Question

$2PbO + C\xrightarrow{{}}2Pb + C{O_2}$ is an example of
A.Oxidation reaction
B.Reduction reaction
C.Redox reaction
D.None

Answer 1

Hint: We can define redox reactions as chemical reactions in which transfer of electrons takes place between two reactants. We can identify the transfer of electrons by observing the change in oxidation states of the species that are reacting. Batteries (or) electrochemical cells are the examples of redox reactions.

Complete step by step answer:
The given chemical equation is,
$2PbO + C\xrightarrow{{}}2Pb + C{O_2}$
From the given chemical equation, we can see that lead oxide reacts with carbon to form metallic lead with the evolution of carbon dioxide.
We can define oxidation reactions as loss of electrons from a substance.
Similarly, reduction reactions are defined as gain of electrons.
In order to identify the type of reaction, let us see the oxidation state of the elements in reactants and products.
For lead, the oxidation state of lead in $PbO$ is $ + 2$ and the oxidation state of $Pb$ is zero. (Element in its free state will have zero as its oxidation number).
For carbon, the oxidation state of carbon in reactant side is $0$ and the oxidation state of carbon in $C{O_2}$ is ${\text{ + 4}}{\text{.}}$
We can observe that carbon has lost electrons, so it is oxidized and lead has gained electrons, and is reduced.
The oxidation reaction is written as,
${C^0}\xrightarrow{{}}{C^{4 + }}$
The reduction reaction is written as,
$P{b^{2 + }}\xrightarrow{{}}Pb$
We can see that both oxidation and reduction reactions have occurred, therefore the given reaction is a redox reaction.
Hence option (C) is correct.

Note:
We must know that respiration, photosynthesis, combustion, rusting are some examples of redox reactions. Oxidizing agents are that species (molecule/ion) that accepts electrons and reducing agents are species (molecule/ion) that donates electrons. A substance that is oxidized acts as a reducing agent and substance that is reduced acts as oxidizing agent.