Current Supply/Electrolysis Driving unfavorable reaction

[anasofia]

In lecture 20, prof lavelle gave the example of magnesium metal and chloride gas being produced from molten magnesium chloride, and how it is an unfavorable reaction driven by an electrical current. He said that a current supply pulls the e- off of the anode side (the 2Cl- --> Cl(g) + 2e-) and forces them onto the cathode side. When he says forces what does he mean by that, because at that point, the current supply would be very negative due to all of the e- pulled off of the anode half reaction, and the cathode side is positive, so I am wondering if he misrepresented the process by saying forced, as the electrons should naturally flow to the positive solution.

[Abdallah Fares 3H]

When Professor Lavelle mentions that the electrical current "forces" electrons onto the cathode side, he is referring to the action of the external electrical power source. Yes electrons do naturally flow from the anode to the cathode due to the potential difference created by the redox reaction, the external power source applies an additional driving force to ensure that this flow of electrons occurs. Even though the cathode side may become more positive as electrons accumulate on it during the reduction half-reaction, the external power source continuously maintains the potential difference required for the reaction to proceed. I think that's what he meant by "force" in this context.