chemistry

When 1.24g of an organic compound with the formula CxHyOz is burned in excess oxygen, 1.76g of carbon dioxide and 1.08g of water vapor are obtained. What is the empirical formula of the compound?



Determine the moles of CO2 in 1.76grams, that will give you the moles of C in the original compound.

Determine the moles of H2O in 1.08 grams, that will give you the moles of H2, double it, and you have the number of moles in the original compound.

Add the weight of the moles of C in the original compouond to the weight of moles of H in the orig compound, then subtract that weight from 1.24g. The remainder is the weight of O in the compound, now calculate the moles of O in that.

You have the moles of C, H, and O in the original compound.

Take the smaller of those three numbers, and divide into all three. The numbers you get will be the mole ratio.

For instance, assume you had these numbers....C .0024 moles, H .0050 moles, and O .0025 moles.

C is the lower number, dividing, we get
CH2O

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩

Respond to this Question

First Name

Your Response

Similar Questions

  1. CHEM

    A 0.4647-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in oxygen to yield 0.8635 g of CO2 and 0.1767 g of H2O. What is the empirical formula of the compound? i got C3H3O2 IS IT RIGHT?

  2. Chemistry

    A- 50.0 g of H2SO4 react with 75.0 g of NaOH. Identify the limiting and excess reactants. How many grams of Na2SO4 will be formed? B- A chemist burns 160.0 g of aluminum in 200.0 g of oxygen. She produces 275.0 g of aluminum

  3. Stoichiometry

    4. Vitamin C, M= 176.12 g/mol, is a compound of composed of carbon, hydrogen, and oxygen. Vitamin C is found in many natural sources especially citrus fruits. When a 1.000-g sample of vitamin C is burned in a combustion apparatus

  4. chemistry

    A sample of liquid consisting of only C,H and O and having a mass of 0.5438g was burned in pure oxygen and 1.039g of CO2 and 0.6369g H2O were obtained. what is the empirical formula of the compound?

  1. AP Chemistry

    a 5.15g sample of a hydrocarbon is burned in oxygen, producing 15.6g of carbon dioxide and 8.45g of water. Assuming an excess of oxygen, what is the empirical formula of the hydrocarbon?

  2. Chemistry

    An organic compound x contains 40% carbon, 6.7% hydrogen the third compound oxygen. If the relative molecular mass of the compound is 60, calculate (i) the empirical formular of x (ii) the molecular formular of x

  3. Chemistry

    When 1.5173g of an a organic iron compound contains Fe,C,HH and O was burned in oxygen 2.838g CO2 and 0.8122g H2O wereproduce.in a separate experiment to determine mass % of iron, 0.3355g of the compound yield 0.0758g Fe2O3.What

  4. Chemistry

    Consider the following reaction: CH4 +2O2 -> CO2 + 2H2O. Delta H = -891 kJ Calculate the enthalpy change for each of the following cases: a. 1.00 g methane is burned in excess oxygen b. 1.00 x 10^3 L methane gas at 740. torr and

  1. science

    Tristan is given the task of studying the compound CO2. Before he even begins his research, what information can Tristan obtain from the compound's chemical formula alone? Select all that apply. He can tell the compound contains

  2. chemistry

    1- A compound is 87.5% nitrogen and 12.5% hydrogen. The molecular weight of the compound is 32 g/mol. Describe the molecule referencing shape, and inter-molecular forces. 2- Gaseous butadiene, C4H6 , reacts with hydrogen gas in

  3. AS ORGANIC CHEM

    An organic compound, X, will react with an excess of calcium metal to produce a salt with the empirical formula CaC4H6O4. What could be the identity of X? 1 ethanoic acid 2 butanedioic acid 3 methylpropanedioic acid With

  4. Chemistry

    A 0.5438 g sample of a compound contains only C H and O was burned completely in oxygen.the products were 1.0390 g CO2 and 0.6369g H2O. Determine the empirical formula of thr compound

View more similar questions or ask a new question.