Dorothy walks past 26-100 and can hear the large 5.11 lecture inside. For some reason she picks up this week's problem set. She has a feeling it might be useful to her.

A hydrocarbon was found to contain the following elements: hydrogen, carbon, bromine, chlorine, nitrogen, oxygen, and sulfur. When 5.110 grams of the compound were combusted in excess oxygen, the products were analyzed. The analysis is summarized below.

There was 88.01 mg of water collected. The carbon dioxide was collected on solid calcium oxide, which forms calcium carbonate in the presence of carbon dioxide. The calcium oxide originally weighed 345.520 g, but weighed 346.810 g after exposure to the carbon dioxide. The nitrogen dioxide was collected at STP and occupied a volume of 766.49 mL. The two halides were collected as a mixture of silver bromide and silver chloride weighing 8.5216 g after treatment with silver nitrate. This mixture was then converted to silver chloride alone by treatment with excess hydrochloric acid. The resulting silver chloride weighed 7.0010 g. The sulfur dioxide was collected and bubbled through water to produce a solution of sulfurous acid. The solution of this acid was titrated with a solution of 0.1246 M sodium hydroxide until the acid was completely deprotonated. The endpoint required 235.22 mL of the sodium hydroxide. What is the empirical formula of the hydrocarbon?