of mater and assume the unknown compound is a liquid. /4 (d) How many grams of nitrogen dioxide would be produced in the reaction above? /6 (d) Suppose an insufficient amount of oxygen is used for the combustion analysis and some of the carbon is converted into carbon monoxide instead of carbon dioxide. If an empirical formula is determined using only the mass of collected carbon dioxide to determine the amount of oxygen, will the empirical formula determined from the results be too high or too low in carbon? Assume other product yields are unchanged. Explain. /2
CHEM111Practice E1Spring 20151)11) (20 points) You take 1.00 g of aspirin (CxHyOz) and burn it to collect 2.2 g carbondioxide (44.01 g mol-‐1) and 0.400 g water (18.015 g mol-‐1). You know that the molarmass of aspirin is between 170 and 190 g mol-‐1.(a)What is the empirical formula of aspirin?(b)What is the molecular formula of aspirin?(c)Reacting 1 mole of compound SA and 1 mole of acetic anhydride (C2H6O3) gives you1 mole of aspirin and 1 mole of acetic acid (C2H4O2). What is the molecular formulaof SA?
CHEM111Practice E1Spring 2015GradingQuestionsScoreOut of1 to 7/148/189/2010/2411/24Total/100