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What is the empirical formula for Chrysene?

Combustion analysis of chrysene, a polycyclic aromatic hydrocarbon used in the manufacture of some dyes , produced 13.20 {g} CO2 and 1.80 g H2O.I don’t know if I need to find the mass of Oxygen or not…and I keep getting it wrong 🙁 Can someone help me?
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Mina Herzog

Feb 20, 2025

Well it states that it is a hydrocarbon so there are no oxygen atoms in the molecule. So first off lets find grams of CO2 and H2O:13.2 g CO2 * 1 mol CO2 / (12.01 + 16*2) g CO2 = .3 mol CO2 * 12.01 g C / 1 mol CO2 = 3.6 g C1.8 g H2O * 1 mol H2O / (1.008*2 + 16) = .0999 g H2O * 1.008 * 2 g H / 1 mol H2O = .2 g H Then find moles of both:3.6 / 12.01 = .3 mol C.2 / 1.008 = .2 mol HSo if we divide both by .2 we get this ratio:1 mol H : 1.5 mol Cwhich equals:2 mol H : 3 mol CThus the empirical formula is C3H2... Show More
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