Question

$\underset{\mathrm{lead}\mathrm{oxide}}{2\mathrm{PbO}\left(\mathrm{s}\right)}+\underset{\mathrm{Carbon}}{\mathrm{C}\left(\mathrm{s}\right)}\to \underset{\mathrm{Lead}}{2\mathrm{Pb}\left(\mathrm{s}\right)}+\underset{\mathrm{Carbon}\mathrm{dioxide}}{{\mathrm{CO}}_2\left(\mathrm{g}\right)}$

Name the oxidized substance, reduced substance, reducing agent, and oxidizing agent in this reaction.

Answer 1

$\underset{\mathrm{lead}\mathrm{oxide}}{2\mathrm{PbO}\left(\mathrm{s}\right)}+\underset{\mathrm{Carbon}}{\mathrm{C}\left(\mathrm{s}\right)}\to \underset{\mathrm{Lead}}{2\mathrm{Pb}\left(\mathrm{s}\right)}+\underset{\mathrm{Carbon}\mathrm{dioxide}}{{\mathrm{CO}}_2\left(\mathrm{g}\right)}$

Oxidized substance=Carbon$\left(\mathrm{C}\right)$[Increase in oxidation number of carbon]

$\mathrm{C}\mathrm{is}\mathrm{oxidised}\mathrm{from}0\mathrm{to}+4$

Reduced substance= Lead oxide$\left(\mathrm{PbO}\right)$[Decrease in oxidation number of lead]

$\mathrm{Pb}\mathrm{is}\mathrm{reduced}\mathrm{from}+2\mathrm{to}0$

Reducing agent=Carbon$\left(\mathrm{C}\right)$

Oxidizing agent=Lead oxide$\left(\mathrm{PbO}\right)$