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

The Correct Option is A

Oxidation and reduction reactions are defined by electron transfer. Oxidation involves the loss or gain of electrons, often with oxygen. Reduction also involves electron gain or loss, frequently related to oxygen.

Consider the reaction between lead (II) oxide (PbO) and carbon (C), yielding lead (Pb) and carbon dioxide (CO₂). The balanced chemical equation is:
\(\text{ 2PbO(s) + C(s) → 2Pb(s) + C}O_2\text{(g)}\)

Lead gains electrons, indicating reduction:
Pb²⁺ + 2e^-\(→\) Pb
Reduction occurs in lead oxide.
Carbon loses electrons, indicating oxidation:
C \(→\) C²⁺ + 2e^-
Carbon dioxide is the oxidized product.

The incorrect choices are based on misidentification of oxidation and reduction. In this reaction, lead oxide is reduced, and carbon is oxidized to carbon dioxide. Thus, options (B), (C), and (D) are incorrect.

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