Question

What is the balanced equation for the preparation of iron (III) chloride?
(A) $ Fe\left( {heated} \right) + 3C{l_2}\left( {dry} \right) \to 2FeC{l_3} $
(B) $ 2Fe\left( {heated} \right) + C{l_2}\left( {dry} \right) \to FeC{l_3} $
(C) $ 2Fe\left( {heated} \right) + 3C{l_2}\left( {dry} \right) \to 2FeC{l_3} $
(D) $ Fe\left( {heated} \right) + 3C{l_2}\left( {dry} \right) \to FeC{l_3} $

Answer 1

Hint: Iron is a metal that can undergo loss of electrons which is termed as oxidation. Chlorine is a chemical element that belongs to halogens and has non-metallic character. By treating iron metal with chlorine, a salt iron (III) chloride can be formed. Iron should be heated, and chlorine gas must be dried before chemical reaction.

Complete answer:
Chemical elements in the periodic table were classified into metals and non-metals. Metals can easily undergo loss of electrons. non-metals are the chemical elements that try to gain electrons by attaining the nearest noble gas configuration.
Metals and non-metals react with each other and form an ionic compound known as salts.
Iron is a metal that can easily undergo oxidation, chlorine is a non-metal that belongs to halogens and has more electronegativity value.
Iron and chlorine react with each other and form a compound known as iron (III) chloride with the molecular formula of $ FeC{l_3} $ .
Iron (III) chloride can be prepared by mixing heated iron metal with dry chlorine gas. The balanced chemical equation can be represented as:
 $ 2Fe\left( {heated} \right) + 3C{l_2}\left( {dry} \right) \to 2FeC{l_3} $
In the above equation, there were the same number of atoms on both sides of the reactants and products.
Option C is the correct one.

Note:
In the balanced chemical equation, all the atoms on both sides of the chemical reaction must be equal. Thus, the number of atoms must be calculated. While preparing iron (III) chloride, the heating should stop when the reaction starts as the reaction is an exothermic process.