Question

Why is iron not extracted by electrolysis?

Answer 1

Hint: The chemical element iron has the atomic number 26 and the symbol Fe. It is a metal that is found in group 8 of the periodic table and the first transition series. It makes up a large portion of both the outer and inner core of the planet and is, by mass, the second most prevalent element after oxygen. Chemically, iron's two most frequent oxidation states are iron(II) and iron(III) (III).

Complete Step by Step Solution:
An ordinarily non-spontaneous chemical reaction can be accelerated using the electrolysis approach in chemistry and manufacturing. As a step in the electrolytic cell-based separation of elements from naturally existing sources like ores, electrolysis is significant from a commercial standpoint. The decomposition potential is the voltage required for electrolysis to take place.

In other words, electrolysis would be referred to as "breakdown using electricity" because the word "lysis" implies to separate or break. Choosing the right reducing agent is crucial to successfully extracting a metal from its ore. Iron is a moderately active metal, therefore carbon, rather than electrolysis, can be used to decrease its oxides.

According to energy considerations, iron can be easily reduced utilising coke (CO in particular), as it not only lowers iron but also supplies the process with the necessary quantity of heat energy. Further carbon is an element that is more active than iron but less active than Na, Mg, Ca, or Al.

Iron is a moderately active element, and carbon can be used to decrease its oxides as opposed to electrolysis. Based on energy considerations, coke not only makes it simple to reduce iron, but it also supplies all of the necessary heat energy.

Note: The exchange of atoms and ions by the removal or addition of electrons caused by the applied current is the primary electrolysis process. The required electrolysis products can frequently be physically separated from the electrolyte and are in a distinct state (e.g. by collecting gas above an electrode or precipitating a product out of the electrolyte). When two or more electrolytic cells are linked in series to the same power source, the products created in the cells are proportional to their equivalent weight. The quantity of the products is proportional to the current. Faraday's laws of electrolysis are these.