Question

write the reaction of oxidation of iron at cathode​

Answer 1

Corrosion is a REDOX reaction.

Explanation:

Corrosion is a galvanic method by which elements decay through oxidation usually but not forever to their oxides.

• For example, when shown to air, iron rots, silver smudges, and copper and brass obtain a bluish-green covering called a patina.

• Of the different elements subject to corrosion, iron is by far the numerous material commercially.

• An expected $100 billion per cycle is spent in the United States only to replace iron-containing things damaged by corrosion.

Consequently, the evolution of techniques for preserving metal coverings from corrosion creates a very dynamic area of manufacturing research.

• at cathode:

$O_{2(g)} + 4H^{+} _{aq} 4e^{-} -> 2H_{2}O\ E^{0} =1.23V$

• at anode:

$Fe(s)->Fe^{2+} (aq)+2e^{-}\ E^{0} =-0.45V$

• overall:

$2Fe(s)+O_{2(g)} +4H^{+}_{aq} ->2Fe^{2+}_{aq} +2H_{2} O_{l} \ E^{0} =1.68V$

To learn more:

write the reaction of oxidation of iron at cathode ​ - Brainly.in

https://brainly.in/question/16008769

write the reaction of oxidation of iron at cathode​ - Brainly.in

https://brainly.in/question/16038071

Answer 2

The reaction at the cathode:

O2(g) + 4H+ (aq) + 4e − → 2H2O(l)    E° = 1.23V

Explanation:

• The reaction of iron at cathode means the corrosion reaction.
• During the corrosion reaction, the iron metal is oxidized to Fe+2 ion at the anode while at cathode reduction takes place.
• The reaction at the cathode:
• O2(g) + 4H+ (aq) + 4e − → 2H2O(l)    E° = 1.23V
• In this reaction, the Oxygen combines with hydrogen ions and forms water which causes rusting on the surface of iron metal.