# Why is cell potential defined as E0[Reduction]-E0[Oxidation] and not the reverse?

Why is the cell potential defined as:

$$E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}$$

or $$E^\circ_{cell} = E^\circ_{reduction} - E^\circ_{oxidation}$$

as opposed to $$E^\circ_{cell} = E^\circ_{anode} - E^\circ_{cathode}$$

or $$E^\circ_{cell} = E^\circ_{oxidation} - E^\circ_{reduction}$$

A few definitions which relate to the problem:

Cell potential is the measure of the potential difference between two half cells in an electrochemical cell

The potential difference is caused by the ability of electrons to flow from one half cell to the other

The difference between the potential for the reducing agent to become oxidized and the oxidizing agent to become reduced will determine the cell potential. (Chem.Libretexts)

But why is this the case?

Also, why does it then say here that $E^\circ_{cell} = E^\circ_{reduction} + E^\circ_{oxidation}$ rather than $E^\circ_{cell} = E^\circ_{reduction} - E^\circ_{oxidation}$