Hydrogen sulfide reacts with sulfur dioxide to form sulfur as one of the products. The two relevant redox equations are given below. $\mathrm{H_2S}(aq) \rightleftharpoons \mathrm{S}(s) + 2\mathrm{H}^{+}(aq) + 2e^{-}$ $\mathrm{SO_2}(aq) + 4\mathrm{H}^{+}(aq) + 4e^{-} \rightleftharpoons \mathrm{S}(s) + 2\mathrm{H_2O}(l)$ How many moles of hydrogen sulfide are required to react with sulfur dioxide and produce 1 mol of sulfur?
- A$\frac{1}{3}\text{ mol}$
- B$\frac{2}{3}\text{ mol}$
- C$\frac{3}{2}\text{ mol}$
- D$2\text{ mol}$