Question

Which of the statements about the reaction below are incorrect?
$\text{ 2PbO(s) + C(s) → 2Pb(s) + C}O_2\text{(g)}$
(a) Lead is getting reduced.
(b) Carbon dioxide is getting oxidized.
(c) Carbon is getting oxidized.
(d) Lead oxide is getting reduced.

• A. (a) and (b)
• B. (a) and (c)
• C. (a), (b) and (c)
• D. all

Answer 1

Answer: (A)

(a) and (b)

Answer 2

Oxidation and reduction reactions involve the transfer of electrons between two substances.
In oxidation, a substance either gains or loses electrons, typically involving oxygen.
Conversely, reduction entails the gain or loss of electrons, often in relation to oxygen.

Lead (II) oxide (PbO) undergoes a reaction with carbon (C) to produce lead (Pb)and carbon dioxide (CO2).
The chemical reaction can be represented as follows:
$\text{ 2PbO(s) + C(s) → 2Pb(s) + C}O_2\text{(g)}$

Electrons are gained by lead.
The reaction is as follows:
Pb2+ + 2e-$→$ Pb
Reduction occurs in lead oxide.
Electrons are lost by carbon.
C $→$ C2+ + 2e-
Carbon dioxide is oxidized.

The rationale for the incorrect choices is as follows:
In this scenario, lead oxide undergoes reduction, and carbon dioxide undergoes oxidation.
Therefore, options (B), (C), and (D) are deemed incorrect.

Therefore, the correct option is (A) (a) and (b).