Chemistry

Calculate empirical formula

C=41.7%,H=6.2%,N=19.3%, and O=33.1%

Thanks. any help at all will be awesome!

  1. 👍 0
  2. 👎 0
  3. 👁 152
  1. Well, um...make sure you gave the percentages right. I added all the percentages together and I got 100.3%. Anyway, Imma still gunna work with these numbers just so you know the process of things.

    First, to make things easier, you can assume a 100 g sample.

    C = 41.7% --> 41.7 g
    H = 6.2 % --> 6.2 g
    N = 19.3% --> 19.3 g
    O = 33.1% -- > 33.1 g

    Second, convert all the grams to moles of their respective substance. In other words, divide by their atomic mass. (round to about 3-4 decimal places)

    C = (41.7 g) / (12.01 g/mol) = 3.472 mol
    H = (6.2 g) / (1.01 g/mol) = 6.139 mol
    N = (19.3 g) / (14.01 g/mol) = 1.378 mol
    O = (33.1 g) / (16.00 g/mol) = 2.069 mol

    Next, divide all the moles by the smallest number. In this case, divide everything by 1.378 (nitrogen).

    C = 3.472 / 1.378 = 2.5
    H = 6.139 / 1.378 = 4.5
    N = 1.378 / 1.378 = 1
    O = 2.069 / 1.378 = 1.5

    Since the numbers are generally in halves (a lot of .5's), we multiply everything by 2.

    C = 2.5 x 2 = 5
    H = 4.5 x 2 = 9
    N = 1 x 2 = 2
    O = 1.5 x 2 = 3

    Finally, put together the formula. Each number corresponds to the element's subscript.

    C5H9N2O3

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate the empirical formula of Tylenol: C, 63.56%; H, 6.00%; N, 9.27%; O, 21.17%

  2. Chemistry

    Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 3.279 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich

  3. chemistry

    Calculate the empirical formula for each of the following natural flavors based on their elemental mass percent composition. nitroglycerin (used medically as a vasodilator to treat heart conditions): C 15.87% H 2.22% N 18.50% O

  4. Chemistry

    I am completing my lab and cannot figure this out. I need someone to go over it and make sure I am right because I can't figure out why my empirical formula does not match the molecular formula. #7 is the one I am really having a

  1. Chemistry

    A certain compound containing only carbon and hydrogen was found to have a vapor density of 2.550 g/L at 100 degrees C and 760 mm Hg. If the empirical formula of this compound is CH, what is the molecular formula of this compound?

  2. Chemistry

    the formula H2O2 is an example of 1.molecular formula 2. an empirical formula 3.an ionic formula 4.an organic formula

  3. chemistry

    Calculate the empirical formula for compound ethyl butyrate (pineapple oil): C, 62.04%; H, 10.41%; O, 27.55% Can someone show me the steps?

  4. Chemistry

    2) What is the empirical formula of a compound containing C, H, O if combustion of 1.23g of the compound yields 1.8g CO2 and .74g of H2O 3) What are the empirical and molecular formulas of a hydrocarbon if combustion of 2.10g of

  1. chemistry- empirical formulas

    Calculate the empirical formula of a molecule with the following percent compositions: 55.0% gallium (Ga) and 45.0% fluorine (F). mass of 100g #of Moles in 100g of the compound Ga55.0% _____ ______ F45.0% ______ _______ c.

  2. Physical science

    1. Nicotine,a poisonous compound found in tobacco leaves,is 74% carbon,8,65% hydrogen and 17,35% nitrogen (a)calculate the empirical formula of nicotine (b)what is the molecular formula of nicotine if it has a molar mass of 165

  3. chemistry

    Water is added to 4.267 grams of UF6. The only products are 3.730 grams of a solid containing only uranium, oxygen and fluorine and 0.970 gram of gas. The gas is 95.0% flourine, and the remainder is hydrogen. From data determine

  4. AP Chemistry

    The structural formula for acetic acid is CH3CO2H. What is its empirical formula; what is its molecular formula?

You can view more similar questions or ask a new question.