Question

Can you balance this chemical equation?
\[Mn{O_2} + Al \to Mn + A{l_2}{O_3}\]

Answer 1

Hint: We have to remember that redox reactions are oxidation-reduction chemical reactions in which the reactants undergo a change in their oxidation states. The term ‘redox’ is a short form of reduction-oxidation. All the redox reactions can be broken down into two different processes – a reduction process and an oxidation process.

Complete answer:
As we know that the oxidation and reduction reactions always occur simultaneously in the redox reaction or Oxidation-Reduction reaction. The substance getting reduced in a chemical reaction is known as the oxidizing agent, while a substance that is getting oxidized is known as the reducing agent.
Balanced chemical equation:
\[3Mn{O_2} + 4Al \to {\text{3}}Mn + 2A{l_2}{O_3}\]
Manganese oxide itself gets reduced to Manganese and thus reduction is taking place as oxygen is being removed. In the case of aluminum, aluminum gets oxidized as oxygen is added to it. Thus this type of reaction is a redox reaction.
The two species that exchange electrons in a redox reaction are given special names:
The ion or molecule that accepts electrons is called the oxidizing agent - by accepting electrons it oxidizes another species.
The ion or molecule that donates electrons is called the reducing agent - by giving electrons it reduces the other species.

Note:
As we know that most oxidation-reduction (redox) processes involve the transfer of oxygen atoms, hydrogen atoms, or electrons, with all three processes sharing two important characteristics: (1) they are coupled—i.e., in any oxidation reaction a reciprocal reduction occurs, and (2) they involve a characteristic net chemical change—i.e., an atom or electron goes from one unit of matter to another.