chemistry

posted by .

Is this correct?

A 0.1471 g sample of a compound containing C, H, and F was burned to produce 0.1960 g CO2 and 0.08024 g H2O. If the molar mass of the compound was determined to be approximately 66.05 g/mol, what is its molecular formula?

My answer is: C_12 H O_20

  • chemistry -

    You probably made the same mistake I did the first time through this problem; that's F and not O.
    I obtained CH2F for the empirical formula and C2H4F2 for the molecular formula.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    a 2.500g sample of an unknown compound containing only C, H and O was burned in O2. The products were 4.776g of CO2 and 2.934g of H2O. a) what is the percent compostion of the original compound?
  2. Chemistry

    a compound was analyzed and found to contain C,H,N,O, and Cl. When o.150g sample of this compound was burned, it produced 0.138 g of CO2 and 0.0566 g of H2O. All of the Nitrogen in another sample of mass 0.200 g was converted to 0.0238 …
  3. Chemistry

    A 0.5595 g sample of a compound containing C, H, and O was burned to produce 1.429 g CO2 and 0.5850 g H2O. If the molar mass of the compound was determined to be approximately 86.13 g/mol, what is its molecular formula?
  4. chemistry

    A 0.6996 g sample of a compound containing C, H, and F was burned to produce 0.6039 g CO2 and 0.1235 g H2O. If the molar mass of the compound was determined to be approximately 102.0 g/mol, what is its molecular formula?
  5. chemistry

    I need help with this problem... A 1.208 g sample of a compound containing C, H, and O was burned to produce 2.561 g CO2 and 0.3930 g H2O. Calculate the empirical formula of the compound. I always get stuck when it comes to finding …
  6. Chemistry

    Is this correct? A 0.7473 g sample of a compound containing C, H, and O was burned to produce 1.909 g CO2 and 0.7813 g H2O. Calculate the empirical formula of the compound. I got C5 H10 O1. I'm not sure if that's correct..
  7. Chemistry

    A 0.5595 g sample of a compound containing C, H, and O was burned to produce 1.429 g CO2 and 0.5850 g H2O. If the molar mass of the compound was determined to be approximately 86.13 g/mol, what is its molecular formula?
  8. chemistry

    I got C_4 H_3 O_8 for this question but I'd like someone to check my answer, please. A 1.012 g sample of a compound containing C, H, and O was burned to produce 2.145 g CO2 and 0.3293 g H2O. Calculate the empirical formula of the compound
  9. Chemistry

    A 0.7381 g sample of a compound containing C, H, and F was burned to produce 0.6368 g CO2 and 0.1303 g H2O. Calculate the empirical formula of the compound. Do I have to take in account the O atoms?
  10. Chemistry

    A 2.20 g-sample of a compound containing carbon, hydrogen, and oxygen is burned and it produces 4.61 g CO2 and 0.94 g H2O. What is the empirical formula of this compound?

More Similar Questions