Hydrogen sulfide is burned in an excess of oxygen, as represented by the equation below. $2\text{H}_2\text{S}(g) + 3\text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(g) + 2\text{SO}_2(g)$ $48\,\text{dm}^3$ of hydrogen sulfide is burned. What volume of sulfur dioxide will be produced at room temperature and pressure? [All volumes are measured at the same temperature and pressure.]
- A$24\,\text{dm}^3$
- B$36\,\text{dm}^3$
- C$48\,\text{dm}^3$
- D$96\,\text{dm}^3$