battery (-) anode to cathode (-) of the cell.
Do we then show this by electron flow as cathode (-) ------> anode (+) [in the actual cell itself]??