Question

In the reaction, \[PbO{\text{ }} + {\text{ }}C{\text{ }} \to {\text{ }}Pb{\text{ }} + {\text{ }}CO:\]
(A) \[PbO\] is reduced
(B) C acts as an oxidizing agent
(C) C acts as a reducing agent
(D) This reaction does not represent redox reaction

Answer 1

Hint: Those chemical reactions in which change of oxidation states of atoms of both reactants and products take place are known as redox reactions. The term redox is formed by the combination of reduction-oxidation.

Complete step-by-step solution:
In simple terms, oxidation means gain of oxygen and reduction means loss of oxygen. In case of electron transfer, oxidation is loss of electrons and reduction is gain of electrons. There exists an interlinking between oxidation and reduction reaction and we name it as redox reactions.
In redox reactions, those species that accept electrons and undergo reduction are called an oxidizing agent and the species that donate electrons and undergo oxidation are called reducing agents. An oxidizing agent oxidizes the other reactant and itself get reduced and vice versa in case of reduction.
In the given reaction, \[PbO{\text{ }} + {\text{ }}C{\text{ }} \to {\text{ }}Pb{\text{ }} + {\text{ }}CO\]
 We see that carbon is donating its electrons and undergoing oxidation by forming CO, therefore carbon acts as a reducing agent.
In a similar way, \[{\text{PbO}}\] acts as an oxidizing agent as it accepts electrons and undergoes reduction to become a neutral atom.
Since the reaction involves both oxidation and reduction, it assures that the given reaction is a redox reaction. Thus, option (d) is wrong.

Hence, the correct answer is (C).

Note: The alternative way is to observe the change in oxidation states of reactants and product. Oxidation state of \[{\text{Pb}}\] changes from +2 to 0 and C changes from 0 to +2. This is known as displacement redox reaction.