Sulfur dioxide gas $(SO2)$ reacts with excess oxygen gas $(O2)$ and excess liquid water $(H2O)$ to form liquid sulfuric acid $(H2SO4).$ In the laboratory, a chemist carries out this reaction with $67\mathrm{.}2L$ of sulfur dioxide and gets $250g$ of sulfuric acid.

Write a balanced equation for the reaction.

Calculate the theoretical yield of sulfuric acid.

Calculate the percent yield of the reaction.

$($One mole of any gas occupies $22\mathrm{.}4L$ under certain conditions of temperature and pressure. Assume those conditions for this question.$)$