Complex electrolysis question
Posted: Wed Aug 02, 2023 8:12 pm
The question in regard to the attached image below is:
Explain why the carbon electrode cannot be replaced with an iron electrode.
The answer states that iron is a STRONGER REDUCING AGENT than fluorine and would be preferentially oxidised.
Iron’s standard potential for oxidation is +0.44 V. Fluorine’s standard potential for oxidation is -2.89 V.
This is my thought process: the stronger the reducing agent, the more likely the substance is to oxidise. The more likely a substance is to oxidise, the lower its standard electrode potential. So how is iron the stronger reducing agent if fluorine’s standard reduction potential is lower? Am I not meant to flip the signs when determining what reduces and oxidises even for species I know are oxidising?
Explain why the carbon electrode cannot be replaced with an iron electrode.
The answer states that iron is a STRONGER REDUCING AGENT than fluorine and would be preferentially oxidised.
Iron’s standard potential for oxidation is +0.44 V. Fluorine’s standard potential for oxidation is -2.89 V.
This is my thought process: the stronger the reducing agent, the more likely the substance is to oxidise. The more likely a substance is to oxidise, the lower its standard electrode potential. So how is iron the stronger reducing agent if fluorine’s standard reduction potential is lower? Am I not meant to flip the signs when determining what reduces and oxidises even for species I know are oxidising?