What is the empirical formula for Chrysene?

NetherCraft 0

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?

1 Answer

  • 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 C

    1.8 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 H

    So if we divide both by .2 we get this ratio:

    1 mol H : 1.5 mol C

    which equals:

    2 mol H : 3 mol C

    Thus the empirical formula is

    C3H2

Also Check This  What is this from? “Do not meddle in the affairs of dragons, for you are crunchy and taste good with ketchup”

Leave a Reply

Your email address will not be published.