Question

$2{\mathrm{H}}_2\mathrm{S}+{\mathrm{SO}}_2\to 2{\mathrm{H}}_2\mathrm{O}+3\mathrm{S}$

In the following reaction, what is the magnitude of difference in the oxidation state of sulfur in ${\mathrm{H}}_2\mathrm{S}$ and in ${\mathrm{SO}}_2$?

• A. 0,+2
• B. -4,0
• C. -2,+2
• D. +2,-4

Answer 1

The correct option is D

+2,-4

The oxidation number of sulfur$\left(\mathrm{S}\right)$ in Dihydrogen sulfide$\left({\mathrm{H}}_2\mathrm{S}\right)$

$$\begin{gathered} {\mathrm{H}}_2\mathrm{S}\to \mathrm{S} \\ 0-(-2) \\ =+2 \end{gathered}$$

The oxidation number of sulfur$\left(\mathrm{S}\right)$ in Sulfur dioxide$\left({\mathrm{SO}}_2\right)$

$$\begin{gathered} {\mathrm{SO}}_2\to \mathrm{S} \\ 0-\left(4\right) \\ =-4 \end{gathered}$$

The oxidation number of sulfur$\left(\mathrm{S}\right)$ in the elemental state$\left(\mathrm{S}\right)$ will be $0$.

The difference in the oxidation state of $\mathrm{S}\mathrm{from}{\mathrm{H}}_2\mathrm{S}\mathrm{and}+4\mathrm{in}{\mathrm{SO}}_2\mathrm{to}0\mathrm{in}\mathrm{S}$.

Therefore option D is the correct option.