The volume of chlorine required for the complete reaction of 10 litres of ${\mathrm{H}}_2 \mathrm{S}$ at STP is lit.

$[{\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{S}\to 2\mathrm{HCl}+\mathrm{S}]$

• Chlorine reacts with hydrogen sulfide to form hydrochloric acid and sulphur. The balanced chemical equation is,

                     ${\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{S}\to 2\mathrm{HCl}+\mathrm{S}$

Here, 1 volume of chlorine reacts with 1 volume of ${\mathrm{H}}_2 \mathrm{S}$.

So, $10 \mathrm{L}$ of ${\mathrm{H}}_2 \mathrm{S}$ requires $10 \mathrm{L}$ of chlorine for the completion of oxidation in the reaction.