Question

Write balanced equations for the following reactions:
(a) reduction of copper oxide by hydrogen.
(b) reduction of iron (III) oxide by carbon monoxide.
(c) reduction of lead (II) oxide by carbon.

Answer 1

(a) On heating copper oxide in the presence of hydrogen gas, it gets reduced to copper metal and water.​
$$\begin{gathered} \mathrm{CuO}+{\mathrm{H}}_2\stackrel{\mathrm{Heat}}{\to }\mathrm{Cu}+{\mathrm{H}}_2\mathrm{O} \\ \mathrm{Copper}\mathrm{oxide}\mathrm{Hydrogen}\mathrm{gas}\mathrm{Copper}\mathrm{Water} \end{gathered}$$

(b) On heating iron (III) oxide in the presence of a reducing agent such as carbon monoxide, it reduces to iron and carbon dioxide gas is liberated in the process.​
$$\begin{gathered} {\mathrm{Fe}}_2{\mathrm{O}}_3+3\mathrm{CO}\stackrel{\mathrm{Heat}}{\to }2\mathrm{Fe}+3{\mathrm{CO}}_2 \\ \mathrm{Iron}\left(\mathrm{III}\right)\mathrm{oxide}\mathrm{Carbon}\mathrm{monoxide}\mathrm{Iron}\mathrm{Carbon}\mathrm{dioxide} \end{gathered}$$

(c) On heating lead (II) oxide with carbon as a reducing agent​, it gets reduced to lead and carbon monoxide gas is liberated in the process.​
$$\begin{gathered} \mathrm{PbO}+\mathrm{C}\stackrel{\mathrm{Heat}}{\to }\mathrm{Pb}+\mathrm{CO} \\ \mathrm{Lead}\left(\mathrm{II}\right)\mathrm{oxide}\mathrm{Carbon}\mathrm{Lead}\mathrm{Carbon}\mathrm{monoxide} \end{gathered}$$