A certain molecular liquid compound is found to be composed of carbon, hydrogenand oxygen. When 13.3 milligrams (mg) of the compound were strongly heated in an atmosphereof O2 (gas), 32.0 mg of CO2 (gas) and 6.53 mg of H2O (liq) were formed. Another sample of theliquid compound was vaporized and, from its vapor density, it's molar mass (GMM) wasestimated to be 1.1 x 102 g/mole.

(a) From these data, show that the empirical formula for the liquid compound is C3H3O.

(b) Show that the molecular formula for the liquid compound is C6H6O2.

(c) Write a balanced equation showing one mole of this liquid compound combusting inO2 (gas) to produce CO2 (gas) and H2O (liq).

(d) If 10.0 grams of the liquid compound were reacted with 21.0 grams of O2 (gas), whichwould be the limiting reagent (C6H6O2 or O2), how many grams of excess reagent shouldbe left un-reacted, how many moles of carbon dioxide should be produced, and howmany molecules of water should be produced? Given: NA = 6.02 x 1023.