Chemistry Electrochemistry SET 2019
PMDC Verified Question 51 of 73
Rusting of iron metal Fe occurs when Fe gets converted into Fe2O3. What happened with Fe?
A
Fe is neutralized
B
Fe is sublimed
C
Fe is reduced
D
Fe is oxidized
Tap any option to test your recall and reveal the step-by-step Propolis autopsy.

Propolis Cognitive Error Autopsy

Official Correct Choice:
Option D: Fe is oxidized
Concept:

Corrosion (rusting) is fundamentally a spontaneous electrochemical redox process where a refined metal reverts to a more stable oxide form.

Solution:

  • In its elemental state, iron (\( Fe \)) has an oxidation number of \( 0 \).


  • In rust (iron(III) oxide, \( Fe_2O_3 \)), the oxidation state of iron is \( +3 \).


  • Because the oxidation state increases from \( 0 \) to \( +3 \), Iron has lost electrons.


  • The loss of electrons is strictly defined as oxidation.


Why other options are incorrect:

Reduction would mean gaining electrons (which happens to ambient Oxygen in this reaction, not Iron). Neutralization is an acid-base reaction. Sublimation is a physical phase change from solid to gas.

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