An environmental engineer analyzes a sample of air contaminated with sulfur
dioxide. To a 500.-mL sample at 700 . torr and \(38^{\circ} \mathrm{C},\) she
adds \(20.00 \mathrm{~mL}\) of \(0.01017 M\) aqueous iodine, which reacts as
follows:
\(\mathrm{SO}_{2}(g)+\mathrm{I}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)
\longrightarrow\)
$$\mathrm{HSO}_{4}^{-}(a q)+\mathrm{I}^{-}(a q)+\mathrm{H}^{+}(a q)
\quad[\text { unbalanced }]$$
Excess \(\mathrm{I}_{2}\) reacts with \(11.37 \mathrm{~mL}\) of \(0.0105
\mathrm{M}\) sodium thiosulfate:
\(\mathrm{I}_{2}(a q)+\mathrm{S}_{2} \mathrm{O}_{3}^{2-}(a q) \longrightarrow
\mathrm{I}^{-}(a q)+\mathrm{S}_{4} \mathrm{O}_{6}^{2-}(a q) \quad[\) unbalanced
\(]\)
What is the volume \(\%\) of \(\mathrm{SO}_{2}\) in the air sample?