# What volume of oxygen is needed to react with solid sulfur to form 6.20 L of sulfur dioxide?

$S \left(s\right) + {O}_{2} \left(g\right) \rightarrow S {O}_{2} \left(g\right)$
Given that the reaction proceeds quantitatively, whatever the conditions of temperature and pressure, if there were $6.20 \cdot L$ of $S {O}_{2} \left(g\right)$, there were $6.20 \cdot L$ $\text{dioxygen}$ required to make it. Stoichiometry demands this.
How much oxygen is required to form $6.20 \cdot L$ of $S {O}_{3} \left(g\right)$ from elemental sulfur?