Question

Which of the statements about the reaction below are incorrect?

$2\mathrm{PbO}\left(\mathrm{s}\right)+\mathrm{C}\left(\mathrm{s}\right)\to 2\mathrm{Pb}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

(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

(a) and (b)

The explanation for the correct option

(A) (a) and (b)

Oxidation and reduction reaction

• An oxidation-reduction reaction is a chemical process in which electrons are transferred between two reactants.
• The oxidation reaction is a process in which oxygen is gained or lost electrons.
• The reduction reaction is one in which oxygen is lost or gain of electrons.

Lead(II) oxide reacts with carbon

• Lead(II) oxide $\left(\mathrm{PbO}\right)$ reacts with carbon $\left(\mathrm{C}\right)$ to form lead $\left(\mathrm{Pb}\right)$ and carbon dioxide $\left({\mathrm{CO}}_2\right)$.
• The reaction is as follows:

$2\mathrm{PbO}\left(\mathrm{s}\right)+\mathrm{C}\left(\mathrm{s}\right)\to 2\mathrm{Pb}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

• Lead gains electrons.
• The reaction is as follows:

${\mathrm{Pb}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Pb}$

• Lead oxide is reduced.
• Carbon loses electrons.
• The reaction is as follows:

$\mathrm{C}\to {\mathrm{C}}^{2+}+2{\mathrm{e}}^{–}$

• Carbon dioxide is oxidized.

The explanation for incorrect options

• Here, lead oxide is reduced, and carbon dioxide is oxidized.
• Hence, all other options (B), (C) and (D) are incorrect.

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