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Hydrochloric acid reacts with aluminum sulfite in the following way: 6 HCl (aq) +Al2(SO3)3 (s) -> 3 SO2 (g) + 3 H2O (l) + 6 AlCl3 (aq) the reaction is done at 22.7 degrees C and 0.954 atm, to produce 28.2 mL of sulfur dioxide gas. How many grams of aluminum sulfite was used in this reaction? I was able to work out that moles of SO2 are 0.0011076 using the PV=nRT formula; I am just not how to proceed.