Standard hydrogen electrode
A platinum electrode is inserted in a solution with a concentration of H+ of 1M, and hydrogen gas at 25℃ of 1 atm surrounding the platinum electrode is in equilibrium with H+. At this time, the electrode potential value represented by this half-cell is set to 0V, which is the standard for all standard electrode potentials.
Standard reduction potential
This is the other side's electrode potential having a standard hydrogen electrode.
If the standard reduction potential value is (+), it is easier to accept electrons than hydrogen ions, and if it is (-), it is more difficult to accept electrons than hydrogen ions.
electromotive force (=cell voltage)
The electromotive force (= cell voltage) of a battery can be easily obtained using the difference between the two electrode potentials.
The higher the standard reduction potential becomes (+), the lower one becomes (-).
The higher the standard reduction potential difference, the greater the electromotive force.
Even if the standard reduction potential is (-), if it has a larger value than the counterpart, it becomes a (+) pole.
Even if the standard reduction potential is (+), it becomes a (-) pole if it has a smaller value than the counterpart.