Question

In the following reaction, identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent.
\[4HCl+Mn{{O}_{2}}\to MnC{{l}_{2}}+2{{H}_{2}}O+C{{l}_{2}}\]

Answer 1

Hint: This reaction is an example of redox reaction. To solve this question, look at the oxidation states of individual elements in the given reaction. Now, compare the oxidation states in reactant and product side to identify oxidizing and reducing agents.

Complete step by step answer:
In the given reaction –
\[4HCl+Mn{{O}_{2}}\to MnC{{l}_{2}}+2{{H}_{2}}O+C{{l}_{2}}\]
Let us take a look at the given reaction and observe the oxidation state of individual atoms.
In HCl, the oxidation state of hydrogen is +1 and that of Chlorine is -1.
In \[Mn{{O}_{2}}\], the oxidation state of manganese is +4 and the oxidation state of oxygen is -2.
In \[MnC{{l}_{2}}\], the oxidation state of manganese is +2 and the oxidation state of chlorine is -1.
In \[{{H}_{2}}O\], the oxidation state of hydrogen is +1 and the oxidation state of oxygen is -2.
In \[C{{l}_{2}}\], the oxidation state of chlorine is zero.
As we can see,
Oxidation state of chlorine increases from -1 to 0.
Chlorine is therefore oxidized.
HCl is a reducing agent.
Oxidation state of Manganese reduces from +4 to +2.
Manganese is therefore reduced.
Manganese dioxide is an oxidizing agent.

Therefore, the answer is –
species oxidized – Hydrochloric acid (HCl)
species reduced – Manganese dioxide (\[Mn{{O}_{2}}\])
oxidizing agent – Manganese dioxide (\[Mn{{O}_{2}}\])
reducing agent – Hydrochloric acid (HCl)

Additional Information: A reaction where oxidation and reduction take place simultaneously is known as a redox reaction.

Note: “Oxidizing agent is defined as the species which itself gets reduced and helps the other substance to get oxidized”. It itself undergoes reduction. “Reducing agent is defined as the species which itself gets oxidized and helps the other substance to get reduced”. It itself undergoes oxidation.